Notes: Unit 10 Kinetics and Equilibrium
|
|
- Terence Newton
- 5 years ago
- Views:
Transcription
1 Name: Regents Chemistry: Mr. Palermo Notes: Unit 10 Kinetics and Equilibrium
2 Name: KEY IDEAS Collision theory states that a reaction is most likely to occur if reactant particles collide with the proper energy and orientation. (3.4d) The rate of a chemical reaction depends on several factors: temperature, concentration, nature of reactants, surface area, and the presence of a catalyst. (3.4f) Some chemical and physical changes can reach equilibrium. (3.4h) At equilibrium the rate of the forward reaction equals the rate of the reverse reaction. The measurable quantities of reactants and products remain constant at equilibrium. (3.4i) LeChatelier s principle can be used to predict the effect of stress (change in pressure, volume, concentration, and temperature) on a system at equilibrium. (3.4j) Energy released or absorbed by a chemical reaction can be represented by a potential energy diagram. (4.1c) Energy released or absorbed during a chemical reaction (heat of reaction) is equal to the difference between the potential energy of the products and the potential energy of the reactants. (4.1d) A catalyst provides an alternate reaction pathway, which has a lower activation energy than an uncatalyzed reaction. (3.4g) VOCABULARY For each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbook definitions. Write something to help you remember the word. Explain the word as if you were explaining it to an elementary school student. Give an example if you can. Don t use the words given in your definition! Reaction Rate: Entropy: Potential Energy: Catalyst: Activation Energy: Activated Complex: Spontaneous Reaction: LeChatelier s Principle:
3 Lesson 1: Collision Theory and Factors Affecting Rx Rate Objective: Determine what factors affect the rate of reaction KINETICS: Study of the RATE or SPEED at which REACTIONS occur A Reaction is the BREAKING and REFORMING of BONDS to make entirely new compounds as products. EFFECTIVE COLLISIONS: In order for a reaction to occur, reactant PARTICLES MUST COLLIDE (effectively) with the following: 1.) 2.) Example: H2 + I2 2HI 1
4 Lesson 1: Collision Theory and Factors Affecting Rx Rate Factors Affecting Reaction Rate SIX FACTORS that affect the rate of reaction by changing the number of effective collisions that take place between particles. The MORE EFFECTIVE COLLISIONS, THE FASTER THE REACTION! 1. TYPE OF SUBSTANCE: substances react Easily break into IONS when you dissolve them. Example: AgNO3 (s) Ag + + NO3 - substances react Requires more energy/time to break bonds Example: H2 (g)+i2 (g) 2 HI (g) 2. CONCENTRATION: Concentration reaction rate (speed) a. More particles increases chance of effective collisions 2
5 Lesson 1: Collision Theory and Factors Affecting Rx Rate 3. TEMPERATURE: temperature Reaction Rate: a. Increases # of effective collisions Reactants have more energy when colliding 4. PRESSURE (GASES ONLY) pressure, reaction rate (affects GASES ONLY!) a. Due to an increase in concentration 5. SURFACE AREA: in surface area the reaction rate. a. Due to more exposed particles that can react (more effective collisions) 6. CATALYST: Substance that rxn rate without being consumed in the rxn 3
6 Lesson 1: Collision Theory and Factors Affecting Rx Rate SUMMARY: Ionic solutions have faster reactions than molecule compounds. (bonding) Temp. Rate conc. rate surface area rate Pressure rate, P rate Catalysts speed up reactions. PRACTICE: At room temperature which reaction would be expected to have the fastest reaction rate? a.) Pb 2+ (aq) + S -2 (aq) b.) 2H2(g) + O2(g) c.) N2(g) + 2O2(g) d.) 2KClO3(s) PbS(s) 2H2O(l) 2NO2(g) 2KCl(s) + 3O2(g) PRACTICE: Under what conditions will the rate of a chemical reaction always decrease? a.) The concentration of the reactants decreases and the temp decreases b.) The concentration of the reactants decreases, and the temp increases c.) The concentration of the reactants increases and the temp increases d.) The concentration of the reactants increases, and the temp increases CHECK YOUR UNDERSTANDIND: Given the reaction: Zn(s) + 2HCl(aq) ZnCl2 + H2(g) The reaction occurs more slowly when a single piece of zinc is used than when the same mass of powdered zinc is used. Why does this occur? a.) The powdered zinc is more concentrated b.) The powdered zinc has a greater surface area c.) The powdered zinc requires less activation energy d.) The powdered zinc generates more heat energy 4
