Chemistry 121 Chapters 7& 8 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question.
|
|
- Brook Holmes
- 5 years ago
- Views:
Transcription
1 Chemistry 121 Chapters 7& 8 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A sample of carbon dioxide occupies 22.4 L at STP. Which of the following statements apply to the sample? a. The sample contains atoms. b. The sample contains atoms of oxygen. c. The sample contains molecules. d. None of the above is correct. 2. What is the volume occupied by a 8.00 gram sample of molecular oxygen at STP? a L c L b L d L 3. Standard temperature and pressure are which of the following? a. 0 C and 1 atm c. 273 K and 1 atm b. 32 F and 1 atm d. all of these 4. Which of the following is a mathematical statement of the ideal gas law? a. PV = n/rt c. V = np/rt b. PV = nrt d. PV = RT/n 5. A vessel under atm pressure contains nitrogen, N 2, and water vapor, H 2 O. The partial pressure of N 2 is atm. What is the partial pressure of the water vapor? a atm c atm b atm d atm 6. According to the kinetic molecular theory, which of the following is not true? a. The average kinetic energy of gas particles is proportional to the Celsius temperature. b. Gas molecules are assumed to have no volume. c. Gas pressure is caused by collisions between gas molecules and the container walls. d. None, all of the above are true. 7. The term solution is synonymous with which of the following? a. compound c. heterogeneous mixture b. element d. homogeneous mixture 8. Which of the following cannot serve as a solvent in a solution? a. a gas c. a solid b. a liquid d. None, all can serve as solvents. 9. A student is preparing a sugar water solution to make rock candy. When the student continues to add sugar to the solution the sugar dissolves. Which kind of solution does the student have? a. a saturated solution c. an unsaturated solution b. a supersaturated solution d. We cannot tell. 10. When considering the solubility of a particular solute in a particular solvent the term like dissolves like generally refers to which of the following properties? a. formula weight c. both a and b b. molecular polarity d. neither a nor b 11. Water is generally a good solvent for which of the following types of compounds? a. nonpolar compounds c. both a and b b. polar compounds d. neither a nor b
2 12. Which of the following is true regarding the solubility of gases? a. Solubility always decreases as pressure increases. b. Solubility always increases as pressure increases. c. Solubility usually decreases as pressure increases. d. Solubility usually increases as pressure increases. 13. Which of the following is the definition of molarity? a. moles of solute/1000 grams of solvent b. moles of solute/liter of solution c. moles of solute/liter of solvent d. moles of solvent/1000 grams of solute 14. If we wish to prepare 250. ml of M BaCl 2, how much solid is BaCl 2 is needed? a g c g b g d g 15. If we wish to prepare a 0.50 M solution of NaCl, how much water must be added to 1.0 mole of NaCl? a. 2.0 mol b. 2.0 L c g d. Enough water to make 2.0 L of solution. 16. What is the mass of NaCl in a L bottle of 2.00 M NaCl? a g c. 117 g b g d. 234 g 17. Which of the following solutions will have the higher electrical conductivity? a. 0.1 M NaCl c. Both a and b have the same conductivity. b. 0.2 M NaCl d. Neither conducts electricity. 18. Which of the following is true of methanol, CH 3 OH, when it dissolves in water? a. It dissociates into ions. b. It forms covalent bonds with water. c. It forms hydrogen bonds with water. d. None of the above, methanol does not dissolve in water. 19. Water is likely to be a poor solvent for which types of molecules? a. molecules which can form hydrogen bonds b. nonpolar molecules c. polar molecules d. None, water is considered a universal solvent. 20. Thermal pollution generally means refers to which of the following? a. the decrease in the O 2 content of warm water as compared to cold water b. the increase in the O 2 content of cold water as compared to warm water c. both a and b d. neither a nor b 21. A certain wine contains M NaHSO 3 as a preservative. What mass of NaHSO 3 is in a 750 ml bottle of this wine? a g c g b g d. 1.5 g 22. How many moles of solute are contained in 500. ml of 0.50 M KCl? a c. 1.0 b d. 2.0
