1. The rate of decomposition of HI into its diatomic elements is 5.0 x 10 3 mole/l s. What is the rate of formation of hydrogen in the same reaction?
|
|
|
- Eustace Bridges
- 5 years ago
- Views:
Transcription
1 1. The rate of decomposition of HI into its diatomic elements is 5.0 x 10 3 mole/l s. What is the rate of formation of hydrogen in the same reaction? 2. Butene, decomposes to ethylene according to C4H8(g) 2 C2H4(g) The following data were collected as a function of time [C 4 H 8 ] (M) Time (s) a. Estimate the instantaneous rate of decomposition of C4H8 at 75 s. b. Estimate the instantaneous rate of formation of C2H4 at 75 s.
2 3. Aspirin (I) hydrolyzes in the body to the active form, salicylic acid (II), and acetic acid (III). H O O O O H O CH 3 O H H O CH 3 O O + H2O(l) + I II III The following data were collected as a function of time [aspirin] (M) Time (s) a. Estimate the instantaneous rate of hydrolysis of aspirin at 100 s. b. Estimate the instantaneous rate of formation of salicylic acid at 100 s.
3 4. Initial rate data for 2 HgCl2(aq) + C2O4 2 (aq) 2 Cl (aq) + 2 CO2(g) + Hg2Cl2(s) are tabulated below: Exp# [HgCl2]i, M [C2O4 2 ]i, M Initial rate, M/s x x x ? a. Write the rate law for the reaction. b. What is the order of the reaction in oxalate ion? c. Calculate the numerical value of the rate constant. d. Calculate the rate of experiment #4. f. What function of [HgCl2], when plotted versus time, would give a straight line?
4 5. Initial rate data for 2 NO(g) + Cl2(g) 2 NOCl(g) are tabulated below: Exp# [NO]i, M [Cl2]i, M Initial rate, M/s x x x ? a. Write the rate law for the reaction. b. What is the overall order of the reaction? c. Calculate the numerical value of the rate constant. d. Calculate the rate of experiment #4. f. What function of [NO], when plotted versus time, would give a straight line?
5 6. The integrated forms of the rate laws for 0 th, 1 st, and 2 nd order reactions all contain k. What would be the units for k in each expression. If nescessary, use the time unit seconds (s). 7. A temperature increase from 10.0 to 20.0 ºC doubles the rate of a reaction, calculate Ea. 8. Given, H2(g) + 2 BF3(g) + N2H4(g) 2 F3BNH3(g) Sketch the clearly labeled (approximately to scale) reaction profile if ΔH = 2.71 kj and Ea = J.
6 9. The rate constant of the following reaction was studied as a function of temperature: NO(g) + O3(g) NO2(g) + O2(g) Exp# Temperature (ºC) k (L/mole s) x x x x x Plot the proper function of the data to determine the activation energy, Ea.
7 10. A proposed mechanism for: is NO2(g) + CO(g) NO(g) + CO2(g) k NO2 NO3 + NO (slow) 2. NO3 + CO NO + CO2 k2 What is the testable rate law for the reaction?
8 12. a. Write the equilibrium constant expression for the reaction, CS2(g) + 4 H2(g) CH4(g) + 2 H2S(g) b. A flask is filled with M (each) of CS2, CH4, and H2S and heated to 960 ºC. At equilibrium, the concentration of H2S is measured to be M. Calculate the value of K for this reaction at 960 ºC. c. Using the equilibrium constant calculated for the above reaction (in b), determine the value of K, at 960 ºC, of the following: CH4(g) + 2 H2S(g) CS2(g) + 4 H2(g) ½ CS2(g) + 2 H2(g) ½ CH4(g) + H2S(g) 3 CH4(g) + 6 H2S(g) 3 CS2(g) + 12 H2(g) d. Using the equilibrium constant calculated in b, calculate the value of KP for this reaction.