7 Lesson 2: Energy Changes in Chemical Reactions Review Objective: Determine if a reaction is endo or exothermic Use table I to determine the type of reaction HEAT OF REACTION ΔH: The amount of HEAT ENERGY LOST or GAINED throughout a REACTION ΔHheat of reaction = Hproducts - Hreactants (ΔH = enthalpy) TYPES OF CHEMICAL REACTIONS: ENDOTHERMIC REACTIONS: Heat is by Energy stored in chemical bonds of products ΔH is (+) A + B + ENERGY ---> C + D EXAMPLE: Reaction A + B C If HA =40kJ and HB =20kJ, then reactants have a total of 60kJ If HC =110kJ, then ( =) 50kJ of heat must have been absorbed by the reactants. Rewritten: A + B + 50kJ C Total energy on both sides are equal (law of conservation of energy) EXAMPLE from TABLE I 1
8 Lesson 2: Energy Changes in Chemical Reactions Review EXOTHERMIC REACTIONS: Heat is as a ΔH is (-) More stable reaction Spontaneous A + B ---> C + D + ENERGY Example: Reaction A + B C If HA =60kJ and HB =40kJ,then reactants have a total of 100kJ If HC =30kJ, then ( =) 70kJ of heat must have been released as a product. Rewritten: A + B C + 70kJ Total energy on both sides are equal (law of conservation of energy) EXAMPLE from TABLE I Example: Reverse reactions on Table I What is the ΔH of the following reaction? Is this exothermic or endothermic? 2H2O(l) 2H2(g) + O2(g) ***For reverse reactions switch signs of ΔH kJ (endothermic) 2
9 Lesson 2: Energy Changes in Chemical Reactions Review PRACTICE: What is the heat of reaction (ΔH) of the following? Is this exothermic or endothermic? 2H2(g) + O2(g) 2H2O(l) CHECK YOUR UNDERSTANDING: Fill in the table using table I 3
10 Lesson 3: Potential Energy Diagrams Objective: Label potential energy diagrams and determine the type of diagram represented POTENTIAL ENERGY DIAGRAMS: Shows the change in potential (stored) energy during a chemical reaction Types of Potential Energy Diagrams: EXOTHERMIC POTENTIAL ENERGY DIAGRAM: than reactant side WHY? Energy is released as a product, so the net amount of potential energy decreases. (-) ΔH ENDOTHERMIC POTENTIAL ENERGY DIAGRAM than reactant side WHY? Energy is absorbed by the reactants, so the net amount of potential energy increases. (+) ΔH 1
11 Lesson 3: Potential Energy Diagrams Parts of the Potential Energy Diagram You must be able to label these so label the diagrams in your notes as we go through this!!! ACTIVATION ENERGY: Minimum energy required for a reaction to occur (energy needed to get over the hill) ACTIVATED COMPLEX: Highest energy point of reaction Temporary Where bonds are broken and reformed 2
12 Lesson 3: Potential Energy Diagrams HEAT OF REACTANTS/PRODUCTS: Amount of potential energy possessed by the reactants and products HEAT OF REACTION ΔH Amount of energy lost/gained in a reaction SUBTRACT heat of products minus reactants ΔH = H(products) H(reactants) EFFECTS OF ADDING A CATALYST the activation energy (energy needed to start the reaction) Reaction occurs 3
13 Lesson 3: Potential Energy Diagrams PRACTICE: Is this an endothermic or exothermic reaction? How do you know? PRACTICE: Which arrow represents the activation energy of the forward reactants? CHECK YOUR UNDERSTANDING: Is the ΔH positive or negative for this reaction? 4
14 Lesson 4: equilibrium Objective: Determine if a reaction is spontaneous Determine if entropy increases or decreases in a reaction EQUILIBRIUM: The of the forward reaction is to the rate of the reverse reaction Equilibrium is Dynamic (in constant motion) Equilibrium is represented by double arrow 1. Physical (Phase) Equilibrium: Types of Equilibrium (all occur in closed systems) Rate of forward phase change equals rate of reverse phase change Ratevaporizing = Ratecondensing Ex. Water is vaporizing at the same rate it is condensing 2. Chemical Equilibrium : The rate of the forward reaction is equal to the rate of the reverse reaction Ex. The Haber Process 1
15 Lesson 4: equilibrium 3. Solution Equilibrium: The rate of dissolving equals the rate of precipitating. Ex. Will a reaction happen on its own once it s started? SPONTANEOUS REACTIONS: A reaction that happens on its own once initiated (lower activation energy) Increase in Recall. Entropy The randomness (disorder) of the system. The More substances the more entropy The higher the temperature the more entropy ENTROPY AND STATES OF MATTER: Changes in Entropy 2
16 Lesson 4: equilibrium EXAMPLE: (determine if there is an increase or decrease in entropy) 1. KClO3(s) 2KCl(s) + 3O2(g) 2. KCl(l) KCl(s) 3. CO2(s) CO2(g) PRACTICE: (determine if there is an increase or decrease in entropy) 1. H + (aq) + C2H3O2 - (aq) HC2H3O3(l) 2. H + (aq) + OH (aq) H2O(l) PRACTICE: What point on the heating curve has the most entropy? PRACTICE: Which reaction will occur spontaneously? 3
17 Lesson 4: equilibrium PRACTICE: According to table I which reaction will occur spontaneously? a. N2(g) + 2O2(g) 2NO2(g) b. 2H2(g) + O2(g) 2H2O(g) CHECK YOUR UNDERSTANDING: (determine if there is an increase or decrease in entropy) 1. H2(g) + Cl2(g) 2HCl(g) 2. H2O(g) H2O(s) 4