3 23. What volume of 12.0 M HCl must be used to make 300. ml of M HCl? a ml c ml b ml d ml 24. Which of the following is true of electrolytes? a. All electrolytes have mobile ions. b. All electrolytes contain equal numbers of cations and anions. c. both a and b d. neither a nor b 25. Which of the following is true of all strong electrolytes? a. They are all ionic compounds. c. both a and b b. They all dissociate completely. d. neither a nor b Consider the following graph. 26. Approximately what mass of A will dissolve in 100 ml of water at 75 C? a. 25 g c. 55 g b. 40 g d. 70 g 27. Which substance exhibits solubility behavior that is similar to that of a gas? a. A b. B c. C d. None of the substances listed show this behavior. 28. Which of the following generally occurs as temperature increases? a. Solubility of a solid solute decreases. b. Solubility of a solid solute increases. c. Solubility of a solid solute remains the same. d. Molarity of a solid solute doubles. 29. Oxygen in nitrogen is an example of which solute-solvent combination? a. gas-liquid c. gas-solid b. liquid-gas d. gas-gas
4 30. Convert the pressure 2.50 atm to kpa. a. 1 kpa c. 760 kpa b. 253 kpa d kpa 31. Which of the following compounds is insoluble in water? a. CaCO 3 c. Ca(NO 3 ) 2 b. CaCl 2 d. Ca(C 2 H 3 O 2 ) When a solution of ammonium chloride, NH 4 Cl, is added to a solution of lead(ii) nitrate, Pb(NO 3 ) 2, a white precipitate of lead chloride, PbCl 2, forms. Which of the following is the total ionic equation for this reaction? a. 2 NH 4 Cl(aq) + Pb(NO 3 ) 2 (aq) PbCl 2 (s) + 2 NH 4 NO 3 (aq) b. 2 NH + 4 (aq) + 2 Cl-(aq) + Pb 2+ (aq) + 2 NO 3 -(aq) PbCl 2 (s) + 2 NH + 4 (aq) + 2 NO 3 -(aq) c. Pb 2+ (aq) + 2 Cl-(aq) PbCl 2 (s) d. Pb 2+ (aq) + Cl 2 2 -(aq) PbCl 2 (s) 33.Which of the following sulfides is soluble in water? a. Ag 2 S c. K 2 S b. FeS d. PbS Part II. Short Answer. Please show all work. Only one point will be given for the correct answer. Make sure all calculated values have units written after the number and are reported to the correct number of significant digits. Equations are given below: M 1 V 1 = M 2 V 2 P 1 V 1 = P 2 V 2 PV = nrt molarity, M = n/v T 1 T 2 R = L atm/mol K 1 kg = 1000g 1 L = 1000 ml 1 atm = 760 torr = 760 mmhg = kpa K = C A diver at a depth of 20 m inhales 0.50 L of an air mixture at a pressure of kpa. If the diver holds his breath and quickly swims to the surface where the pressure is 1.00 atm, calculate the new volume of air in his lungs. Explain why doing this would be dangerous. Assume conditions of constant temperature. 2. What is the molarity of 5.00 g of potassium chloride in ml of solution?
5 3. How much concentrated hydrochloric acid (12.4 M) would be needed to prepare ml of 3.00 M hydrochloric acid? 4. If you were to take a volleyball scuba diving with you what would be its new volume if it started at the surface with a volume of 2.00L, under a pressure of mmhg and a temperature of 20.0 C? On your dive you take it to a place where the pressure is 2943 mmhg, and the temperature is C. 5. A 10.0 gram chunk of dry ice (solid CO 2 ) changes to gas. What is the volume of that gas measured at 27 C and 740 mmhg? 6. If 10.0 ml of mol/l HCl (aq) react exactly with 12.0 ml of Ba(OH) 2(aq), find the molar concentration of the barium hydroxide solution. 7. If ml of mol/l AgNO 3 completely reacts with copper, what mass of silver will be produced?