9 13. An analysis of the decomposition at 340 o C, PCl5(g) PCl3(g) + Cl2(g) shows that at one instant PCl5, PCl3 and Cl2 are present in equal concentrations of M. a. Given an equilibrium constant of at 340 o C, is the reaction mixture moving towards products, toward reactant or is it at equilibrium? b. If the reaction is not at equilibrium, determine the equilibrium concentration of each component at 340 o C.
10 14. A mixture of hydrogen, iodine and hydrogen iodide, each at a concentration of M, is introduced into a container heated to 490 ºC. H2(g) + I2(g) 2 HI(g) K = 46 a. Predict the direction that the reaction goes to reach equilibrium.. b. Calculate the equilibrium concentrations of all three species. 15. Using Le Châtelier Principle, predict which direction (left, right, or no change) the reaction below will go if the following occurs. Explain, briefly. 4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g) ΔH = kj a. Nitrogen monoxide is added to the vessel. b. The pressure in the vessel is increased. c. The reaction is cooled. d. Xenon gas is pumped into the reaction vessel.
11 16. What is the hydroxide ion concentration of a solution that has a ph of 4.56? 17. Calculate the ph of the following. Show an appropriate chemical equation of each. a. 1.2 x 10 3 M HI b M Sr(OH)2 c M HCHO2
12 d M hydrazine e M sodium perchlorate f M lithium pyruvate g M dimethylammonium bromide
CHM 112 Chapter 13 Extra Credit : Chemical Equilibrium Name:
CHM 112 Chapter 13 Extra Credit : Chemical Equilibrium Name: 1. Write the equilibrium expression for following reactions. In each case indicate whether the equilibrium is Homogeneous or Heterogeneous 2
CHEMICAL EQUILIBRIUM. Chapter 15
Chapter 15 P a g e 1 CHEMICAL EQUILIBRIUM Examples of Dynamic Equilibrium Vapor above a liquid is in equilibrium with the liquid phase. rate of evaporation = rate of condensation Saturated solutions rate
Name Chem 6 Section #
Equilibrium Constant and its Meaning 1. Write the expressions for K eq for the following reactions. a) CH 4 (g) + 2 H 2 S(g) CS 2 (g) + 4 H 2 (g) b) 2 N 2 O 5 (g) 4 NO 2 (g) + O 2 (g) c) 3 O 2 (g) 2 O
Write equilibrium law expressions from balanced chemical equations for heterogeneous and homogeneous systems. Include: mass action expression.
Equilibrium 1 UNIT 3: EQUILIBRIUM OUTCOMES All important vocabulary is in Italics and bold. Relate the concept of equilibrium to physical and chemical systems. Include: conditions necessary to achieve
91166 Demonstrate understanding of chemical reactivity Collated questions on equilibria
(2017:2) 91166 Demonstrate understanding of chemical reactivity Collated questions on equilibria The addition of a small amount of iron to a mixture of nitrogen and hydrogen gases helps to speed up the
CHEM 122 CHEMICAL EQUILIBRIUM CHAP 15 ASSIGN
CHEM 122 CHEMICAL EQUILIBRIUM CHAP 15 ASSIGN PLACE THE LETTER REPRESENTING THE BEST ANSWER TO EACH QUESTION ON THE APPROPRIATE LINE ON THE ANSWER SHEET. FOR OTHER QUESTIONS, CLEARLY WRITE THE ANSWER, INCLUDING
Equilibrium means that the rxn rates are equal. evaporation H20(l) condensation
Reversible reactions Most chemical reactions are reversible they can occur backwards as well as forwards reactants products Consider an open container of water (non-equilibrium) A closed water bottle is