18 Lesson 5: Changing Equilibrium Objective: Determine the shift in equilibrium when a stress is placed on a system LE CHATELIER s PRINCIPLE: If a system at equilibrium is subjected to a STRESS, the equilibrium will shift in the direction that relieves that stress Causes a change in concentration of both the reactants and products until the equilibrium is re-established. TYPES OF STRESS: Concentration temperature pressure for gases 1
19 Lesson 5: Changing Equilibrium TRICK FOR EQUILIBIRUM SHIFTS: How to determine equilibrium shifts When you a stress the equilibrium shifts from the stress When you (take away) a stress the equilibrium will shift back the decrease to replace it. CONCENTRATION: TEMPERATURE: 2
20 Lesson 5: Changing Equilibrium PRESSURE (GASES ONLY): CATALYST: on equilibrium because both the forward and reverse reactions will be affected equally (both will speed up). EXAMPLE: The Haber Process N2 (g) + 3 H2 (g) 2 NH3 (g) + heat a) [N2] shift towards products (right) b) [H2] shift towards reactants (left) c) [NH3] shift towards reactants (left) d) [NH3] shift towards products (right) e) pressure shift towards products (right) f) pressure shift towards reactants (left) g) temperature shift towards reactants (left) h) temperature shift towards products (right) 3
21 Lesson 5: Changing Equilibrium PRACTICE: 2CO(g) + O2(g) 2CO2(g) kj 1. If concentration of CO is increased what direction will the equilibrium shift? 2. What happens to the concentration of CO2? 3. What happens to the concentration of O2? PRACTICE: 2CO(g) + O2(g) 2CO2(g) kj 1. If O2 is removed, what direction does the equilibrium shift? 2. What happens to the concentration of CO? 3. What happens to the concentration of CO2? CHECK YOUR UNDERSTANDING: Given the equation representing a reaction at equilibrium: N2(g) + 3H2(g) <==>2NH3(g) What occurs when the concentration of H2(g) is increased? (1) The equilibrium shifts to the left, and the concentration of N2(g) decreases. (2) The equilibrium shifts to the left, and the concentration of N2(g) increases. (3) The equilibrium shifts to the right,and the concentration of N2(g) decreases. (4) The equilibrium shifts to the right, and the concentration of N2(g) increases 4
Notes: Unit 11 Kinetics and Equilibrium
Name: Regents Chemistry: Notes: Unit 11 Kinetics and Equilibrium Name: KEY IDEAS Collision theory states that a reaction is most likely to occur if reactant particles collide with the proper energy and
More informationName: Unit!!: Kinetics and Equilibrium REGENTS CHEMISTRY
Name: Unit!!: Kinetics and Equilibrium REGENTS CHEMISTRY 1 Name: Unit!!: Kinetics and Equilibrium Collision theory states that a reaction is most likely to occur if reactant particles collide with the
More informationUNIT 8 KINETICS & EQ: NOTE & PRACTICE PACKET
UNIT 8 KINETICS & EQ: NOTE & PRACTICE PACKET 1 2 Lesson 1: Kinetics = study of the RATE or SPEED at which REACTIONS occur A REACTION is the Reaction Mechanism = STEP BY STEP PROCESS needed to make a product;
More informationUnit 6 Kinetics and Equilibrium.docx
6-1 Unit 6 Kinetics and Equilibrium At the end of this unit, you ll be familiar with the following: Kinetics: Reaction Rate Collision Theory Reaction Mechanism Factors Affecting Rate of Reaction: o Nature
More informationKinetics and Equilibrium Extra Credit
1. The potential energy diagram below represents the reaction 2 KClO3 2 KCl + 3 O2. 4. When AgNO3(aq) is mixed with NaCl(aq), a reaction occurs which tends to go to completion and not reach equilibrium
More informationName Unit 10 Practice Test
1. Increasing the temperature increases the rate of a reaction by A) lowering the activation energy B) increasing the activation energy C) lowering the frequency of effective collisions between reacting
More information8. A piece of Mg(s) ribbon is held in a Bunsen burner flame and begins to burn according to the equation: 2Mg(s) + O2 (g) 2MgO(s).
1. Which event must always occur for a chemical reaction to take place? A) formation of a precipitate B) formation of a gas C) effective collisions between reacting particles D) addition of a catalyst
More informationEnergy Changes, Reaction Rates and Equilibrium. Thermodynamics: study of energy, work and heat. Kinetic energy: energy of motion
Energy Changes, Reaction Rates and Equilibrium Thermodynamics: study of energy, work and heat Kinetic energy: energy of motion Potential energy: energy of position, stored energy Chemical reactions involve
More informationUNIT 9: KINETICS & EQUILIBRIUM. Essential Question: What mechanisms affect the rates of reactions and equilibrium?