6 8. A solution of ml of M KOH solution is added to ml of a M nickel (II) nitrate solution. a. Write the balanced chemical equation for the reaction that occurs. b. What precipitate forms? c. What is the limiting reactant? d. How many grams of the precipitate form?
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A solution containing a large concentration of dissolved ions can be classified as a(n).
More informationChemistry 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 informationName: 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 informationc. K 2 CO 3 d. (NH 4 ) 2 SO 4 Answer c
Chem 130 Name Exam 2, Ch 4-6 July 7, 2016 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units and
More informationName Date Class PROPERTIES OF SOLUTIONS
16.1 PROPERTIES OF SOLUTIONS Section Review Objectives Identify the factors that determine the rate at which a solute dissolves Identify the units usually used to express the solubility of a solute Calculate
More informationExam 1, Ch October 12, Points
Chem 130 Name Exam 1, Ch 46.7 October 12, 2018 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units
More informationUNIT 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 information3. Which of the following compounds is soluble? The solubility rules are listed on page 8.
1. Classify the following reaction. Sb 2 O 3 + 3 Fe 2 Sb + 3 FeO a) Combination reaction b) Decomposition reaction c) Neutralization reaction d) Single-replacement reaction e) Double-replacement reaction
More informationExplain 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"It s not that I m so smart, it s just that I stay with problems longer." --Albert Einstein--
CHEMISTRY 101 Hour Exam II October 29, 2013 Adams/Lindquist Name Signature Section "It s not that I m so smart, it s just that I stay with problems longer." --Albert Einstein-- This exam contains 17 questions
More information5. Which barium salt is insoluble in water? (1) BaCO3 (3) Ba(ClO4)2 (2) BaCl2 (4) Ba(NO3)2
1. A 3.0 M HCl(aq) solution contains a total of (1) 3.0 grams of HCl per liter of water (2) 3.0 grams of HCl per mole of solution (3) 3.0 moles of HCl per liter of solution (4) 3.0 moles of HCl per mole
More informationResearch tells us fourteen out of any ten individuals like chocolate. Happy Halloween!
CHEMISTRY 101 Hour Exam II October 31, 2006 Adams/Le Name KEY Signature T.A./Section Research tells us fourteen out of any ten individuals like chocolate. Happy Halloween! This exam contains 17 questions
More informationThe solvent is the dissolving agent -- i.e., the most abundant component of the solution
SOLUTIONS Definitions A solution is a system in which one or more substances are homogeneously mixed or dissolved in another substance homogeneous mixture -- uniform appearance -- similar properties throughout
More informationCHEM 101A EXAM 1 SOLUTIONS TO VERSION 1
CHEM 101A EXAM 1 SOLUTIONS TO VERSION 1 Multiple-choice questions (3 points each): Write the letter of the best answer on the line beside the question. Give only one answer for each question. B 1) If 0.1
More informationWater & Solutions Chapter 17 & 18 Assignment & Problem Set
Water & Solutions Chapter 17 & 18 Assignment & Problem Set Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Water & Solutions 2 Vocabulary (know
More informationGravimetric Analysis (Analysis by Mass)
Week 2 Measuring water content Gravimetric Analysis (Analysis by Mass Water is a component in many consumer products It may occur naturally or may be added in manufacturing Water content can reveal the
More informationCHAPTER 8 CHEMICAL REACTIONS AND EQUATIONS
CHAPTER 8 CHEMICAL REACTIONS AND EQUATIONS CHEMICAL REACTIONS Occurs when matter combines or breaks apart to produce new kinds of matter with different properties with a change in energy. EVIDENCE FOR
More informationACP Chemistry (821) - Mid-Year Review
ACP Chemistry (821) - Mid-Year Review *Be sure you understand the concepts involved in each question. Do not simply memorize facts!* 1. What is chemistry? Chapter 1: Chemistry 2. What is the difference
More informationChem 1411 Practice Exam 2
Chem 1411 Practice Exam 2 Instructions 1. Write your name on your exam. 2. You may use only the scratch paper and periodic table provided with the exam. You may also use a calculator, provided it cannot
More informationChem 1411 Practice Exam 2
Chem 1411 Practice Exam 2 Instructions 1. Write your name on your exam. 2. You may use only the scratch paper and periodic table provided with the exam. You may also use a calculator, provided it cannot
More informationSolutions CHAPTER OUTLINE
Chapter 8A Solutions 1 CHAPTER OUTLINE Type of Solutions Electrolytes & Nonelectrolytes Equivalents of Electrolytes Solubility & Saturation Soluble & Insoluble Salts Formation of a Solid Precipitation
More informationExam 2, Ch 4-6 October 12, Points
Chem 130 Name Exam 2, Ch 4-6 October 12, 2016 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units
More information100 C = 100 X = X = 218 g will fit in this solution. 25 C = 100 X = 3640 X = 36.4 g will fit in this solution.