Unit 8: Equilibrium Unit Review
1. Predict the effect of increasing pressure on the position of equilibrium in the following systems: a. CH 4 (g) + 2H 2 O(g) CO 2 (g) + 4H 2 (g) b. N 2 O 5 (g) + NO(g) 3NO 2 (g) c. NO(g) + NO 2 (g) N
1) Define the following terms: a) catalyst; b) half-life; c) reaction intermediate
Problems - Chapter 19 (without solutions) 1) Define the following terms: a) catalyst; b) half-life; c) reaction intermediate 2) (19.10) Write the reaction rate expressions for the following reactions in
6.5 x 10 M/s. t ( ) s
1. Iodide ion can be oxidized by iodate ion to triiodide ion: IO3 (aq) + 8 I (aq) + 6 H + (aq) 3 I3 (aq) + 3 H2O(l) a. Using the data from the graph above, estimate the instantaneous rate of formation
Quiz B3: Le Chatelier s Principle Block:
Quiz B3: Le Chatelier s Principle Name: Block: 1. Consider the following reaction: 2SO2(g) + O2(g) 2SO3(g) H = -197 kj/mol Which of the following will not shift the equilibrium to the right? A. Adding
Chapter 13: Chemical Equilibrium
Chapter 13: Chemical Equilibrium May 5 2:04 PM 13.1 The Equilibrium Condition When you finish this section you will be able to list some characteristics of reactions at equilibrium. Chemical equilibrium
Downloaded from
IMPORTANT POINTS (EQUILLIBRIUM) IMPORTANT QUESTIONS CHAPTER EQUILIBRIUM 1. Equilibrium constant helps in predicting the direction in which a given reaction will proceed at any stage. a) In which one of
1.6 Chemical equilibria and Le Chatelier s principle
1.6 Chemical equilibria and Le Chatelier s principle Reversible reactions: Consider the reaction: Mg(s) + H2SO4(aq) MgSO4(aq) + H2(g) The reaction stops when all of the limiting reagent has been used up.
a. rate = k[no] 2 b. rate = k([no][o 2 ] c. rate = k[no 2 ] 2 [NO] -2 [O 2 ] -1/2 d. rate = k[no] 2 [O 2 ] 2 e. rate = k([no][o 2 ]) 2
![a. rate = k[no] 2 b. rate = k([no][o 2 ] c. rate = k[no 2 ] 2 [NO] -2 [O 2 ] -1/2 d. rate = k[no] 2 [O 2 ] 2 e. rate = k([no][o 2 ]) 2](/thumbs/82/85645750.jpg "a. rate = k[no] 2 b. rate = k([no][o 2 ] c. rate = k[no 2 ] 2 [NO] -2 [O 2 ] -1/2 d. rate = k[no] 2 [O 2 ] 2 e. rate = k([no][o 2 ]) 2")
General Chemistry III 1046 E Exam 1 1. Cyclobutane, C 4 H 8, decomposes as shown: C 4 H 8 (g)! 2 C 2 H 4 (g). In the course of a study of this reaction, the rate of consumption of C 4 H 8 at a certain
Study Guide for Module 13 An Introduction to Equilibrium
Chemistry 1020, Module 13 Name Study Guide for Module 13 An Introduction to Equilibrium Reading Assignment: Section 12.1 and Chapter 13 of Chemistry, 6th Edition by Zumdahl. Guide for Your Lecturer: 1.
K P VERSUS K C PROPERTIES OF THE EQUILIBRIUM CONSTANT
K P VERSUS K C 1. What are the units of K p and K c for each of the following? a) 2H 2 S(g) 2H 2 (g) + S 2 (g) b) 4NH 3 (g) + 3O 2 (g) 2N 2 (g) + 6H 2 O(g) 2. What are the units of K p and K c for each
January 03, Ch 13 SB equilibrium.notebook
Ch 13: Chemical Equilibrium exists when 2 opposing reactions occur simultaneously at the same rate (dynamic rather than static) Forward rate = reverse rate https://www.youtube.com/watch?v=wld_imyqagq The
the following equilibrium constants. Label the thermodynamic and kinetic regions.
