Properties of Solutions and Kinetics. Unit 8 Chapters 4.5, 13 and 14

Save this PDF as:
 WORD  PNG  TXT  JPG

Size: px
Start display at page:

Download "Properties of Solutions and Kinetics. Unit 8 Chapters 4.5, 13 and 14"

Transcription

1 Properties of Solutions and Kinetics Unit 8 Chapters 4.5, 13 and 14

2 Unit 8.1: Solutions Chapters 4.5,

3 Classification of Matter Solutions are homogeneous mixtures

4 Solute A solute is the dissolved substance in a solution. Salt in salt water Sugar in soda drinks Solvent Carbon dioxide in soda drinks A solvent is the dissolving medium in a solution. Water in salt water Water in soda

5 Heat of Solution The Heat of Solution is the amount of heat energy absorbed (endothermic) or released (exothermic) when a specific amount of solute dissolves in a solvent. Substance Heat of Solution (kj/mol) NaOH NH 4 NO KNO HCl

6 Steps in Solution Formation H 1 Expanding the solute Separating the solute into individual components (requires energy) H 2 Expanding the solvent Overcoming intermolecular forces of the solvent molecules (requires energy) H 3 Interaction of solute and solvent to form the solution (releases energy)

7 Like Dissolves Like Nonpolar solutes dissolve best in nonpolar solvents Fats Steroids Waxes Benzene Hexane Toluene Polar and ionic solutes dissolve best in polar solvents Inorganic Salts Sugars Water Small alcohols Acetic acid

8 Solubility Trends The solubility of MOST solids increases with temperature. The rate at which solids dissolve increases with increasing surface area of the solid, higher temperatures, and agitating. The solubility of gases decreases with increases in temperature. The solubility of gases increases with the pressure above the solution.

9 Therefore Solids tend to dissolve best when: o Heated o Stirred o Ground into small particles gases tend to dissolve best when: o The solution is cold o Pressure is high

10 Saturation of Solutions A solution that contains the maximum amount of solute that may be dissolved under existing conditions is saturated. (equilibrium is reached and additional solute will not dissolve) A solution that contains less solute than a saturated solution under existing conditions is unsaturated. A solution that contains more dissolved solute than a saturated solution under the same conditions is supersaturated.

11 Solubility Chart

12 Calculations of Solution Concentration Mole fraction the ratio of moles of solute to total moles of solution Mole fraction of A = χ A = n A n A + n B Mol fractions do not have a unit 1.00 mol of HCl in 8.00 mol of water X HCl = X H2O = 0.889

13 Calculations of Solution Concentration Parts per million (ppm) mass of solute x 10 6 mass of solution Parts per billion (ppb) mass of solute x 10 9 mass of solution

14 Calculations of Solution Concentration: Molarity is the ratio of moles of solute to liters of solution Molarity = M = moles of solute Liter of solution 5 M or 5 molar means 5 moles of solute are in 1 liter of solution

15

16 MOLARITY A measurement of the concentration of a solution Molarity (M) is equal to the moles of solute (n) per liter of solution M = n / V = mol / L Calculate the molarity of a solution prepared by mixing 1.5 g of NaCl in ml of solution First calculate the moles of solute: 1.5 g NaCl ( 1 mole NaCl ) = moles of NaCl g NaCl Next convert ml to L: L of solution Last, plug the appropriate values into the correct variables in the equation: M = n / V = moles / L = mol/l

17 MOLARITY M = n / V = mol / L How many grams of LiOH are needed to prepare ml of a 1.25 M solution? First calculate the moles of solute needed: M = n / V, now rearrange to solve for n: n = MV n = (1.25 mol / L ) ( L) = moles of solute needed Next calculate the molar mass of LiOH: g/mol Last, use diminsional analysis to solve for mass: moles (23.95 g LiOH / 1 mol LiOH) = 7.48 g of LiOH

18 Review of electrolytes Strong electrolytes: conduct electricity strongly in solution because there are a lot of ions (soluble ionic, strong acids) Weak electrolytes: conduct electricity weakly in solution because there are a few ions (insoluble ionic, weak acids Nonelectrolyes: Do not conduct electricity in solution because there are no ions (covalent compounds)

19 Concentrations of ions in solution For strong electrolytes K 2 SO 4 2K + + SO 4 2-2M K 2 SO 4 solution is 4M of potassium ions and 2M of sulfate ions

20 MOLARITY & DILUTION M 1 V 1 = M 2 V 2 The act of diluting a solution is to simply add more water (the solvent) thus leaving the amount of solute unchanged. Since the amount or moles of solute before dilution (n i ) and the moles of solute after the dilution (n f ) are the same: n i = n f And the moles for any solution can be calculated by n=mv A relationship can be established such that M i V i = n i = n f = M f V f Or simply : M i V i = M b V b

21 MOLARITY & Dilution Calculate the molarity of a solution prepared by diluting 25.0 ml of 0.05 M potassium iodide with 50.0 ml of water M 1 = 0.05 mol/l M 2 =? V 1 = 25.0 ml V 2 = = 75.0 ml M 1 V 1 = M 2 V 2 M 1 V 1 = M 2 = (0.05 mol/l) (25.0 ml) = M of KI V ml

22 MOLARITY & dilution Given a 6.00 M HCl solution, how would you prepare ml of M HCl? M 1 = 6.00 mol/l M 2 = V 1 =? ml V 2 = ml M 1 V 1 = M 2 V 2 M 2 V 2 = V 1 = (0.150 mol/l) (250.0 ml) = 6.25 ml of 6 M HCl 6.00 mol/l M 1 You would need 6.25 ml of the 6.00 M HCl reagent which would be added to about 100 ml of DI water in a ml graduated cylinder then more water would be added to the mixture until the bottom of the menicus is at ml. Mix well.

23 MOLARITY & Stoichiometry How many grams of calcium carbonate will be precipitated by adding 25.0 ml calcium chloride to 25.0 ml of 0.56 M potassium carbonate? CaCl 2 + K 2 CO 3 CaCO KCl V = 25.0 ml M = 0.56 mol/l m=? V = 25.0 ml First convert volume of A to moles of A: L K 2 CO 3 (0.56 mol/l) = moles of K 2 CO 3 Now convert moles of A to moles of B: mol K 2 CO 3 (1 mol CaCO 3 /1 mol K 2 CO 3 ) =0.014 mol CaCO 3 Next convert moles of B to grams of B:

24 0.028 mol KCl / L = 0.56 M of KCl MOLARITY & Stoichiometry What would be the molarity of the potassium chloride solution from the last problem? CaCl 2 + K 2 CO 3 CaCO KCl V = 25.0 ml M = 0.56 mol/l M =? V = 25.0 ml First convert volume of A to moles of A: L K 2 CO 3 (0.56 mol/l) = moles of K 2 CO 3 Now convert moles of A to moles of B: mol K 2 CO 3 (2 mol KCl /1 mol K 2 CO 3 ) =0.028 mol KCl Next convert moles of B to molarity of B:

25 Suspensions and Colloids Suspensions and colloids are NOT solutions. Suspensions: The particles are so large that they settle out of the solvent if not constantly stirred. Colloids: The particles intermediate in size between those of a suspension and those of a solution.