58 Questions for Solutions - You should be able to do ALL of these problems. Use a calculator, write all formulas, watch SF, and find the answers online at Arbuiso.com on the SOLUTIONS page. This is great
More informationSettling? 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 informationChapter 12 & 13 Test Review. Bond, Ionic Bond
Chapter 12 & 13 Test Review A solid solute dissolved in a solid solvent is an Alloy What is happening in a solution at equilibrium? The Ionic rate of Bond dissolving is equal to the rate of crystallization.
More informationChemistry 20 Lesson 36 The Whole Enchilada
Unit I: Science 10 Review Chemistry 20 Lesson 36 The Whole Enchilada 1. Classify the substances as ionic (i), molecular (m), or acid (a) and provide the IUPAC name and the state of matter at SATP where
More information4 CO O 2. , how many moles of KCl will be produced? Use the unbalanced equation below: PbCl 2. PbSO 4
Honors Chemistry Practice Final 2017 KEY 1. Acetylene gas, C 2, is used in welding because it generates an extremely hot flame when combusted with oxygen. How many moles of oxygen are required to react
More informationChem 12: Chapters 10, 11, 12, 13, 14 Unit 3 Worksheet
C h e m i s t r y 1 2 U n i t 3 R e v i e w P a g e 1 Chem 12: Chapters 10, 11, 12, 13, 14 Unit 3 Worksheet 1. What is miscible? Immiscible? 2. What is saturated? Unsaturated? Supersaturated? 3. How does
More informationCHM1045 Exam 2 Chapters 3, 4, & 10
1. Upon analysis, a compound is found to contain 22.8% sodium, 21.8% boron, and 55.4% oxygen. What is its empirical formula? a. NaBO b. NaB 2 O 5 c. Na 2 B 4 O 7 d. Na 3 BO 4 e. None of the above. 2. The
More informationSOLUTIONS. Solutions - page
SOLUTIONS For gases in a liquid, as the temperature goes up the solubility goes. For gases in a liquid, as the pressure goes up the solubility goes. Example: What is the molarity of a solution with 2.0
More informationReview 7: Solubility Equilibria
Review 7: Solubility Equilibria Objectives: 1. Be able to write dissociation equations for ionic compounds dissolving in water. 2. Given Ksp, be able to determine the solubility of a substance in both
More informationI. Properties of Aqueous Solutions A) Electrolytes and Non-Electrolytes B) Predicting Solubility* II. Reactions of Ionic Compounds in Solution*
Chapter 5 Reactions in Aqueous Solutions Titrations Kick Acid!!! 1 I. Properties of Aqueous Solutions A) Electrolytes and Non-Electrolytes B) Predicting Solubility* II. Reactions of Ionic Compounds in
More informationQuick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent
Quick Review - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent Water H 2 O Is water an ionic or a covalent compound? Covalent,
More informationM = Molarity = mol solute L solution. PV = nrt % yield = actual yield x 100 theoretical yield. PM=dRT where d=density, M=molar mass
Solubility Rules: 1. Most nitrate salts are soluble. 2. Most salts of alkali metals and ammonium cations are soluble. 3. Most chloride, bromide and iodide salts are soluble. Exceptions: salts containing
More informationBrass, 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(A) Composition (B) Decomposition (C) Single replacement (D) Double replacement: Acid-base (E) Combustion
AP Chemistry - Problem Drill 08: Chemical Reactions No. 1 of 10 1. What type is the following reaction: H 2 CO 3 (aq) + Ca(OH) 2 (aq) CaCO 3 (aq) + 2 H 2 O (l)? (A) Composition (B) Decomposition (C) Single
More informationIB Chemistry Solutions Gasses and Energy
Solutions A solution is a homogeneous mixture it looks like one substance. An aqueous solution will be a clear mixture with only one visible phase. Be careful with the definitions of clear and colourless.