REACTION RATES 1. Distinguish between kinetic and thermodynamic regions of a reaction. 2. How does an increase in pressure affect the rate of a gas-phase reaction? What effect on the rate would doubling
6. Which expression correctly describes the equilibrium constant for the following reaction? 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g)
1. Which of the following can we predict from an equilibrium constant for a reaction? 1. The extent of a reaction 2. Whether the reaction is fast or slow 3. Whether a reaction is exothermic or endothermic
(02) WMP/Jun10/CHEM2
Energetics 2 Section A Answer all the questions in the spaces provided. 1 An equation for the equilibrium reaction between hydrogen, iodine and hydrogen iodide is shown below. H 2 (g) + I 2 (g) 2HI(g)
6. 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
Name May 2, 2012 Physical Behavior of Matter and Bonding Review
Name May 2, 2012 Physical Behavior of Matter and Bonding Review Base your answers to questions 1 through 3 on the information below. Starting as a gas at 206 C, a sample of a substance is allowed to cool
Equilibrium & Reaction Rate
Equilibrium & Reaction Rate 1. One of the important reactions in coal gasification is the catalytic methanation reaction: CO(g) + H (g) H O(g) + CH 4 (g) H 06 kj a) Predict the direction in which this
Chemistry 116: Exam 3 March 25, 2014
March 5, 014 1. Each of the following pairs contains one strong acid and one weak acid except a. HNO3 and HCO3 b. HF and HNO c. HSO4 and HS d. HCH3O and HCl e. HBr and H3PO4. Given that KB of CH3NH is
B. The rate will increase by a factor of twelve. C. The rate will increase by a factor of twenty-four. D. The rate will decrease by a factor of six.
1. If O 2 (g) disappears at a rate of 0.250 M/s at a particular moment in the reaction below, what is the rate of appearance of H 2 O(g) at the same time? C 3 H 8 (g) + 5 O 2 (g) 3 CO 2 (g) + 4 H 2 O(g)
B 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
Name: 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
8. 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
CHEMICAL EQUILIBRIUM -2
CHEMICAL EQUILIBRIUM - 1. The gaseous reaction A + B C + D + heat, has reached equilibrium. It is possible to make the reaction to proceed forward 1) by adding more of C ) by adding more of D 3) by raising
Chapter 15 Chemical Equilibrium
Equilibrium To be in equilibrium is to be in a state of balance: Chapter 15 Chemical Equilibrium - Static Equilibrium (nothing happens; e.g. a tug of war). - Dynamic Equilibrium (lots of things happen,
Practice Test F.1 (pg 1 of 7) Unit F - General Equilibrium Kp and Kc Name Per
Practice Test F. (pg of 7) Unit F - General Equilibrium Kp and Kc Name Per This is practice - Do NOT cheat yourself of finding out what you are capable of doing. Be sure you follow the testing conditions
AP Questions: Kinetics
AP Questions: Kinetics 1972 2 A + 2 B C + D The following data about the reaction above were obtained from three experiments: Rate of Formation of [A] [B] C (mole. liter -1 min -1 ) 1 0.60 0.15 6.3 10-3
Ch 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)
Q1. (a) State what is meant by the term activation energy of a reaction. (1)
Q1. (a) State what is meant by the term activation energy of a reaction. (c) State in general terms how a catalyst increases the rate of a chemical reaction. The curve below shows the Maxwell Boltzmann
Unit 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
Name period AP Unit 8: equilibrium
Name period AP Unit 8: equilibrium 1. What is equilibrium? Rate of the forward reaction equals the rate of the reverse reaction 2. How can you tell when equilibrium has been reached? The concentrations
AP Chapter 13: Kinetics Name
AP Chapter 13: Kinetics Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 13: Kinetics 2 Warm-Ups (Show your work for credit) Date 1.