26 Types of Colloids Examples Dispersing Dispersed Colloid Type Medium Substance Fog, aerosol sprays Gas Liquid Aerosol Smoke, airborn germs Gas Solid Aerosol Whipped cream, soap suds Liquid Gas Foam Milk, mayonnaise Liquid Liquid Emulsion Paint, clays, gelatin Liquid Solid Sol Marshmallow, Styrofoam Solid Gas Solid Foam Butter, cheese Solid Liquid Solid Emulsion Ruby glass Solid Solid Solid sol

27 Colloids scatter light, making a beam visible. Solutions do not scatter light. The Tyndall Effect Which glass contains a colloid? colloid solution

28 Unit 8.2: Rates of reactions Chapter 14

29 Collision Model Key Idea: Molecules must collide to react. However, only a small fraction of collisions produces a reaction. Why?

30 Collision Model 1. Collisions must have sufficient energy to produce the reaction (must equal or exceed the activation energy). 2. Colliding particles must be correctly oriented to one another in order to produce a reaction.

31 Endothermic Reactions

32 Exothermic Reactions

33 Factors Affecting Rate Increasing temperature always increases the rate of a reaction. Particles collide more frequently Particles collide more energetically Increasing surface area (particle size) increases the rate of a reaction Increasing Concentration (pressure for gases) USUALLY increases the rate of a reaction Presence of Catalysts, which lower the activation energy by providing alternate pathways

34 Catalysis Catalyst: A substance that speeds up a reaction without being consumed Enzyme: A large molecule (usually a protein) that catalyzes biological reactions. Homogeneous catalyst: Present in the same phase as the reacting molecules. Heterogeneous catalyst: Present in a different phase than the reacting molecules.

35 Lowering of Activation Energy by a Catalyst

36 The Arrhenius Equation k = Ae E / RT a k = rate constant at temperature T A = frequency factor E a = activation energy R = Gas constant, J/K mol

37 Reaction Rate The change in concentration of a reactant or product per unit of time Rate = [ A] at timet [ A] at timet t t Rate [ A] = t

38 A B 1 mole 0 mol 20 min mol 0.46 mol 40 min. 0.3 mol 0.7 mol A negative rate just means it s the reactant disappearing and a positive rate means it s the product appearing

39 2 HI H 2 + I 2 What is the rate of appearance of hydrogen if the rate of disappearance of HI is 6.0 x M/s? Answer: 3.0 x M/s -1/2 rate HI = rate H 2 = rate I 2

40 Reaction Rates: 2NO 2 (g) 2NO(g) + O 2 (g) 1. Can measure disappearance of reactants 2. Can measure appearance of products 3. Are proportional stoichiometrically

41 Reaction Rates: 2NO 2 (g) 2NO(g) + O 2 (g) 4. Are equal to the slope tangent to that point [NO 2 ] t 5. Change as the reaction proceeds, if the rate is dependent upon concentration [ NO2 ] t constant

42 Unit 8.3: Rate Laws Chapter 14

43 Rate Laws Differential rate laws express (reveal) the relationship between the concentration of reactants and the rate of the reaction. The differential rate law is usually just called the rate law. Integrated rate laws express (reveal) the relationship between concentration of reactants and time

44 Writing a (differential) Rate Law Problem - Write the rate law, determine the value of the rate constant, k, and the overall order for the following reaction: Experiment 2 NO(g) + Cl 2 (g) 2 NOCl(g) [NO] (mol/l) [Cl 2 ] (mol/l) Rate Mol/L s x x x x 10-6

45 Writing a Rate Law Part 1 Determine the values for the exponents in the rate law: R = k[no] x [Cl 2 ] y Experiment [NO] (mol/l) [Cl 2 ] (mol/l) Rate Mol/L s x x x x 10-5 In experiment 1 and 2, [Cl 2 ] is constant while [NO] doubles. The rate quadruples, so the reaction is second order with respect to [NO] R = k[no] 2 [Cl 2 ] y

46 Writing a Rate Law Part 1 Determine the values for the exponents in the rate law: Experiment R = k[no] 2 [Cl 2 ] y [NO] (mol/l) [Cl 2 ] (mol/l) Rate Mol/L s x x x x 10-5 In experiment 2 and 4, [NO] is constant while [Cl 2 ] doubles. The rate doubles, so the reaction is first order with respect to [Cl 2 ] R = k[no] 2 [Cl 2 ]

47 Writing a Rate Law Part 2 Determine the value for k, the rate constant, by using any set of experimental data: R = k[no] 2 [Cl 2 ] Experiment [NO] [Cl 2 ] Rate (mol/l) (mol/l) Mol/L s x x10 k mol mol mol = L s L L k x 10 mol L x10 L = 3 3 = L s mol mol s

48 Writing a Rate Law Part 3 Determine the overall order for the reaction. R = k[no] 2 [Cl 2 ] = 3 The reaction is 3 rd order Overall order is the sum of the exponents, or orders, of the reactants Most reactions go faster with increasing temperatures. In the rate law equation, k is higher at higher temperatures.

49 Determining Order with Concentration vs. Time data (the Integrated Rate Law) Zero Order: First Order: timevs. concentrationislinear timevs.ln( concentration) islinear Second Order: timevs. 1 concentration islinear

50 Solving an Integrated Rate Law Time (s) [H 2 O 2 ] (mol/l) Problem: Find the integrated rate law and the value for the rate constant, k A graphing calculator with linear regression analysis greatly simplifies this process!!

51 Time vs. ln[h 2 O 2 ] Time (s) ln[h 2 O 2 ]

52 Time vs. [H 2 O 2 ] Time (s) [H 2 O 2 ]

53 Time vs. 1/[H 2 O 2 ] Time (s) 1/[H 2 O 2 ]

54 And the winner is Time vs. ln[h 2 O 2 ] 1. As a result, the reaction is 1 st order 2. The (differential) rate law is: R = kho [ ] The integrated rate law is: ln[ HO] = kt+ ln[ HO] But what is the rate constant, k?