More informationChapter 4. Aqueous Reactions and Solution Stoichiometry
Sample Exercise 4.1 (p. 127) The diagram below represents an aqueous solution of one of the following compounds: MgCl 2, KCl, or K 2 SO 4. Which solution does it best represent? Practice Exercise 1 (4.1)
More informationChapter 4 Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Homework Chapter 4 11, 15, 21, 23, 27, 29, 35, 41, 45, 47, 51, 55, 57, 61, 63, 73, 75, 81, 85 1 2 Chapter Objectives Solution To understand the nature of ionic substances
More information"No matter what costume you wear, when you start eating Halloween candy, you will be a goblin. - Unknown
CHEMISTRY 101 Hour Exam II October 31, 2017 Andino/McCarren Name Signature Section "No matter what costume you wear, when you start eating Halloween candy, you will be a goblin. - Unknown This exam contains
More informationGas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T
Name Period Teacher Practice Test: OTHS Academic Chemistry Spring Semester 2017 The exam will have 100 multiple choice questions (1 point each) Formula sheet (see below) and Periodic table will be provided
More informationChemistry 20 Unit 3A Solutions FITB Notes. Topic A Classification of Solutions
Chemistry 20 Unit 3A Solutions FITB Notes General Outcome: Topic A Classification of Solutions Matter is a substance with and A substance is a type of matter with one definite formula (elements, compounds)
More informationPart 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 informationCP 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 informationChemistry 51 Chapter 8 TYPES OF SOLUTIONS. Some Examples of Solutions. Type Example Solute Solvent Gas in gas Air Oxygen (gas) Nitrogen (gas)
TYPES OF SOLUTIONS A solution is a homogeneous mixture of two substances: a solute and a solvent. Solute: substance being dissolved; present in lesser amount. Solvent: substance doing the dissolving; present
More informationmolality: m = = 1.70 m
C h e m i s t r y 1 2 U n i t 3 R e v i e w P a g e 1 Chem 12: Chapters 10, 11, 12, 13, 14 Unit 3 Worksheet 1. What is miscible? Immiscible? Miscible: two or more substances blend together for form a solution
More informationDuring photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:
Example 4.1 Stoichiometry During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Suppose that a particular plant consumes 37.8 g of CO 2
More informationOH (ammonium hydroxide) are in 3.47 moles of NH 4. OH? 1 grams. 2 Na(s) + Cl 2. (g) 2 NaCl(s) (32.00 g/mol) according to the reaction C 3
Question #: 1 Posting ID: 423347 Course: CHE 105 2015 SU Instructor: Sarah Edwards How many grams of NH 4 OH (ammonium hydroxide) are in 3.47 moles of NH 4 OH? 1 grams Question #: 2 When 2.61 grams of
More informationCST Review Part 2. Liquid. Gas. 2. How many protons and electrons do the following atoms have?