AP* General Equilibrium Free Response Questions page 1
AP* General Equilibrium Free Response Questions page 1 General Equilibrium Problems 1983 Sulfuryl chloride, SO 2 Cl 2, is a highly reactive gaseous compound. When heated, it decomposes as follows: SO 2
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. A) B) 1588 C) 397 D) 28 E) 0.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The value of Keq for the equilibrium 1) H2 (g) + I2 (g) 2 HI (g) is 794 at 25 C. What
Exam 2 Sections Covered: (the remaining Ch14 sections will be on Exam 3) Useful Information Provided on Exam 2:
Chem 101B Study Questions Name: Chapters 12,13,14 Review Tuesday 2/28/2017 Due on Exam Thursday 3/2/2017 (Exam 2 Date) This is a homework assignment. Please show your work for full credit. If you do work
AQA A2 CHEMISTRY TOPIC 4.2 EQUILIBRIA BOOKLET OF PAST EXAMINATION QUESTIONS
AQA A2 CHEMISTRY TOPIC 4.2 EQUILIBRIA BOOKLET OF PAST EXAMINATION QUESTIONS 1 1. (a) The diagram below shows the effect of temperature and pressure on the equilibrium yield of the product in a gaseous
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. A) 1588 B) C) 28 D) 397 E) 0.
Chapter 15 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The value of Keq for the equilibrium 1) H2 (g) + I2 (g) 2 HI (g) is 794 at 25 C. What
Name May 2, 2012 Physical Behavior of Matter and Bonding Review
Name May 2, 2012 Physical Behavior of Matter and Bonding Review Base your answers to questions 1 through 3 on the information below. Starting as a gas at 206 C, a sample of a substance is allowed to cool
Unit 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
2. a. Define the term reaction rate. b. For the following chemical reaction O 5 2N 2. (g) 4NO 2. (g) O 2. (g) write a rate expression in terms of
I N T R O D U C T I O N T O K I N E T I C S Name Section 1. List four factors that affect the rate of a chemical reaction. For each, provide a brief statement describing how it affects the speed of a chemical
Exam 4, Ch 14 and 15 December 7, Points
Chem 130 Name Exam 4, Ch 14 and 15 December 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
Chemical Equilibrium
Chemical Equilibrium Concept of Equilibrium Equilibrium Constant Equilibrium expressions Applications of equilibrium constants Le Chatelier s Principle The Concept of Equilibrium The decomposition of N
Solubility Equilibrium, Ksp and more Name
MC Practice F.2 (Ch 15 & 17.4-6) This is practice - Do NOT cheat yourself of finding out what you are capable of doing. Be sure you follow the testing conditions outlined below. DO NOT USE A CALCULATOR.
Calculating equilibrium constants
Equilibrium Work Book Writing Equilibrium Constants Expressions 1. Write the equilibrium law (mass action expression) for each of the following reactions: a. SO 2 (g) + NO 2 (g) SO 3 (g) + NO(g) b. 2 C(s)
Section 10. Rates of Reactions Goal: Learn how temperature, concentration, and catalysts affect the rate of reaction. Summary
Chapter 10 Reaction Rates and Chemical Equilibrium Section 10. Rates of Reactions Goal: Learn how temperature, concentration, and catalysts affect the rate of reaction. Summary The rate of a reaction is
REACTION 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
Name Date Class SECTION 16.1 PROPERTIES OF SOLUTIONS
SOLUTIONS Practice Problems In your notebook, solve the following problems. SECTION 16.1 PROPERTIES OF SOLUTIONS 1. The solubility of CO 2 in water at 1.22 atm is 0.54 g/l. What is the solubility of carbon
Higher Unit 3 Part 2 Tutorial Sheet Please attempt the following questions in preparation for the session on 13 th March.