55 Finding the Rate Constant, k Method #1: Calculate the slope from the Time vs. ln[h 2 O 2 ] table. slope ln[ HO] t 3600 s 2 2 = = slope = 8.32 x10 s Now remember: ln[ HO] = kt+ ln[ HO] k = -slope 4 1 k = 8.32 x 10-4 s -1 Time (s) ln[h 2 O 2 ]

56 Rate Laws Summary Zero Order First Order Second Order Rate Law Rate = k Rate = k[a] Rate = k[a] 2 Integrated Rate Law [A] = -kt + [A] 0 ln[a] = -kt + ln[a] = kt + [ A] [ A] 0 Plot the produces a straight line Relationship of rate constant to slope of straight line [A] versus t ln[a] versus t 1 [ A] versus t Slope = -k Slope = -k Slope = k Half-Life t 1/2 [ A] 0 = t1/2 2k k = 1/2 t 1 = ka [ ] 0

57 Unit 8.4: Kinetics Chapter 14

58 Class starter Dinitrogen pentoxide gas decomposes according to the equation: N 2 O 5 4NO 2 + O 2. This first-order reaction was allowed to proceed at 40 ᴼC and the data was collected. [N2O5] time (min) a. Calculate the rate constant using the values for concentration and time given in the table. Include units. b. After how many minutes will [N 2 O 5 ] be equal to M? c. What will be the concentration of N 2 O 5 after 100 minutes have elapsed? d. Calculate the initial rate of the reaction. Include units with your answer. e. What is the half life of the reaction?

59 Reaction Mechanism The reaction mechanism is the series of elementary steps by which a chemical reaction occurs. The sum of the elementary steps must give the overall balanced equation for the reaction The mechanism must agree with the experimentally determined rate law

60 NO 2 + CO NO + CO 2 Mechanism 1. NO 2 + NO 2 NO 3 + NO 2. NO 3 + CO NO 2 + CO 2 The two steps add up to give the overall rxn. NO 3 is not a reactant or a product in the overall rxn. It was produced and then consumed. NO 3 is the intermediate step.

61 Rate-Determining Step In a multi-step reaction, the slowest step is the rate-determining step. It therefore determines the rate of the reaction. The experimental rate law must agree with the rate-determining step

62 Determining the rate law from the NO 2 + CO NO + CO 2 Mechanism: mechanism 1. NO 2 + NO 2 NO 3 + NO (slow) 2. NO 3 + CO NO 2 + CO 2 (fast) Rate law is determined from the slow step Rate = k [NO 2 ] 2 The intermediate cannot be in the rate law

63 Another example 2 NO + Br 2 2 NOBr Mechanism 1. NO + Br 2 NOBr 2 (fast equilibrium) 2. NOBr 2 + NO 2NOBr (slow) Rate = k [NOBr 2 ][NO] This is a problem because NOBr 2 is an intermediate and cannot be in the rate law, but because the first step is a fast equilibrium we can replace NOBr 2 with NO and Br 2 so Rate = k [NO][Br 2 ][NO] or Rate = k [Br 2 ][NO] 2

64 Identifying Intermediates For the reaction: 2H 2 (g) + 2NO(g) N 2 (g) + 2H 2 O(g) Which species in the reaction mechanism are intermediates? Step #1 Step #2 H 2 (g) + 2NO(g) N 2 O(g) + H 2 O(g) N 2 O(g) + H 2 (g) N 2 (g) + H 2 O(g) 2H 2 (g) + 2NO(g) N 2 (g) + 2H 2 O(g) N 2 O(g) is an intermediate

65 Identifying the Rate-Determining Step For the reaction: 2H 2 (g) + 2NO(g) N 2 (g) + 2H 2 O(g) The experimental rate law is: R = k[no] 2 [H 2 ] Which step in the reaction mechanism is the ratedetermining (slowest) step? Step #1 Step #2 H 2 (g) + 2NO(g) N 2 O(g) + H 2 O(g) N 2 O(g) + H 2 (g) N 2 (g) + H 2 O(g) Step #1 agrees with the experimental rate law

Solvents. Solvents at the hardware store

Solvents. Solvents at the hardware store Solution Chemistry Parts of a Solution Review Solute A solute is the dissolved substance in a solution. Salt in salt water Sugar in soda drinks Solvent Carbon dioxide in soda drinks A solvent is the dissolving

More information

MIXTURES AND DISSOLVING. CE/Honors Chemistry Unit 10

MIXTURES AND DISSOLVING. CE/Honors Chemistry Unit 10 MIXTURES AND DISSOLVING CE/Honors Chemistry Unit 10 TYPES OF MIXTURES Solution: homogeneous mixture of two or more substances in a single phase Two parts: solvent (greater amt) and solute Does not separate

More information

Chapter 12. Preview. Objectives Solutions Suspensions Colloids Solutes: Electrolytes Versus Nonelectrolytes

Chapter 12. Preview. Objectives Solutions Suspensions Colloids Solutes: Electrolytes Versus Nonelectrolytes Preview Objectives Solutions Suspensions Colloids Solutes: Electrolytes Versus Nonelectrolytes Section 1 Types of Mixtures Objectives Distinguish between electrolytes and nonelectrolytes. List three different

More information

Chapter 12. Preview. Objectives Solutions Suspensions Colloids Solutes: Electrolytes Versus Nonelectrolytes

Chapter 12. Preview. Objectives Solutions Suspensions Colloids Solutes: Electrolytes Versus Nonelectrolytes Preview Objectives Solutions Suspensions Colloids Solutes: Electrolytes Versus Nonelectrolytes Section 1 Types of Mixtures Objectives Distinguish between electrolytes and nonelectrolytes. List three different

More information

H 2 O WHAT PROPERTIES OF WATER MAKE IT ESSENTIAL TO LIFE OF EARTH? Good solvent High Surface tension Low vapor pressure High boiling point

H 2 O WHAT PROPERTIES OF WATER MAKE IT ESSENTIAL TO LIFE OF EARTH? Good solvent High Surface tension Low vapor pressure High boiling point Unit 9: Solutions H 2 O WHAT PROPERTIES OF WATER MAKE IT ESSENTIAL TO LIFE OF EARTH? Good solvent High Surface tension Low vapor pressure High boiling point Water is a polar molecule. It experiences hydrogen

More information

AP CHEMISTRY CHAPTER 12 KINETICS

AP CHEMISTRY CHAPTER 12 KINETICS AP CHEMISTRY CHAPTER 12 KINETICS Thermodynamics tells us if a reaction can occur. Kinetics tells us how quickly the reaction occurs. Some reactions that are thermodynamically feasible are kinetically so

More information

SOLUTIONS. Heterogeneous Mixtures. Section 8.1: Solutions and Other Mixtures. Heterogeneous Mixtures (cont d) CHAPTER 8.