UNIT 9: KINETICS & EQUILIBRIUM Essential Question: What mechanisms affect the rates of reactions and equilibrium? What is Kinetics? Kinetics is the branch of chemistry that explains the rates of chemical
More informationRegents review Kinetics & equilibrium
2011-2012 1. A is most likely to occur when reactant particles collide with A) proper energy, only B) proper orientation, only C) both proper energy and proper orientation D) neither proper energy nor
More informationUnit 13: Rates and Equilibrium- Guided Notes
Name: Period: What is a Chemical Reaction and how do they occur? Unit 13: Rates and Equilibrium- Guided Notes A chemical reaction is a process that involves of atoms Law of Conservation of : Mass is neither
More information1. As the number of effective collisions between reacting particles increases, the rate of reaction (1) decreases (3) remains the same (2) increases
1. As the number of effective collisions between reacting particles increases, the rate of reaction (1) decreases (3) remains the same (2) increases 2. The energy needed to start a chemical reaction is
More informationName Chemistry Exam #8 Period: Unit 8: Kinetics, Thermodynamics, & Equilibrium
1. Which quantities must be equal for a chemical reaction at equilibrium? (A) the potential energies of the reactants and products (B) the concentrations of the reactants and products (C) the activation
More informationName: Kinetics & Thermodynamics Date: Review
Name: Kinetics & Thermodynamics Date: Review 1. What is required for a chemical reaction to occur? A) standard temperature and pressure B) a catalyst added to the reaction system C) effective collisions
More informationKinetics & Equilibrium
Kinetics & Equilibrium Name: Essential Questions How can one explain the structure, properties, and interactions of matter? Learning Objectives Explain Collision Theory Molecules must collide in order
More informationUnit 13 Kinetics & Equilibrium Page 1 of 14 Chemistry Kinetics, Entropy, Equilibrium, LeChatelier s Principle, K, Unit 13 Quiz: Unit 13 Test:
Unit 13 Kinetics & Equilibrium Page 1 of 14 Chemistry Kinetics, Entropy, Equilibrium, LeChatelier s Principle, K, Unit 13 Quiz: Unit 13 Test: Final Project: VOCABULARY: 1 Chemical equilibrium 2 equilibrium
More informationUNIT 15 - Reaction Energy & Reaction Kinetics. I. Thermochemistry: study of heat in chemical reactions and phase changes
I. Thermochemistry: study of heat in chemical reactions and phase changes II. A. Heat equation (change in temperature): Q = m. C. p T 1. Q = heat (unit is Joules) 2. m = mass (unit is grams) 3. C p = specific
More informationUnit 10 Thermodynamics, Kinetics and Equilibrium Notes
Unit 10 Thermodynamics, Kinetics and Equilibrium Notes What is Thermodynamics? Almost all chemical reactions involve a between the and its. Thermo = Dynamics = What is energy? What is heat? Thermochemistry
More informationUnit 7 Kinetics and Thermodynamics
17.1 The Flow of Energy Heat and Work Unit 7 Kinetics and Thermodynamics I. Energy Transformations A. Temperature 1. A measure of the average kinetic energy of the particles in a sample of matter B. Heat
More informationUnit 9a: Kinetics and Energy Changes
Unit 9a: Kinetics and Energy Changes Student Name: Key Class Period: Website upload 2015 Page 1 of 43 Unit 9a (Kinetics & Energy Changes) Key Page intentionally blank Website upload 2015 Page 2 of 43 Unit
More informationGummy Bear Demonstration:
Name: Unit 8: Chemical Kinetics Date: Regents Chemistry Aim: _ Do Now: a) Using your glossary, define chemical kinetics: b) Sort the phrases on the SmartBoard into the two columns below. Endothermic Rxns
More informationUnit 8 Kinetics & Equilibrium Notes & CW
Unit 8 Kinetics & Equilibrium Notes & CW 2 The bold, underlined words are important vocabulary words that you should be able to define and use properly in explanations. This is a study guide for what you
More informationReaction Rate and Equilibrium Chapter 19 Assignment & Problem Set
Reaction Rate and Equilibrium Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Reaction Rate and Equilibrium 2 Study Guide: Things You Must Know
More informationName: Regents Chemistry: Mr. Palermo. Student Version. Notes: Unit 6A Heat
Name: Regents Chemistry: Mr. Palermo Student Version Notes: Unit 6A Heat Name: KEY IDEAS Heat is a transfer of energy (usually thermal energy) from a body of higher temperature to a body of lower temperature.
More informationCollision Theory. Unit 12: Chapter 18. Reaction Rates. Activation Energy. Reversible Reactions. Reversible Reactions. Reaction Rates and Equilibrium
Collision Theory For reactions to occur collisions between particles must have Unit 12: Chapter 18 Reaction Rates and Equilibrium the proper orientation enough kinetic energy See Both In Action 1 2 Activation
More informationBase your answers to questions 1 and 2 on the information below. Given the reaction at equilibrium: Base your answers to questions 5 through 7 on the
Base your answers to questions 1 and 2 on the information below. Given the reaction at equilibrium: Base your answers to questions 5 through 7 on the potential energy diagram and the equation below. 2NO
More informationReaction Rates & Equilibrium. What determines how fast a reaction takes place? What determines the extent of a reaction?
Reaction Rates & Equilibrium What determines how fast a reaction takes place? What determines the extent of a reaction? Reactants Products 1 Reaction Rates Vary TNT exploding. A car rusting. Dead plants
More informationReaction Rates & Equilibrium. What determines how fast a reaction takes place? What determines the extent of a reaction?
Reaction Rates & Equilibrium What determines how fast a reaction takes place? What determines the extent of a reaction? Reactants Products 1 Reaction Rates Vary TNT exploding. A car rusting. Dead plants
More informationName: Regents Chemistry: Mr. Palermo. Notes: Unit 7 Heat.