Higher Unit 3 Part 2 Tutorial Sheet Please attempt the following questions in preparation for the session on 13 th March. 1. During a redox process in acid solution, iodate ions, IO3 (aq), are converted
Chapter 9. Chemical Equilibrium
Chapter 9. Chemical Equilibrium 9.1 The Nature of Chemical Equilibrium -Approach to Equilibrium [Co(H 2 O) 6 ] 2+ + 4 Cl- [CoCl 4 ] 2- + 6 H 2 O Characteristics of the Equilibrium State example) H 2 O(l)
Chemical Equilibrium - Chapter 15
Chemical Equilibrium - Chapter 15 1. Dynamic Equilibrium a A + b B c C + d D At Equilibrium: Reaction is proceeding in both directions at the same rate. There is no net change in concentrations of reactants
CHEM 1423 Chapter 17 Homework Questions TEXTBOOK HOMEWORK
CHEM 1423 Chapter 17 Homework Questions TEXTBOOK HOMEWORK 17.29 At 425 o C, Kp = 4.18x10-9 for the reaction 2HBr(g) H 2 (g) + Br 2 (g) In one experiment, 0.20 atm of HBr(g), 0.010 atm of H 2 (g), and 0.010
Questions 1-3 relate to the following reaction: 1. The rate law for decomposition of N2O5(g) in the reaction above. B. is rate = k[n2o5] 2
![Questions 1-3 relate to the following reaction: 1. The rate law for decomposition of N2O5(g) in the reaction above. B. is rate = k[n2o5] 2](/thumbs/91/106996700.jpg "Questions 1-3 relate to the following reaction: 1. The rate law for decomposition of N2O5(g) in the reaction above. B. is rate = k[n2o5] 2")
Questions 1-3 relate to the following reaction: 2N2O5(g) 4NO2(g) + O2(g) 1. The rate law for decomposition of N2O5(g) in the reaction above A. is rate = k[n2o5] B. is rate = k[n2o5] 2 C. is rate = [NO2]
Chem 1B Dr. White 1 Chapter 13: Chemical Equilibrium Outline Chemical Equilibrium. A. Definition:
Chem 1B Dr. White 1 Chapter 13: Chemical Equilibrium Outline 13.1. Chemical Equilibrium A. Definition: B. Consider: N 2 O 4 (g, colorless) 2NO 2 (g, brown) C. 3 Main Characteristics of Equilibrium 13.2-13.4.
Thermodynamics Review 2014 Worth 10% of Exam Score
Thermodynamics Review 2014 Worth 10% of Exam Score Name: Period: 1. Base your answer to the following question on the diagram shown below. 4. The heat of combustion for is kcal. What is the heat of formation
Formulate an operational definition of reaction rate. Include: examples of chemical reactions that occur at different rates.
Kinetics 1 UNIT 2: KINETICS OUTCOMES All important vocabulary is in Italics and bold. Formulate an operational definition of reaction rate. Include: examples of chemical reactions that occur at different
A. 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
Chemistry 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
Thermodynamics Unit Test AP Chemistry Address 23 out of 25 Period:
Thermodynamics Unit Test Name: AP Chemistry Address 23 out of 25 Period: 1. Based on the above table what is the H for the reaction below? 2 CH2O2(g) + O2(g) 2 CO2(g) + 2 H2O(g) A) 128 kcal B) +128 kcal
The chemical potential energy of a substance is known as its ENTHALPY and has the symbol H.
Enthalpy Changes The chemical potential energy of a substance is known as its ENTHALPY and has the symbol H. During chemical reactions, the enthalpy can increase or decrease. The change in enthalpy during
What does the magnitude of the equilibrium constant tell us? N2(g) + O2(g) N2 O2(g) N2(g) + 3H2(g) 2NH3(g) In Short
What does the magnitude of the equilibrium constant tell us? N2(g) + O2(g) N2 O2(g) N2(g) + 3H2(g) 2NH3(g) In Short 1 D. Altering Chemical Equations and the Effect on the Equilibrium Constant What is the
10.02 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
Equilibrium. Introduction
Equilibrium Introduction From kinetics, we know that reactants sometimes collide to give products. But why can t products collide to go back to reactants? Theoretically, all chemical reactions are reversible.