SOLUTIONS. Heterogeneous Mixtures. Section 8.1: Solutions and Other Mixtures. Heterogeneous Mixtures (cont d) CHAPTER 8. Section 8.1: Solutions and Other Mixtures CHAPTER 8 SOLUTIONS Key Questions What is a heterogeneous mixture? What is a homogeneous mixture? Heterogeneous Mixtures The tree of matter branches into two distinct

More information

Chapter 12. Chemical Kinetics

Chapter 12. Chemical Kinetics Chapter 12 Chemical Kinetics Chapter 12 Table of Contents 12.1 Reaction Rates 12.2 Rate Laws: An Introduction 12.3 Determining the Form of the Rate Law 12.4 The Integrated Rate Law 12.5 Reaction Mechanisms

More information

CHAPTER 7: Solutions & Colloids 7.2 SOLUBILITY. Degrees of Solution. Page PHYSICAL STATES of SOLUTIONS SOLUTION

CHAPTER 7: Solutions & Colloids 7.2 SOLUBILITY. Degrees of Solution. Page PHYSICAL STATES of SOLUTIONS SOLUTION CHAPTER 7: Solutions & Colloids Predict the relative solubility of materials on the basis of polarity Describe solution formation in terms of solutesolvent interactions Calculate solution concentrations

More information

Warm UP. between carbonate and lithium. following elements have? 3) Name these compounds: 1) Write the neutral compound that forms

Warm UP. between carbonate and lithium. following elements have? 3) Name these compounds: 1) Write the neutral compound that forms Warm UP 1) Write the neutral compound that forms between carbonate and lithium 2) How many valence electrons do the following elements have? a) Chlorine b) Neon c) Potassium 3) Name these compounds: a)

More information

Chemistry Grade : 11 Term-3/Final Exam Revision Sheet

Chemistry Grade : 11 Term-3/Final Exam Revision Sheet Chemistry Grade : 11 Term-3/Final Exam Revision Sheet Exam Date: Tuesday 12/6/2018 CCS:Chem.6a,6b,6c,6d,6e,6f,7a,7b,7d,7c,7e,7f,1g Chapter(12):Solutions Sections:1,2,3 Textbook pages 378 to 408 Chapter(16):Reaction

More information

Today is Thursday, May 31 st, 2018

Today is Thursday, May 31 st, 2018 In This Lesson: Unit 6: Solutions Solutions and Solubility (Lesson 1 of 4) Today is Thursday, May 31 st, 2018 Stuff You Need: Calculator Periodic Table Polyatomic Ion List Pre-Class: Where have you seen

More information

SOLUTIONS CHAPTER 13

SOLUTIONS CHAPTER 13 SOLUTIONS CHAPTER 13 SOLUTIONS Solutions, also known as homogeneous mixtures, are composed of two components: solute and solvent. In a sugar-water solution, water acts as a solvent (dissolving medium);

More information

CHAPTER 12 REVIEW. Solutions. Answer the following questions in the space provided. b. sea water. c. water-absorbing super gels

CHAPTER 12 REVIEW. Solutions. Answer the following questions in the space provided. b. sea water. c. water-absorbing super gels CHAPTER 12 REVIEW Solutions SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Match the type of mixture on the left to its representative particle diameter on the right. c

More information

CP Chapter 15/16 Solutions What Are Solutions?

CP Chapter 15/16 Solutions What Are Solutions? CP Chapter 15/16 Solutions What Are Solutions? What is a solution? A solution is uniform that may contain solids, liquids, or gases. Known as a mixture Solution = + o Solvent The substance in abundance

More information

CHAPTER 13 (MOORE) CHEMICAL KINETICS: RATES AND MECHANISMS OF CHEMICAL REACTIONS

CHAPTER 13 (MOORE) CHEMICAL KINETICS: RATES AND MECHANISMS OF CHEMICAL REACTIONS CHAPTER 13 (MOORE) CHEMICAL KINETICS: RATES AND MECHANISMS OF CHEMICAL REACTIONS This chapter deals with reaction rates, or how fast chemical reactions occur. Reaction rates vary greatly some are very

More information

Chapter 12. Chemical Kinetics

Chapter 12. Chemical Kinetics Chapter 12 Chemical Kinetics Section 12.1 Reaction Rates Reaction Rate Change in concentration of a reactant or product per unit time. Rate = concentration of A at time t t 2 1 2 1 concentration of A at

More information

Solutions. Why does a raw egg swell or shrink when placed in different solutions?

Solutions. Why does a raw egg swell or shrink when placed in different solutions? Solutions 1 Why does a raw egg swell or shrink when placed in different solutions? Classification of Matter 2 Some Definitions 3 If a compound is soluble it is capable of being dissolved. A solution is

More information

Solvent does the dissolving (acetone) Solute the substance being dissolved (Styrofoam ) Soluble able to be dissolved

Solvent does the dissolving (acetone) Solute the substance being dissolved (Styrofoam ) Soluble able to be dissolved Solvent does the dissolving (acetone) Solute the substance being dissolved (Styrofoam ) Soluble able to be dissolved Like dissolves Like Ionic & polar compounds dissolve each other. Nonpolar dissolves

More information

Kinetics - Chapter 14. reactions are reactions that will happen - but we can t tell how fast. - the steps by which a reaction takes place.

Kinetics - Chapter 14. reactions are reactions that will happen - but we can t tell how fast. - the steps by which a reaction takes place. The study of. Kinetics - Chapter 14 reactions are reactions that will happen - but we can t tell how fast. - the steps by which a reaction takes place. Factors that Affect Rx Rates 1. The more readily

More information

Chapter 13 - Solutions

Chapter 13 - Solutions Chapter 13 - Solutions 13-1 Types of Mixtures Solutions A. Soluble 1. Capable of being dissolved B. Solution 1. A homogeneous mixture of two or more substances in a single phase C. Solvent 1. The dissolving

More information

Chapter 12. Chemical Kinetics

Chapter 12. Chemical Kinetics Chapter 12 Chemical Kinetics Section 12.1 Reaction Rates Section 12.1 Reaction Rates Section 12.1 Reaction Rates Section 12.1 Reaction Rates Section 12.1 Reaction Rates Section 12.1 Reaction Rates Section

More information

Aqueous Solutions (When water is the solvent)

Aqueous Solutions (When water is the solvent) Aqueous Solutions (When water is the solvent) Solvent= the dissolving medium (what the particles are put in ) Solute= dissolved portion (what we put in the solvent to make a solution) Because water is

More information

Brass, a solid solution of Zn and Cu, is used to make musical instruments and many other objects.

Brass, a solid solution of Zn and Cu, is used to make musical instruments and many other objects. Brass, a solid solution of Zn and Cu, is used to make musical instruments and many other objects. 14.1 General Properties of Solutions 14.2 Solubility 14.3 Rate of Dissolving Solids 14.4 Concentration

More information

Settling? Filterable? Tyndall Effect? * 1 N N Y nm

Settling? Filterable? Tyndall Effect? * 1 N N Y nm Types of Mixtures Notes *What is the Tyndall Effect? When a light shines through a mixture, the beams of light scatter. Homogeneous or Heterogeneous # of visible phases Settling? Filterable? Tyndall Effect?