Name: Regents Chemistry: Mr. Palermo Notes: Unit 7 Heat 1 Name: KEY IDEAS Heat is a transfer of energy (usually thermal energy) from a body of higher temperature to a body of lower temperature. Thermal
More information6. [EXO] reactants have more energy 7. [EXO] H is negative 8. [ENDO] absorbing sunlight to make sugar 9. [ENDO] surroundings get cold
10.A Thermo: Endo/Exo and ΔH 1. For each of the following laws of thermodynamics, what does each actually mean in terms of the behavior of energy and particles? 1 st Law of Thermodynamics? Energy is neither
More informationHC- Kinetics and Thermodynamics Test Review Stations
HC- Kinetics and Thermodynamics Test Review Stations Station 1- Collision Theory and Factors Affecting Reaction Rate 1. Explain the collision theory of reactions. 2. Fill out the following table to review
More informationChemical Equilibrium
Chemical Equilibrium Forward Rxn: A + B C + D Reverse Rxn: A + B C + D Written as: A + B C + D OR A + B C + D A reversible reaction has both an endothermic rxn and an exothermic rxn Reactants Exothermic
More informationEnd of Year Review ANSWERS 1. Example of an appropriate and complete solution H = 70.0 g 4.19 J/g C T = 29.8 C 22.4 C 7.4 C
End of Year Review ANSWERS 1. Example of an appropriate and complete solution H = mc T mol HCl m = 70.0 g c = 4.19 J/g C T = 9.8 C.4 C = 7.4 C mol HCl = 3.00 mol/ 0.000 = 0.0600 mol H = 70.0 g 4.19 J/g
More information) DON T FORGET WHAT THIS REPRESENTS.
5.J Thermo: Endo/Exo and ΔH I Pledge : ( Initial ) DON T FORGET WHAT THIS REPRESENTS. 1. For each of the following laws of thermodynamics, what does each actually mean in terms of the behavior of energy
More informationName AP CHEM / / Collected AP Exam Essay Answers for Chapter 16
Name AP CHEM / / Collected AP Exam Essay Answers for Chapter 16 1980 - #7 (a) State the physical significance of entropy. Entropy (S) is a measure of randomness or disorder in a system. (b) From each of
More informationUNIT #10: Reaction Rates Heat/Energy in Chemical Reactions Le Chatlier s Principle Potential Energy Diagrams
UNIT #10: Reaction Rates Heat/Energy in Chemical Reactions Le Chatlier s Principle Potential Energy Diagrams NAME: 1. REACTION RATES a) The speed of a chemical reaction determined by the change in concentration
More informationWarm up. 1) What is the conjugate acid of NH 3? 2) What is the conjugate base of HNO 2? 3) If the ph is 9.2, what is the [H 3 O + ], poh, and [OH - ]?
Warm up 1) What is the conjugate acid of NH 3? 2) What is the conjugate base of HNO 2? 3) If the ph is 9.2, what is the [H 3 O + ], poh, and [OH - ]? 4) What is the concentration of H 2 SO 4 if 30.1 ml
More informationKinetic energy is the energy of motion (of particles). Potential energy involves stored energy (energy locked up in chemical bonds)
Enthalpy (H) Enthalpy (H) is the total energy amount (Epotential + Ekinetic) of a system during a chemical reaction under constant temperature and pressure conditions. Kinetic energy is the energy of motion
More informationKinetics & Equilibrium. Le Châtelier's Principle. reaction rates. + Packet 9: Daily Assignment Sheet '19 Name: Per
Daily Assignment Sheet '19 Name: Per (check them off as you complete them) Due Date Assignment Thur 2/21 Do clock reaction lab Fri 2/22 Do Not Write In That Box Below Mon 2/25 Do WS 9.1 Tue 2/26 Do WS
More informationCollision Theory. and I 2
Collision Theory To explain why chemical reactions occur, chemists have proposed a model, known as collision theory, which states that molecules must collide in order to react. These collisions can involve
More informationCHAPTER 16: REACTION ENERGY AND CHAPTER 17: REACTION KINETICS. Honors Chemistry Ms. Agostine
CHAPTER 16: REACTION ENERGY AND CHAPTER 17: REACTION KINETICS Honors Chemistry Ms. Agostine 16.1 Thermochemistry Definition: study of the transfers of energy as heat that accompany chemical reactions and
More informationHow fast or slow will a reaction be? How can the reaction rate may be changed?
Part I. 1.1 Introduction to Chemical Kinetics How fast or slow will a reaction be? How can the reaction rate may be changed? *In order to understand how these factors affect reaction rates, you will also
More informationCollision Theory. Collision theory: 1. atoms, ions, and molecules must collide in order to react. Only a small number of collisions produce reactions
UNIT 16: Chemical Equilibrium collision theory activation energy activated complex reaction rate reversible reaction chemical equilibrium law of chemical equilibrium equilibrium constant homogeneous equilibrium
More informationUnit 13: Rates and Equilibrium- Funsheets
Name: Period: Unit 13: Rates and Equilibrium- Funsheets Part A: Reaction Diagrams 1) Answer the following questions based on the potential energy diagram shown here: a. Does the graph represent an endothermic
More informationREACTION EQUILIBRIUM
REACTION EQUILIBRIUM A. REVERSIBLE REACTIONS 1. In most spontaneous reactions the formation of products is greatly favoured over the reactants and the reaction proceeds to completion (one direction). In
More informationUnit 9 Kinetics SA Review
1. Base your answer to the following question on the information below. The equilibrium equation below is related to the manufacture of a bleaching solution. In this equation, means that chloride ions
More informationChemistry 12 Provincial Workbook Unit 01: Reaction Kinetics. Multiple Choice Questions
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 1 / 68 Chemistry 1 Provincial Workbook Unit 01: Reaction Kinetics Multiple Choice Questions 1. Which of the following describes what happens
More informationHEAT, TEMPERATURE, & THERMAL ENERGY. Work - is done when an object is moved through a distance by a force acting on the object.