CST Review Part 2 1. In the phase diagram, correctly label the x-axis and the triple point write the names of all six phases transitions in the arrows provided. Liquid Pressure (ATM) Solid Gas 2. How many
More informationSolutions. Heterogenous Mixture (Not a Solution) Ice Water (w/ Ice Cubes) Smog Oil and Water
Solutions Unit 6 1 Solutions Homogenous Mixture (Solution) two or more substances mixed together to have a uniform composition, its components are not distinguishable from one another Heterogenous Mixture
More information2. If a gas is released in a reaction (ex: Hydrogen gas bubbles off), is it written as a reactant or a product?
PRE-AP CHEMISTRY SPRING FINAL EXAM REVIEW Name _ Period Exam Date 100% COMPLETION OF THIS REVIEW BY THE DAY OF YOUR FINAL EXAM WILL COUNT AS A 5 POINT BONUS ADDED TO YOUR FINAL EXAM SCORE. THERE WILL BE
More informationName 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 informationMoorpark College Chemistry 11 Fall 2011 Instructor: Professor Gopal. Examination #2: Section Two October 17, Name: (print)
Moorpark College Chemistry 11 Fall 2011 Instructor: Professor Gopal Examination #2: Section Two October 17, 2011 Name: (print) Directions: Make sure your examination contains ELEVEN total pages (including
More informationName 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 informationStoichiometry. Percent composition Part / whole x 100 = %
Stoichiometry Conversion factors 1 mole = 6.02 x 10 23 atoms (element) 1 mole = 6.02 x 10 23 molecules (covalent compounds) 1 mole = 6.02 x 10 23 formula units (ionic compounds) 1 mole (any gas @ STP)
More informationName. Practice Test 2 Chemistry 111
Name Practice Test 2 Chemistry 111 1) In the aqueous reaction of K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) BaSO 4 (s) + 2KNO 3 (aq), which ions are the spectator ions? A) Ba 2+ 2- and SO 4 B) Ba 2+ and K + C) Ba
More informationGeneral Chemistry 1 CHM201 Unit 2 Practice Test
General Chemistry 1 CHM201 Unit 2 Practice Test 1. Which statement about the combustion of propane (C 3H 8) is not correct? C 3H 8 5O 2 3CO 2 4H 2O a. For every propane molecule consumed, three molecules
More informationSolutions. 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 information1. Balance the following chemical equations: a. C 8 H 18 + O 2 à CO 2 + H 2 O. b. B 5 H 9 + O 2 à B 2 O 3 + H 2 O. c. S 8 + Cl 2 à S 2 Cl 2
EXAM 2 PRACTICE QUESTIONS NOTE- THIS IS ONLY A SELECTION OF POSSIBLE TYPES OF QUESTIONS: REFER TO THE EXAM 2 REVIEW GUIDELINES FOR THE LIST OF LEARNING TARGETS. There will likely be other questions on
More informationUnit Two Worksheet WS DC U2
Unit Two Worksheet WS DC U2 Name Period Short Answer [Writing]. Write skeleton equations representing the following reactions and then balance them. Then identify the reaction type. Include all needed
More informationThe 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 informationChemistry. 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 informationLesson Plans Chapter 15: Solutions & Solution Chemistry
Lesson Plans Chapter 15: Solutions & Solution Chemistry I. Solutions a. A solution is simply a homogeneous mixture i. Homogeneous: same throughout (it does not mean one ) ex: water + sugar, air, alloys,
More informationCHEMISTRY 202 Hour Exam I. Dr. D. DeCoste T.A.