More information

Name: Period: Date: solution

Name: Period: Date: solution Name: Period: Date: ID: A Solutions Test A Matching Use the choices below to answer the following 5 questions. a. Hydrogen bond d. Electrolyte b. Polar molecule e. Nonelectrolyte c. Nonpolar molecule 1.

More information

Part A Answer all questions in this part.

Part A Answer all questions in this part. Part A Directions (1-24): For each statement or question, record on your separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question.

More information

How can homogeneous and heterogeneous mixtures be. 1. classified? 2. separated?

How can homogeneous and heterogeneous mixtures be. 1. classified? 2. separated? How can homogeneous and heterogeneous mixtures be 1. classified? 2. separated? 1. HETEROGENEOUS MIXTURE 2. COLLOID 3. EMULSION 4. SUSPENSION 5. FILTRATION 6. TYNDALL EFFECT 7. HOMOGENEOUS MIXTURE 8. SOLUTION

More information

Solutions. LiCl (s) + H2O (l) LiCl (aq) 3/12/2013. Definitions. Aqueous Solution. Solutions. How Does a Solution Form? Solute Solvent solution

Solutions. LiCl (s) + H2O (l) LiCl (aq) 3/12/2013. Definitions. Aqueous Solution. Solutions. How Does a Solution Form? Solute Solvent solution Solutions Definitions A solution is a homogeneous mixture A solute is dissolved in a solvent. solute is the substance being dissolved solvent is the liquid in which the solute is dissolved an aqueous solution

More information

Ch 13 Rates of Reaction (Chemical Kinetics)

Ch 13 Rates of Reaction (Chemical Kinetics) Ch 13 Rates of Reaction (Chemical Kinetics) Reaction Rates and Kinetics - The reaction rate is how fast reactants are converted to products. - Chemical kinetics is the study of reaction rates. Kinetics

More information

Explain freezing-point depression and boiling-point elevation at the molecular level.

Explain freezing-point depression and boiling-point elevation at the molecular level. Solutions 1 UNIT4: SOLUTIONS All important vocabulary is in Italics and bold. Describe and give examples of various types of solutions. Include: suspension, emulsion, colloid, alloy, solute, solvent, soluble,

More information

Solution. Types of Solutions. Concentration and Solution Stoichiometry

Solution. Types of Solutions. Concentration and Solution Stoichiometry Concentration and Solution Stoichiometry Solution homogenous mixture of 2 or more pure substances only one perceptible phase species do not react chemically Types of Solutions solid liquid gas Solutions

More information

How fast reactants turn into products. Usually measured in Molarity per second units. Kinetics

How fast reactants turn into products. Usually measured in Molarity per second units. Kinetics How fast reactants turn into products. Usually measured in Molarity per second units. Kinetics Reaction rated are fractions of a second for fireworks to explode. Reaction Rates takes years for a metal

More information

Chapter 11 Properties of Solutions

Chapter 11 Properties of Solutions Chapter 11 Properties of Solutions 11.1 Solution Composition. Molarity moles solute 1. Molarity ( M ) = liters of solution B. Mass Percent mass of solute 1. Mass percent = 1 mass of solution C. Mole Fraction

More information

Chapter 14 Chemical Kinetics

Chapter 14 Chemical Kinetics Chapter 14 Chemical Kinetics Factors that Affect Reaction rates Reaction Rates Concentration and Rate The Change of Concentration with Time Temperature and Rate Reactions Mechanisms Catalysis Chemical

More information

Lecture (3) 1. Reaction Rates. 2 NO 2 (g) 2 NO(g) + O 2 (g) Summary:

Lecture (3) 1. Reaction Rates. 2 NO 2 (g) 2 NO(g) + O 2 (g) Summary: Summary: Lecture (3) The expressions of rate of reaction and types of rates; Stoichiometric relationships between the rates of appearance or disappearance of components in a given reaction; Determination

More information

Solutions and Solubility. BHS Chemistry

Solutions and Solubility. BHS Chemistry Solutions and Solubility BHS Chemistry MATTER Yes Can it be separated by physical means? No MIXTURES Pure SUBSTANCES Yes Is the composition uniform? Can it be decomposed by regular chemical means? No Yes

More information

Modern Chemistry Chapter 12- Solutions

Modern Chemistry Chapter 12- Solutions Modern Chemistry Chapter 12- Solutions Section 1- Types of Mixtures Solutions are homogeneous mixtures of two or more substances in a single phase. Soluble describes a substance as capable of being dissolved.

More information

Chemistry I 2nd Semester Exam Study Guide

Chemistry I 2nd Semester Exam Study Guide Chemistry I 2nd Semester Exam Study Guide Study the following topics and be able to apply these concepts to answer related questions to best prepare for the Chemistry exam. You should be able to: 1. Identify

More information

concentrations (molarity) rate constant, (k), depends on size, speed, kind of molecule, temperature, etc.

concentrations (molarity) rate constant, (k), depends on size, speed, kind of molecule, temperature, etc. #73 Notes Unit 9: Kinetics and Equilibrium Ch. Kinetics and Equilibriums I. Reaction Rates NO 2(g) + CO (g) NO (g) + CO 2(g) Rate is defined in terms of the rate of disappearance of one of the reactants,

More information

FINAL EXAM REVIEW I will provide all of the same sheets I provided on the quizzes this semester.

FINAL EXAM REVIEW I will provide all of the same sheets I provided on the quizzes this semester. Name: Class: Date: FINAL EXAM REVIEW I will provide all of the same sheets I provided on the quizzes this semester. True/False Indicate whether the statement is true or false. 1) Colligative properties

More information

AP Chem Chapter 14 Study Questions

AP Chem Chapter 14 Study Questions Class: Date: AP Chem Chapter 14 Study Questions 1. A burning splint will burn more vigorously in pure oxygen than in air because a. oxygen is a reactant in combustion and concentration of oxygen is higher

More information

Solutions. Solutions. How Does a Solution Form? Solutions. Energy Changes in Solution. How Does a Solution Form

Solutions. Solutions. How Does a Solution Form? Solutions. Energy Changes in Solution. How Does a Solution Form Ummm Solutions Solutions Solutions are homogeneous mixtures of two or more pure substances. In a solution, the solute is dispersed uniformly throughout the solvent. Solutions The intermolecular forces

More information

Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question.

Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. Assessment Chapter Test A Chapter: Solutions In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. Agitation prevents settling

More information

Name AP CHEM / / Chapter 12 Outline Chemical Kinetics

Name AP CHEM / / Chapter 12 Outline Chemical Kinetics Name AP CHEM / / Chapter 12 Outline Chemical Kinetics The area of chemistry that deals with the rate at which reactions occur is called chemical kinetics. One of the goals of chemical kinetics is to understand

More information

CHEMISTRY. Chapter 14 Chemical Kinetics

CHEMISTRY. Chapter 14 Chemical Kinetics CHEMISTRY The Central Science 8 th Edition Chapter 14 Kozet YAPSAKLI kinetics is the study of how rapidly chemical reactions occur. rate at which a chemical process occurs. Reaction rates depends on The

More information

Mixtures. Chapters 12/13: Solutions and Colligative Properties. Types of Solutions. Suspensions. The Tyndall Effect: Colloid

Mixtures. Chapters 12/13: Solutions and Colligative Properties. Types of Solutions. Suspensions. The Tyndall Effect: Colloid Mixtures Chapters 12/13: Solutions and Colligative Properties Solution - a homogeneous mixture of two or more substances in a single phase Soluble - capable of being dissolved Solutions - 2 Parts Solvent

More information

Name Date. 9. Which substance shows the least change in solubility (grams of solute) from 0 C to 100 C?

Name Date. 9. Which substance shows the least change in solubility (grams of solute) from 0 C to 100 C? Solubility Curve Practice Problems Directions: Use the graph to answer the questions below. Assume you will be using 100g of water unless otherwise stated. 1. How many grams of potassium chloride (KCl)

More information

Chemical Kinetics. Kinetics is the study of how fast chemical reactions occur. There are 4 important factors which affect rates of reactions:

Chemical Kinetics. Kinetics is the study of how fast chemical reactions occur. There are 4 important factors which affect rates of reactions: Chemical Kinetics Kinetics is the study of how fast chemical reactions occur. There are 4 important factors which affect rates of reactions: reactant concentration temperature action of catalysts surface

More information

Chapter 14. Chemical Kinetics

Chapter 14. Chemical Kinetics Chapter 14. Chemical Kinetics Common Student Misconceptions It is possible for mathematics to get in the way of some students understanding of the chemistry of this chapter. Students often assume that

More information

Chapter 13 Kinetics: Rates and Mechanisms of Chemical Reactions

Chapter 13 Kinetics: Rates and Mechanisms of Chemical Reactions Chapter 13 Kinetics: Rates and Mechanisms of Chemical Reactions 14.1 Focusing on Reaction Rate 14.2 Expressing the Reaction Rate 14.3 The Rate Law and Its Components 14.4 Integrated Rate Laws: Concentration

More information

Chapter 14 Chemical Kinetics

Chapter 14 Chemical Kinetics Chapter 14 Chemical Kinetics Factors that Affect Reaction rates Reaction Rates Concentration and Rate The Change of Concentration with Time Temperature and Rate Reactions Mechanisms Catalysis Chemical

More information

Solutions: Multiple Choice Review PSI AP Chemistry. 1. Which of the following would be FALSE regarding mixtures?

Solutions: Multiple Choice Review PSI AP Chemistry. 1. Which of the following would be FALSE regarding mixtures? Solutions: Multiple Choice Review PSI AP Chemistry Name Part A: Mixtures, Solubility, and Concentration 1. Which of the following would be FALSE regarding mixtures? (A) Mixtures do not obey the law of

More information

General Chemistry I Concepts

General Chemistry I Concepts Chemical Kinetics Chemical Kinetics The Rate of a Reaction (14.1) The Rate Law (14.2) Relation Between Reactant Concentration and Time (14.3) Activation Energy and Temperature Dependence of Rate Constants

More information

UNIT 12 Solutions. Homework. CRHS Academic Chemistry. Due Date Assignment On-Time (100) Late (70) Warm-Up

UNIT 12 Solutions. Homework. CRHS Academic Chemistry. Due Date Assignment On-Time (100) Late (70) Warm-Up Name Period CRHS Academic Chemistry UNIT 12 Solutions Homework Due Date Assignment On-Time (100) Late (70) 12.1 12.2 12.3 12.4 Warm-Up EC Notes, Homework, Exam Reviews and Their KEYS located on CRHS Academic

More information

Section 6.2A Intermolecular Attractions

Section 6.2A Intermolecular Attractions Section 6.2A Intermolecular Attractions As we know, molecules are held together by covalent bonds, but there are also attractive forces BETWEEN individual molecules (rather than within). These are called

More information

Solutions and other Mixtures. Ch 20.1

Solutions and other Mixtures. Ch 20.1 Solutions and other Mixtures Ch 20.1 Mixture A A combination of more than one pure substances physically combined. Two Types: Homogeneous Same throughout Heterogeneous Different throughout Homogeneous

More information

Chapter 7 Solutions and Colloids

Chapter 7 Solutions and Colloids Chapter 7 Solutions and Colloids 7.1 Physical States of Solutions Solutions are homogeneous mixtures of two or more substances in which the components are present as atoms, molecules, or ions. Properties

More information

Chapter 7 Solutions and Colloids

Chapter 7 Solutions and Colloids Chapter 7 Solutions and Colloids 7.1 Physical States of Solutions Solutions are homogeneous mixtures of two or more substances in which the components are present as atoms, molecules, or ions. Properties

More information

Basic Concepts of Chemistry Notes for Students [Chapter 12, page 1] D J Weinkauff - Nerinx Hall High School. Chapter 12 Properties of Solutions

Basic Concepts of Chemistry Notes for Students [Chapter 12, page 1] D J Weinkauff - Nerinx Hall High School. Chapter 12 Properties of Solutions Basic Concepts of Chemistry Notes for Students [Chapter 12, page 1] Chapter 12 Properties of Solutions Section 12 1: The Nature of Aqueous Solutions 1) Sec 12 1.1 Mixtures of Two Liquids When two liquids

More information

Name: Regents Chemistry: Dr. Shanzer. Practice Packet. Chapter 11: Solutions

Name: Regents Chemistry: Dr. Shanzer. Practice Packet. Chapter 11: Solutions Name: Regents Chemistry: Dr. Shanzer Practice Packet Chapter 11: Solutions What are Solutions? Objective: How do we recognize the parts of a solution, its characteristics and the difference between dissolving

More information

Chemistry 102 Chapter 14 CHEMICAL KINETICS. The study of the Rates of Chemical Reactions: how fast do chemical reactions proceed to form products

Chemistry 102 Chapter 14 CHEMICAL KINETICS. The study of the Rates of Chemical Reactions: how fast do chemical reactions proceed to form products CHEMICAL KINETICS Chemical Kinetics: The study of the Rates of Chemical Reactions: how fast do chemical reactions proceed to form products The study of Reaction Mechanisms: the steps involved in the change

More information

Chapter 30. Chemical Kinetics. Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved.

Chapter 30. Chemical Kinetics. Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved. Chapter 30 Chemical Kinetics 1 Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved. Chemists have three fundamental questions in mind when they study chemical reactions: 1.) What happens?