HEAT, TEMPERATURE, & THERMAL ENERGY Energy A property of matter describing the ability to do work. Work - is done when an object is moved through a distance by a force acting on the object. Kinetic Energy
More informationWork hard. Be nice. 100% EVERYDAY.
Name: Period: Date: UNIT 10: Energy Lesson 1: Entropy vs. Enthalpy By the end of today, you will have an answer to: What conditions are favored during reactions? Definition Enthalpy is another word for
More informationA reversible reaction is a chemical reaction where products can react to form the reactants and vice versa.
Chemistry 12 Unit II Dynamic Equilibrium Notes II.1 The Concept of Dynamic Equilibrium A reversible reaction is a chemical reaction where products can react to form the reactants and vice versa. A reversible
More informationCHAPTER 17 REVIEW. Reaction Kinetics. Answer the following questions in the space provided. Energy B A. Course of reaction
CHAPTER 17 REVIEW Reaction Kinetics SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Refer to the energy diagram below to answer the following questions. D Energy C d c d
More informationDate: Hybrid Chemistry Regents Prep Ms. Hart/Mr. Kuhnau
Name: Period: Date: Hybrid Chemistry Regents Prep Ms. Hart/Mr. Kuhnau UNIT 5: Kinetics and Equilibrium Lesson 1: Collision theory and potential energy diagrams By the end of today, you will have an answer
More informationRates, Temperature and Potential Energy Diagrams Worksheet
SCH4U1 ER10 Name: Date: Rates, Temperature and Potential Energy Diagrams Worksheet Part 1: 1. Use the potential energy diagram shown to the right to answer the following: a. Label the axis. y axis is potential
More informationB 2 Fe(s) O 2(g) Fe 2 O 3 (s) H f = -824 kj mol 1 Iron reacts with oxygen to produce iron(iii) oxide as represented above. A 75.
1 2004 B 2 Fe(s) + 3 2 O 2(g) Fe 2 O 3 (s) H f = -824 kj mol 1 Iron reacts with oxygen to produce iron(iii) oxide as represented above. A 75.0 g sample of Fe(s) is mixed with 11.5 L of O 2 (g) at 2.66
More informationEnergy Ability to produce change or do work. First Law of Thermodynamics. Heat (q) Quantity of thermal energy
THERMOCHEMISTRY Thermodynamics Study of energy and its interconversions Energy is TRANSFORMED in a chemical reaction (POTENTIAL to KINETIC) HEAT (energy transfer) is also usually produced or absorbed -SYSTEM:
More informationChanges & Chemical Reactions. Unit 5
Changes & Chemical Reactions Unit 5 5 Types of Chemical Reactions Double Decomposition Replacement 1 2 3 4 5 Synthesis Single Replacement Combustion Continue Synthesis 2H 2 + O 2 2H 2 O Menu Decomposition
More informationEnergy Diagram Endothermic Reaction Draw the energy diagram for exothermic and endothermic reactions. Label each part.
CP Chapter 18 Notes A Model for Reaction Rates Expressing Reaction Rates Average Rate = Δquantity Δtime The amount of increase or decrease depends on their mole ratios Units = or mol/ls Expressing Reaction
More informationThermodynamics. Thermodynamics of Chemical Reactions. Enthalpy change
Thermodynamics 1 st law (Cons of Energy) Deals with changes in energy Energy in chemical systems Total energy of an isolated system is constant Total energy = Potential energy + kinetic energy E p mgh
More informationChapter 8: Reaction Rates and Equilibrium
Chapter 8: Reaction Rates and Equilibrium ACTIVATION ENERGY In some reaction mixtures, the average total energy of the molecules is too low at the prevailing temperature for a reaction to take place at
More information10.02 PE Diagrams. 1. Given the equation and potential energy diagram representing a reaction:
10.02 PE Diagrams 1. Given the equation and potential energy diagram representing a reaction: 3. Given the potential energy diagram and equation representing the reaction between substances A and D : If
More informationA. 2.5 B. 5.0 C. 10. D. 20 (Total 1 mark) 2. Consider the following reactions. N 2 (g) + O 2 (g) 2NO(g) 2NO 2 (g) 2NO(g) + O 2 (g)
1. When 100 cm 3 of 1.0 mol dm 3 HCl is mixed with 100 cm 3 of 1.0 mol dm 3 NaOH, the temperature of the resulting solution increases by 5.0 C. What will be the temperature change, in C, when 50 cm 3 of
More informationChemistry 12 Review Sheet on Unit 1 -Reaction Kinetics
Chemistry 12 Review Sheet on Unit 1 -Reaction Kinetics 1. Looking at the expressions for reaction rate on page 1 SW, write similar expressions with which you could express rates for the following reactions.
More informationReview 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 informationNo Brain Too Small CHEMISTRY Energy changes ( ) & Expired ( ) QUESTIONS QUESTION 1 (2016:3)
QUESTION 1 (2016:3) QUESTIONS (iii) Pentane combustion: C5H12(l) + 8O2(g) 5CO2(g) + 6H2O(l) Δr H o = 3509 kj mol 1 Hexane, C6H14, like pentane, will combust (burn) in sufficient oxygen to produce carbon
More information8. The table below describes two different reactions in which Reaction 1 is faster. What accounts for this observation? Reaction 1 Reaction 2.