CHEMISTRY 0 Hour Exam I September, 016 Dr. D. DeCoste Name Signature T.A. This exam contains 3 questions on 11 numbered pages. Check now to make sure you have a complete exam. You have two hours to complete
More informationUnit 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 informationMolecule smallest particle of a substance having its chemical properties Atoms connected via covalent bonds Examples:
Ionic equations, calculations involving concentrations, stoichiometry MUDr. Jan Pláteník, PhD Molecule smallest particle of a substance having its chemical properties Atoms connected via covalent bonds
More informationChapter 3: Solution Chemistry (For best results when printing these notes, use the pdf version of this file)
Chapter 3: Solution Chemistry (For best results when printing these notes, use the pdf version of this file) Section 3.1: Solubility Rules (For Ionic Compounds in Water) Section 3.1.1: Introduction Solubility
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Oxidation is the and reduction is the. A) loss of oxygen, gain of electrons B) gain of
More information2 nd Semester Study Guide 2016
Chemistry 2 nd Semester Study Guide 2016 Name: Unit 6: Chemical Reactions and Balancing 1. Draw the remaining product 2. Write a balanced equation for the following reaction: The reaction between sodium
More informationChemistry 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 informationTest Booklet. Subject: SC, Grade: HS 2008 Grade High School Chemistry. Student name:
Test Booklet Subject: SC, Grade: HS 2008 Grade High School Chemistry Student name: Author: North Carolina District: North Carolina Released Tests Printed: Tuesday July 17, 2012 1 How many protons and electrons
More informationCHEMISTRY 110 EXAM 3 NOVEMER 12, 2012 FORM A
CHEMISTRY 110 EXAM 3 NOVEMER 12, 2012 FORM A 1. Consider a balloon filled with 5 L of an ideal gas at 20 C. If the temperature of the balloon is increased by 70 C and the external pressure acting on the
More informationWhat type of solution that contains all of the
What type of solution that contains all of the solute it can hold at a given temperature? Saturated Solution What type of solution that contains less solute than it is able to hold at a given temperature?
More informationPractice questions for Chapter 4
Practice questions for Chapter 4 1. An unknown substance dissolves readily in water but not in benzene (a nonpolar solvent). Molecules of what type are present in the substance? A) neither polar nor nonpolar
More informationUnit 10: Solutions and Solubility REGENTS CHEMISTRY
Name: Unit 10: Solutions and Solubility REGENTS CHEMISTRY 1 Name: Unit 10: Solutions and Solubility Matter is classified as a pure substance or as a mixture of substances. (3.1q) Mixtures are composed
More informationChapter 8 Chemical Reactions
Chemistry/ PEP Name: Date: Chapter 8 Chemical Reactions Chapter 8: 1 7, 9 18, 20, 21, 24 26, 29 31, 46, 55, 69 Practice Problems 1. Write a skeleton equation for each chemical reaction. Include the appropriate
More informationUNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12)
I. Multiple Choice UNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12) 1) Which one of the following would form an ionic solution when dissolved in water? A. I 2 C. Ca(NO 3 ) 2 B. CH 3 OH D.
More informationName 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 informationUnit 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 informationChem 1100 Pre-Test 3. Multiple Choice Identify the choice that best completes the statement or answers the question.
Chem 1100 Pre-Test 3 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Determine the oxidation number of the underlined element in K 2CO 3. a. 1 b. 2 c.
More informationed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. Sunday, August 18, 13
ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. A solution is a homogenous mixture of 2 or more substances at the molecular level The solute(s) is(are)
More informationMixtures. 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 information2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with
Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12
More informationChapter 17. Additional Aspects of Equilibrium
Chapter 17. Additional Aspects of Equilibrium Sample Exercise 17.1 (p. 726) What is the ph of a 0.30 M solution of acetic acid? Be sure to use a RICE table, even though you may not need it. (2.63) What
More informationCHEMISTRY 102 A/E Fall 2008 HOUR EXAM I NAME Dr. Christine Yerkes. A. DO NOT open the exam until you are instructed to do so.
CHEMISTRY 102 A/E Fall 2008 HOUR EXAM I NAME Dr. Christine Yerkes October 1, 2008 SIGNATURE Test Form A QUIZ TA A. DO NOT open the exam until you are instructed to do so. B. The exam has 6 pages. After
More informationSolubility Rules See also Table 4.1 in text and Appendix G in Lab Manual
Ch 4 Chemical Reactions Ionic Theory of Solutions - Ionic substances produce freely moving ions when dissolved in water, and the ions carry electric current. (S. Arrhenius, 1884) - An electrolyte is a
More informationGive 6 different types of solutions, with an example of each.