More information

Solutions. Experiment 11. Various Types of Solutions. Solution: A homogenous mixture consisting of ions or molecules

Solutions. Experiment 11. Various Types of Solutions. Solution: A homogenous mixture consisting of ions or molecules Solutions Solution: A homogenous mixture consisting of ions or molecules -Assignment: Ch 15 Questions & Problems : 5, (15b,d), (17a, c), 19, 21, 23, 27, (33b,c), 39, (43c,d),45b, 47, (49b,d), (55a,b),

More information

10) On a solubility curve, the points on the curve indicate a solution. 11) Values on the graph a curve represent unsaturated solutions.

10) On a solubility curve, the points on the curve indicate a solution. 11) Values on the graph a curve represent unsaturated solutions. Unit 11 Solutions- Funsheets Part A: Solubility Curves- Answer the following questions using the solubility curve below. Include units! 1) What mass of each solute will dissolve in 100mL of water at the

More information

AP CHEMISTRY NOTES 7-1 KINETICS AND RATE LAW AN INTRODUCTION

AP CHEMISTRY NOTES 7-1 KINETICS AND RATE LAW AN INTRODUCTION AP CHEMISTRY NOTES 7-1 KINETICS AND RATE LAW AN INTRODUCTION CHEMICAL KINETICS the study of rates of chemical reactions and the mechanisms by which they occur FACTORS WHICH AFFECT REACTION RATES 1. Nature

More information

CHEM Chapter 14. Chemical Kinetics (Homework) Ky40

CHEM Chapter 14. Chemical Kinetics (Homework) Ky40 CHEM 1412. Chapter 14. Chemical Kinetics (Homework) Ky40 1. Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2ClO 2 (aq) + 2OH (aq) ClO

More information

Name Chemistry Pre-AP. Notes: Solutions

Name Chemistry Pre-AP. Notes: Solutions Name Chemistry Pre-AP Notes: Solutions Period I. Intermolecular Forces (IMFs) A. Attractions Between Molecules Attractions between molecules are called and are very important in determining the properties

More information

Classification of Solutions. Classification of Solutions. Aqueous Solution Solution in which H2O is the solvent

Classification of Solutions. Classification of Solutions. Aqueous Solution Solution in which H2O is the solvent SOLUTIONS Solution Homogeneous mixture in which one substance is dissolved in another SOLUTE: substance that is dissolved SOLVENT: substance doing the dissolving INSOLUBLE: does NOT dissolve SOLUBLE: does

More information

Honors Chemistry Unit 4 Exam Study Guide Solutions, Equilibrium & Reaction Rates

Honors Chemistry Unit 4 Exam Study Guide Solutions, Equilibrium & Reaction Rates Honors Chemistry Unit 4 Exam Study Guide Solutions, Equilibrium & Reaction Rates Define the following vocabulary terms. Solute Solvent Solution Molarity Molality Colligative property Electrolyte Non-electrolyte

More information

CHAPTER 12 CHEMICAL KINETICS

CHAPTER 12 CHEMICAL KINETICS 5/9/202 CHAPTER 2 CHEMICAL KINETICS CHM52 GCC Kinetics Some chemical reactions occur almost instantaneously, while others are very slow. Chemical Kinetics - study of factors that affect how fast a reaction

More information

Unit 10 Solution Chemistry 1. Solutions & Molarity 2. Dissolving 3. Dilution 4. Calculation Ion Concentrations in Solution 5. Precipitation 6.

Unit 10 Solution Chemistry 1. Solutions & Molarity 2. Dissolving 3. Dilution 4. Calculation Ion Concentrations in Solution 5. Precipitation 6. Unit 10 Solution Chemistry 1. Solutions & Molarity 2. Dissolving 3. Dilution 4. Calculation Ion Concentrations in Solution 5. Precipitation 6. Formula, Complete, Net Ionic Equations 7. Qualitative Analysis

More information

A solution is a homogeneous mixture of two or more substances.

A solution is a homogeneous mixture of two or more substances. UNIT (5) SOLUTIONS A solution is a homogeneous mixture of two or more substances. 5.1 Terminology Solute and Solvent A simple solution has two components, a solute, and a solvent. The substance in smaller

More information

Lecture Presentation. Chapter 14. James F. Kirby Quinnipiac University Hamden, CT. Chemical Kinetics Pearson Education, Inc.

Lecture Presentation. Chapter 14. James F. Kirby Quinnipiac University Hamden, CT. Chemical Kinetics Pearson Education, Inc. Lecture Presentation Chapter 14 James F. Kirby Quinnipiac University Hamden, CT In chemical kinetics we study the rate (or speed) at which a chemical process occurs. Besides information about the speed

More information

Chemistry Fourth Marking Period Review Sheet Spring, Mr. Wicks

Chemistry Fourth Marking Period Review Sheet Spring, Mr. Wicks Chemistry Fourth Marking Period Review Sheet Spring, Mr. Wicks Chapter 11: Chemical Reactions Chemical equations use symbols to represent chemical reactions that take place in a laboratory. I can write

More information

UNIT 8: SOLUTIONS. Essential Question: What kinds of properties affect a chemical s solubility?

UNIT 8: SOLUTIONS. Essential Question: What kinds of properties affect a chemical s solubility? UNIT 8: SOLUTIONS Essential Question: What kinds of properties affect a chemical s solubility? SOLUTIONS & THEIR CHARACTERISTICS (5) Most chemical reactions take place IN solutions 1. Homogeneous mixture

More information

The Water Molecule. Draw the Lewis structure. H O H. Covalent bonding. Bent shape

The Water Molecule. Draw the Lewis structure. H O H. Covalent bonding. Bent shape Water & Solutions 1 The Water Molecule Draw the Lewis structure. H O H Covalent bonding. Bent shape 2 Water What determines whether a molecule is polar? Is water a polar molecule? d- d+ d+ 1. Oxygen is

More information

Lecture Presentation. Chapter 14. James F. Kirby Quinnipiac University Hamden, CT. Chemical Kinetics Pearson Education

Lecture Presentation. Chapter 14. James F. Kirby Quinnipiac University Hamden, CT. Chemical Kinetics Pearson Education Lecture Presentation Chapter 14 James F. Kirby Quinnipiac University Hamden, CT In chemical kinetics we study the rate (or speed) at which a chemical process occurs. Besides information about the speed

More information

Chapter 13. Characteristics of a Solution. Example of A Homogenous Mixtures. Solutions

Chapter 13. Characteristics of a Solution. Example of A Homogenous Mixtures. Solutions Chapter 13 Solutions Characteristics of a Solution A solution is a homogeneous mixture A solution is composed of a: Solute: the substance in lesser amount Solvent: the substance in greater amount Two liquid

More information

Chemical Kinetics -- Chapter 14

Chemical Kinetics -- Chapter 14 Chemical Kinetics -- Chapter 14 1. Factors that Affect Reaction Rate (a) Nature of the reactants: molecular structure, bond polarity, physical state, etc. heterogeneous reaction: homogeneous reaction:

More information

7. A solution has the following concentrations: [Cl - ] = 1.5 x 10-1 M [Br - ] = 5.0 x 10-4 M

7. A solution has the following concentrations: [Cl - ] = 1.5 x 10-1 M [Br - ] = 5.0 x 10-4 M Solubility, Ksp Worksheet 1 1. How many milliliters of 0.20 M AlCl 3 solution would be necessary to precipitate all of the Ag + from 45ml of a 0.20 M AgNO 3 solution? AlCl 3(aq) + 3AgNO 3(aq) Al(NO 3)

More information

Lecture Presentation. Chapter 14. Chemical Kinetics. John D. Bookstaver St. Charles Community College Cottleville, MO Pearson Education, Inc.