Public Review - Rates and Equilibrium June 2005 1. What does X represent in the diagram below? (A) activation energy for the forward reaction (B) activation energy for the reverse reaction (C) heat of
More informationAdvanced Chemistry Practice Problems
Thermodynamics: Review of Thermochemistry 1. Question: What is the sign of DH for an exothermic reaction? An endothermic reaction? Answer: ΔH is negative for an exothermic reaction and positive for an
More informationName Practice Questions Date Kinetics
Name Practice Questions Date Kinetics 1. An experiment was conducted to determine the rate law of the reaction 2 A + 2 B C + D. The data collected is shown below. Base your answers to questions 8 and 9
More informationEnergy Ability to produce change or do work. First Law of Thermodynamics. Heat (q) Quantity of thermal energy
THERMOCHEMISTRY Thermodynamics Study of energy and its interconversions Energy is TRANSFORMED in a chemical reaction (POTENTIAL to KINETIC) HEAT (energy transfer) is also usually produced or absorbed -SYSTEM:
More informationLecture 2. Review of Basic Concepts
Lecture 2 Review of Basic Concepts Thermochemistry Enthalpy H heat content H Changes with all physical and chemical changes H Standard enthalpy (25 C, 1 atm) (H=O for all elements in their standard forms
More informationAP Chemistry 1st Semester Final Review Name:
AP Chemistry 1st Semester Final Review Name: 2015-2016 1. Which of the following contains only sigma (s) bonds? 5. H2O(g) + CO(g) H2(g) + CO2(g) A) CO2 B) C3H6 C) CH3Cl D) N2O3 E) SiO2 2. What is the equilibrium
More informationCh 10 Practice Problems
Ch 10 Practice Problems 1. Which of the following result(s) in an increase in the entropy of the system? I. (See diagram.) II. Br 2(g) Br 2(l) III. NaBr(s) Na + (aq) + Br (aq) IV. O 2(298 K) O 2(373 K)
More informationThermochemistry Lecture
Thermochemistry Lecture Jennifer Fang 1. Enthalpy 2. Entropy 3. Gibbs Free Energy 4. q 5. Hess Law 6. Laws of Thermodynamics ENTHALPY total energy in all its forms; made up of the kinetic energy of the
More informationChemistry 12 Unit I Reaction Kinetics Study Guide
Chemistry 12 Unit I Reaction Kinetics Study Guide I.1 - Introduction: Reaction kinetics is the study of rates (speeds) of chemical reactions and the factors affect them. Rates of reaction are usually expressed
More information(g) burns according to this reaction? D) CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(l)
Name: 7171-1 - Page 1 1) In a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is defined as the A) heat of reaction B) ionization
More informationWhich of the following units could be used to express reaction rate? Reaction Kinetics Monster Review
Chemistry 12 Reaction Kinetics Monster Review 1. Which of the following units could be used to express reaction rate? A. ml s B. ml g C. g ml D. ml mol 2. Consider the reaction: Zn( s) + 2HCl( aq) ZnCl2(
More informationGibb s Free Energy. This value represents the maximum amount of useful work (non PV-work) that can be obtained by a system.
Gibb s Free Energy 1. What is Gibb s free energy? What is its symbol? This value represents the maximum amount of useful work (non PV-work) that can be obtained by a system. It is symbolized by G. We only
More informationRegents Review Kinetics & Equilibrium Worksheet Mr. Beauchamp
Regents Review Kinetics & Equilibrium Worksheet Mr. Beauchamp 1. Which event must always occur for a chemical r eaction to take place? A. formation of a precipitate B. formation of a gas C. effective collisions
More informationChemistry 12 Provincial Workbook Unit 02: Chemical Equilibrium. Multiple Choice Questions
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P. 1 / 63 Chemistry 1 Provincial Workbook Unit 0: Chemical Equilibrium 1. Consider the following... Multiple Choice Questions Which of the following
More informationThe Factors that Determine the Equilibrium State
The Factors that Determine the Equilibrium State The equilibrium state (or the ratio of products to reactants) is determined by two factors: 1. Energy Systems tend to move toward a state of minimum potential
More information1. Which of the following units could be used to express the reaction rate?
Chemistry 12 Kinetics Practice Test # 2 1. Which of the following units could be used to express the reaction rate? A. ml/s B. ml/g C. g/ml D. ml/mol 2. Consider the reaction: Zn (s) + 2HCl (aq) ZnCl 2(aq)
More informationThe Equilibrium State. Chapter 13 - Chemical Equilibrium. The Equilibrium State. Equilibrium is Dynamic! 5/29/2012
Chapter 13 - Chemical Equilibrium The Equilibrium State Not all chemical reactions go to completion; instead they attain a state of equilibrium. When you hear equilibrium, what do you think of? Example:
More informationPractice Packet Unit 3: Phase Changes & Heat
Regents Chemistry: Practice Packet Unit 3: Phase Changes & Heat Name: Assess Yourself: Lesson 1: Lesson 2: Lesson 3: Lesson 4: Vocab: 1 Review (Things you need to know in order to understand the new stuff
More informationChapter 17. Preview. Lesson Starter Objectives Reaction Mechanisms Collision Theory Activation Energy The Activated Complex Sample Problem A
Preview Lesson Starter Objectives Reaction Mechanisms Collision Theory Activation Energy The Activated Complex Sample Problem A Section 1 The Reaction Process Lesson Starter The reaction H 2 + I 2 2HI
More information6. Which will react faster: Magnesium and 2M hydrochloric acid, or Magnesium and 0.5M hydrochloric acid?