AP Questions: Thermodynamics
AP Questions: Thermodynamics 1970 Consider the first ionization of sulfurous acid: H2SO3(aq) H + (aq) + HSO3 - (aq) Certain related thermodynamic data are provided below: H2SO3(aq) H + (aq) HSO3 - (aq)
CHEMICAL EQUILIBRIUM Chapter 13
1 CHEMICAL EQUILIBRIUM Chapter 13 Pb 2+ (aq) + 2 Cl (aq) PbCl 2 (s) 1 Objectives Briefly review what we know of equilibrium Define the Equilibrium Constant (K eq ) and Reaction Quotient (Q) Determining
Dynamic equilibrium: rate of evaporation = rate of condensation II. In a closed system a solid obtains a dynamic equilibrium with its dissolved state
CHEMISTRY 111 LECTURE EXAM III Material PART 1 CHEMICAL EQUILIBRIUM Chapter 14 I Dynamic Equilibrium I. In a closed system a liquid obtains a dynamic equilibrium with its vapor state Dynamic equilibrium:
Chemistry 40S Chemical Equilibrium (This unit has been adapted from
Chemistry 40S Chemical Equilibrium (This unit has been adapted from https://bblearn.merlin.mb.ca) Name: 1 2 Lesson 1: Defining Equilibrium Goals: Describe physical and chemical equilibrium. Describe the
UNIT EIGHT PROBLEM SET CHEMISTRY LEE
CHEMISTRY LEE NAME DATE BLOCK UNIT EIGHT PROBLEM SET Score: Do not cheat by copying the work of another person, or by allowing another person to copy your answers. Cheating results in a % grade for both
AP* General Equilibrium Free Response Questions page 1
AP* General Equilibrium Free Response Questions page 1 General Equilibrium Problems 1983 Sulfuryl chloride, SO 2 Cl 2, is a highly reactive gaseous compound. When heated, it decomposes as follows: SO 2
Ch. 14 In-Class Exercise
1 Chemistry 123/125 Ch. 14 In-Class Exercise Many physical and chemical processes proceed naturally in one direction, but not in the other. In other words, these processes are spontaneous in the direction
UNIT 11 Practice Test Page 1 of 13 Equilibrium
UNIT 11 Practice Test Page 1 of 13 Do NOT write on this test. $0.10/page lost or damaged fee. 1. In which of the following does the reaction go farthest to completion? A. K = 10 5 B. K = 10 5 C. K = 1000
Chapter 16. Rate Laws. The rate law describes the way in which reactant concentration affects reaction rate.
Rate Laws The rate law describes the way in which reactant concentration affects reaction rate. A rate law is the expression that shows how the rate of formation of product depends on the concentration
8. 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
Unit F FR Practice General Equilibrium (pg 1 of 26)
Unit F FR Practice General Equilibrium (pg 1 of 26) 1. Answer the following questions about glucose, C6H12O6, an important biochemical energy source. (a) Write the empirical formula of glucose. In many
AS Paper 1 and 2 Kc and Equilibria
AS Paper 1 and 2 Kc and Equilibria Q1.When one mole of ammonia is heated to a given temperature, 50 per cent of the compound dissociates and the following equilibrium is established. NH 3(g) ½ N 2 (g)
Name 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
Equilibrium Equilibrium. Reversible reactions. Equilibrium. Learning objectives. Extension. CaO + CO2. Rateforward = Ratereverse
Equilibrium 7 7.1 Equilibrium Learning objectives Reversible reactions As the name suggests, reversible reactions are reactions that can go either way. In a common reversible reaction calcium carbonate,