Lecture Presentation. Chapter 14. Chemical Kinetics. John D. Bookstaver St. Charles Community College Cottleville, MO Pearson Education, Inc. Lecture Presentation Chapter 14 John D. Bookstaver St. Charles Community College Cottleville, MO In kinetics we study the rate at which a chemical process occurs. Besides information about the speed at

More information

Review Sheet 6 Math and Chemistry

Review Sheet 6 Math and Chemistry Review Sheet 6 Math and Chemistry The following are some points of interest in Math and Chemistry. Use this sheet when answering these questions. Molecular Mass- to find the molecular mass, you must add

More information

UNIT 7: SOLUTIONS STUDY GUIDE REGENTS CHEMISTRY Unit 7 Exam will be on Thursday 2/16

UNIT 7: SOLUTIONS STUDY GUIDE REGENTS CHEMISTRY Unit 7 Exam will be on Thursday 2/16 UNIT 7: SOLUTIONS STUDY GUIDE Name REGENTS CHEMISTRY Unit 7 Exam will be on Thursday 2/16 Vocabulary- Match the terms to the correct definitions. 1. colligative properties 2. concentration 3. electrolyte

More information

Chemical Kinetics. Chapter 13. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Chemical Kinetics. Chapter 13. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chemical Kinetics Chapter 13 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chemical Kinetics Thermodynamics does a reaction take place? Kinetics how fast does

More information

Kinetics CHAPTER IN THIS CHAPTER

Kinetics CHAPTER IN THIS CHAPTER CHAPTER 14 Kinetics IN THIS CHAPTER Summary: Thermodynamics often can be used to predict whether a reaction will occur spontaneously, but it gives very little information about the speed at which a reaction

More information

11/2/ and the not so familiar. Chemical kinetics is the study of how fast reactions take place.

11/2/ and the not so familiar. Chemical kinetics is the study of how fast reactions take place. Familiar Kinetics...and the not so familiar Reaction Rates Chemical kinetics is the study of how fast reactions take place. Some happen almost instantaneously, while others can take millions of years.

More information

Ch 13 The Properties of Mixtures: Solutions and Colloids

Ch 13 The Properties of Mixtures: Solutions and Colloids Ch 13 The Properties of Mixtures: Solutions and Colloids Key equations: Concentration Unit - Quantitative Ways of Expressing Concentration Principles of Solubility Colligative Properties of Solutions nonelectrolyte

More information

Answers to Unit 4 Review: Reaction Rates

Answers to Unit 4 Review: Reaction Rates Answers to Unit 4 Review: Reaction Rates Answers to Multiple Choice 1. c 13. a 25. a 37. c 49. d 2. d 14. a 26. c 38. c 50. d 3. c 15. d 27. c 39. c 51. b 4. d 16. a 28. b 40. c 52. c 5. c 17. b 29. c

More information

Chapter 14 Chemical Kinetics

Chapter 14 Chemical Kinetics Chapter 14 Chemical Kinetics Learning goals and key skills: Understand the factors that affect the rate of chemical reactions Determine the rate of reaction given time and concentration Relate the rate

More information

Chapter 14. Chemical Kinetics

Chapter 14. Chemical Kinetics Chapter 14. Chemical Kinetics 14.1 Factors that Affect Reaction Rates The speed at which a chemical reaction occurs is the reaction rate. Chemical kinetics is the study of how fast chemical reactions occur.

More information

Chapter 11: CHEMICAL KINETICS

Chapter 11: CHEMICAL KINETICS Chapter : CHEMICAL KINETICS Study of the rate of a chemical reaction. Reaction Rate (fast or slow?) Igniting gasoline? Making of oil? Iron rusting? We know about speed (miles/hr). Speed Rate = changes

More information

Name: UNIT 5 KINETICS NOTES PACEKT #: KINETICS NOTES PART C

Name: UNIT 5 KINETICS NOTES PACEKT #: KINETICS NOTES PART C KINETICS NOTES PART C IV) Section 14.4 The Change of Concentration with Time A) Integrated Rate Law: shows how the concentration of the reactant(s) varies with time 1) [A]0 is the initial concentration

More information

Types of Mixtures. Main Idea. Heterogeneous and Homogeneous Mixtures. Key Terms soluble solute electrolyte solution suspension nonelectrolyte

Types of Mixtures. Main Idea. Heterogeneous and Homogeneous Mixtures. Key Terms soluble solute electrolyte solution suspension nonelectrolyte Types of Mixtures Key Terms soluble solute electrolyte solution suspension nonelectrolyte solvent colloid It is easy to determine that some materials are mixtures because you can see their component parts.

More information

Classifica,on of Solu,ons

Classifica,on of Solu,ons SOLUTIONS Solu,on Homogeneous mixture in which one substance is dissolved in another SOLUTE: substance that is dissolved SOLVENT: substance doing the dissolving INSOLUBLE: does NOT dissolve SOLUBLE: does

More information

CHEM134- Fall 2018 Dr. Al-Qaisi Chapter 4b: Chemical Quantities and Aqueous Rxns So far we ve used grams (mass), In lab: What about using volume in lab? Solution Concentration and Solution Stoichiometry

More information

Chemistry. Approximate Timeline. Students are expected to keep up with class work when absent.

Chemistry. Approximate Timeline. Students are expected to keep up with class work when absent. Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 15 SOLUTIONS Day Plans for the day Assignment(s) for the day 1 Begin Chapter 15

More information

Chemistry 40S Chemical Kinetics (This unit has been adapted from

Chemistry 40S Chemical Kinetics (This unit has been adapted from Chemistry 40S Chemical Kinetics (This unit has been adapted from https://bblearn.merlin.mb.ca) Name: 1 2 Lesson 1: Introduction to Kinetics Goals: Identify variables used to monitor reaction rate. Formulate

More information

Chemistry 40S Chemical Kinetics (This unit has been adapted from

Chemistry 40S Chemical Kinetics (This unit has been adapted from Chemistry 40S Chemical Kinetics (This unit has been adapted from https://bblearn.merlin.mb.ca) Name: 1 2 Lesson 1: Introduction to Kinetics Goals: Identify variables used to monitor reaction rate. Formulate

More information