Warm up (Jan 5) Give 6 different types of solutions, with an example of each. 1 Warm Up (Jan 6) 1. Write the reaction showing the dissolving of the following solids (be sure to note whether they are covalent
More informationTake Home Semester 2 Practice Test for Acc Chem MM 15-16
Take Home Semester 2 Practice Test for Acc Chem MM 15-16 Thermochemistry 1. Determine ΔHrxn. 2SO2(g) + O2(g) 2SO3(g) a) 98.9 b) 98.9 c) 197.8 d) 197.8 ΔHf o SO2(g) 296.8 kj/mol SO3(g) 395.7 kj/mol O2(g)
More informationReactions in Aqueous Solutions
Copyright 2004 by houghton Mifflin Company. Reactions in Aqueous Solutions Chapter 7 All rights reserved. 1 7.1 Predicting if a Rxn Will Occur When chemicals are mixed and one of these driving forces can
More informationUnit 6 ~ Learning Guide Name:
Unit 6 ~ Learning Guide Name: Instructions: Using a pencil, complete the following notes as you work through the related lessons. Show ALL work as is explained in the lessons. You are required to have
More informationWe CAN have molecular solutions (ex. sugar in water) but we will be only working with ionic solutions for this unit.
Solubility Equilibrium The Basics (should be mostly review) Solubility is defined as the maximum amount of a substance which can be dissolved in a given solute at a given temperature. The solubility of
More informationChapter 15. Solutions
Chapter 15 Solutions Key Terms for this Chapter Make sure you know the meaning of these: Solution Solute Solvent Aqueous solution Solubility Saturated Unsaturated Supersaturated Concentrated Dilute 15-2
More informationChem 101 Practice Exam 3 Fall 2012 You will have a Solubility Table and Periodic Table
Chem 101 Practice Exam Fall 01 You will have a Solubility Table and Periodic Table 1. A 1.6-mol sample of KClO was decomposed according to the equation KClO (s) KCl(s) O (g) How many moles of O are formed
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
More informationTOPICS TO BE COVERED 1. WHAT ARE SOLUTIONS? 2. SOLVENTS AND SOLUTES 3. SOLUBILITY AND ITS FACTORS 4. CONCENTRATIONS 5. SOLUTION STOICHIOMETRY 6.
TOPICS TO BE COVERED 1. WHAT ARE SOLUTIONS? 2. SOLVENTS AND SOLUTES 3. SOLUBILITY AND ITS FACTORS 4. CONCENTRATIONS 5. SOLUTION STOICHIOMETRY 6. COLLIGATIVE PROPERTIES SOLUTIONS CHEMICALS + WATER 1. WHAT
More informationCHEMISTRY 102B Practice Hour Exam I. Dr. D. DeCoste T.A (30 pts.) 16 (15 pts.) 17 (15 pts.) Total (60 pts)
CHEMISTRY 102B Practice Hour Exam I Spring 2016 Dr. D. DeCoste Name Signature T.A. This exam contains 17 questions on 5 numbered pages. Check now to make sure you have a complete exam. You have one hour
More informationCHAPTER 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 informationChapter 4: Types of Chemical Reactions and Solution Stoichiometry
Chapter 4: Types of Chemical Reactions and Solution Stoichiometry 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition of Solutions (MOLARITY!)
More informationReactions in aqueous solutions Precipitation Reactions
Reactions in aqueous solutions Precipitation Reactions Aqueous solutions Chemical reactions that occur in water are responsible for creation of cenotes. When carbon dioxide, CO2, dissolves in water, the
More informationSPRING 2017 CHEMISTRY FINAL EXAM REVIEW
SPRING 2017 CHEMISTRY FINAL EXAM REVIEW Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. BONDING What is the formula for diphosphorus pentaoxide?
More information