2. What mass of an aqueous 22.9% sodium chloride solution contains 99.5 g of water?
CHEM 1412 MIDTERM EXAM (100 pts total) ANSWER KEY Student s Name PART A (20 multiple choice questions, 3 pts each): 1. The solubility of a gas in a liquid can always be increased by: a) decreasing the
Chem 401 Unit 2 Exam Spr 2018 (Acids/ Bases/ General Equilibria /Acid-Base Equilibria)
Name: Date: Exam #: _ Chem 401 Unit 2 Exam Spr 2018 (Acids/ Bases/ General Equilibria /Acid-Base Equilibria) Multiple Choice Identify the letter of the choice that best completes the statement or answers
Name: 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
Name 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
Chp 13, 14, 15 SHOW ALL WORK AND CIRCLE FINAL ANSWERS. a) 1 only b) 2 only c) 3 only d) 1 and 2 only e) 1, 2, and H 2
Chp 13, 14, 15 Name: SHOW ALL WORK AND CIRCLE FINAL ANSWERS 1. Which of the following factors affect the initial rate of a reaction? 1) The nature of the reactants. 2) The concentration of the reactants.
Chemistry 12: Dynamic Equilibrium Practice Test
Chemistry 12: Dynamic Equilibrium Practice Test A. Multiple Choice: For each question, select the best answer and record your choice on the answer key provided. /25 1) A system at equilibrium is said to
Kinetics & 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
Answer questions 1a 1d. Color leaf one the color that corresponds to the answer that is used twice.
Station 1 Answer questions 1a 1d. Color leaf one the color that corresponds to the answer that is used twice. Outline the leaf in one of the other colors. Polka-dot the leaf in the third color. 1a. Which
Equilibrium Practice Problems page 1
Equilibrium Practice Problems page 1 1988 D NH 4 HS(s) NH 3 (g) + H 2 S(g) ΔHº = +93 kilojoules The equilibrium above is established by placing solid NH 4 HS in an evacuated container at 25ºC. At equilibrium,
e) KC = [H + ] [HCOO - ] Kp = no expression [HCOOH]
![e) KC = [H + ] [HCOO - ] Kp = no expression [HCOOH]](/thumbs/73/68515947.jpg "e) KC = [H + ] [HCOO - ] Kp = no expression [HCOOH]")
Problems - Chapter 15 (with solutions) 1) What is the significance of the equilibrium constant? What does a large equilibrium constant tell us about a reaction? A small one? The equilibrium constant tells
1. Determine the mass of water that can be produced when 10.0g of hydrogen is combined with excess oxygen. 2 H 2 + O 2 2 H 2 O
Pre-AP Chemistry Spring 2016 Final Review Objective 6.1: Students will recognize indicators of chemical change write balanced chemical equations to describe them based on common reactivity patterns. [S.12.C.1,
Chemical Kinetics and Equilibrium
Chemical Kinetics and Equilibrium 1 Which statement incorrectly describes a chemical reaction approaching equilibrium? As a chemical reaction approaches equilibrium, the net change in the amount of reactants
Section 7.2: Equilibrium Law and the Equilibrium Constant Tutorial 1 Practice, page (a) 2 CO 2 (g) #!!"
Section 7.: Equilibrium Law and the Equilibrium Constant Tutorial Practice, page 4. (a) CO (g) #!!"! CO(g) + O (g) Products: CO(g); O (g) Reactant: CO (g) [CO [O Equilibrium law equation: [CO (b) Cl (g)
AP Chemistry Practice Problems Module 9: Kinetics and Equilibrium
AP Chemistry Practice Problems Module 9: Kinetics and Equilibrium The headings on these problems correspond to the headings on your content pages. You should work on these throughout the unit. Be sure
Enthalpy, Entropy, and Free Energy Calculations
Adapted from PLTL The energies of our system will decay, the glory of the sun will be dimmed, and the earth, tideless and inert, will no longer tolerate the race which has for a moment disturbed its solitude.
CHE 105 Fall 2016 Exam 3
CHE 105 Fall 2016 Exam 3 Your Name: Your ID: Question #: 1 Samples of CO2(g), C6H6(g), Cl2(g) and C3H8(g) are placed in separate glass vessels (only one gas to a vessel) at the same temperature and pressure.