REACTION RATES WORKSHEET WS#1 1. Identify the three components of collision theory. What are the three factors that must be true for a collision to be successful? a. b. c. 2. Do all collisions result in
More informationWhat is a spontaneous reaction? One, that given the necessary activation energy, proceeds without continuous outside assistance
What is a spontaneous reaction? One, that given the necessary activation energy, proceeds without continuous outside assistance Why do some reactions occur spontaneously & others do not? Atoms react to
More informationHenry Le Chatelier ( ) was a chemist and a mining engineer who spent his time studying flames to prevent mine explosions.
Henry Le Chatelier (1850-1936) was a chemist and a mining engineer who spent his time studying flames to prevent mine explosions. He proposed a Law of Mobile equilibrium or Le Chatelier s principle The
More informationSaturday Study Session 1 3 rd Class Student Handout Thermochemistry
Saturday Study Session 1 3 rd Class Student Handout Thermochemistry Multiple Choice Identify the choice that best completes the statement or answers the question. 1. C 2 H 4 (g) + 3 O 2 (g) 2 CO 2 (g)
More informationUnit 9 Kinetics SA Review
1. Base your answer to the following question on the information below. The equilibrium equation below is related to the manufacture of a bleaching solution. In this equation, means that chloride ions
More information1. How much heat is required to warm 400. g of ethanol from 25.0ºC to 40.0ºC?
Heat and q=mcδt 1. How much heat is required to warm 400. g of ethanol from 25.0ºC to 40.0ºC? 2. What mass of water can be heated from 0.00ºC to 25.0ºC with 90,000. J of energy? 3. If 7,500. J of energy
More informationChapter 8 Reaction Rates and Equilibrium
Spencer L. Seager Michael R. Slabaugh www.cengage.com/chemistry/seager Chapter 8 Reaction Rates and Equilibrium SPONTANEOUS PROCESSES Spontaneous processes are processes that take place naturally with
More informationChapter 9. Chemical reactions
Chapter 9 Chemical reactions Topics we ll be looking at in this chapter Types of chemical reactions Redox and non-redox reactions Terminology associated with redox processes Collision theory and chemical
More informationKinetics & Equilibrium Review Packet. Standard Level. 1. Which quantities in the enthalpy level diagram are altered by the use of a catalyst?
Kinetics & Equilibrium Review Packet Standard Level 1. Which quantities in the enthalpy level diagram are altered by the use of a catalyst? Enthalpy I II III Time A. I and II only B. I and III only C.
More informationSection 1 - Thermochemistry
Reaction Energy Section 1 - Thermochemistry Virtually every chemical reaction is accompanied by a change in energy. Chemical reactions usually absorb or release energy as heat. You learned in Chapter 12
More informationReaction Rates and Chemical Equilibrium
Reaction Rates and Chemical Equilibrium 12-1 12.1 Reaction Rates a measure of how fast a reaction occurs. Some reactions are inherently fast and some are slow 12-2 12.2 Collision Theory In order for a
More informationReaction Rates and Chemical Equilibrium
Reaction Rates and Chemical Equilibrium : 12-1 12.1 Reaction Rates : a measure of how fast a reaction occurs. Some reactions are inherently fast and some are slow: 12-2 1 12.2 Collision Theory In order
More informationChapter Seven. Chemical Reactions: Energy, Rates, and Equilibrium
Chapter Seven Chemical Reactions: Energy, Rates, and Equilibrium Endothermic vs. Exothermic 2 Endothermic: A process or reaction that absorbs heat and has a positive ΔH. Exothermic: A process or reaction
More informationName Energy Test period Date
Name Energy Test period Date 1. The temperature 30. K expressed in degrees Celsius is 1) 243ºC 2) 243ºC 3) 303ºC 4) 303ºC 2. The potential energy diagram for a chemical reaction is shown below. 4. A sample
More informationChemistry I-H Types of Reactions / Reaction Prediction / Reaction Theory
Chemistry I-H Types of Reactions / Reaction Prediction / Reaction Theory I. Synthesis (combination) A + B ---------> AB Substances that are chemically combined may be two elements or two compounds. If
More informationFactors that Affect Reaction Rates
Factors that Affect Reaction Rates Preface: There are 2 kinds of reactions: Homogeneous reactions - all reactants are in the same phase (don't consider products) eg.) 3H 2(g) + N 2(g) 2NH 3(g) Ag + (aq)
More informationThermochemistry. Energy. 1st Law of Thermodynamics. Enthalpy / Calorimetry. Enthalpy of Formation
THERMOCHEMISTRY Thermochemistry Energy 1st Law of Thermodynamics Enthalpy / Calorimetry Hess' Law Enthalpy of Formation The Nature of Energy Kinetic Energy and Potential Energy Kinetic energy is the energy
More information