Name Chem 6 Section #
|
|
- Brendan Richardson
- 6 years ago
- Views:
Transcription
1 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 3 (g) 2. The equilibrium constant for the reaction below is K c = 2.4 x 10 3 at 700 o C. 2 SO 3 (g) 2 SO 2 (g) + O 2 (g) a) Calculate K p for this reaction at 700 o C. A) 2.4 x 10 3 B) C) D) 15.3 b) Calculate K c for the reaction 4 SO 2 (g) + 2 O 2 (g) 4 SO 3 (g) at 700 o C. A) 2.4 x 10 3 B) 4.8 x 10 3 C) 4.2 x 10 2 D) 1.7 x 10 5 c) At this temperature, does the equilibrium favor SO 3, or does it favor SO 2 and O 2? Class 14 Page 1 Group Work
2 3. Which one of the following has the greatest tendency to proceed as written? (a) 4NH3(g) + 3O2(g) 2N2(g) + 6H2O(g) Kp = (b) N2(g) + O2(g) 2NO(g) Kp = (c) 2HF(g) F2(g) + H2(g) Kp = (d) 2NOCl(g) 2NO(g) + Cl2(g) Kp = Arrange the reactions in order of their increasing tendency to proceed toward completion. 4A. For which of the reactions below is K c = K p? (There can be more than one correct answer.) a) N 2 (g) + 3 H 2 (g) 2 NH 3 (g) b) H 2 (g) + Br 2 (g) 2 HBr(g) c) CH 4 (g) + 2 H 2 S(g) CS 2 (g) + 4 H 2 (g) d) 2 N 2 O 5 (g) 4 NO 2 (g) + O 2 (g) 4B For which reactions is K c > K P? (There can be more than one correct answer.) 4. The equilibrium constant at 100 C for the following reaction is COCl 2 (g) CO(g) + Cl 2 (g) The equilibrium mixture should be a) mostly COCl 2 (g) b) mostly CO (g) c) mostly Cl 2 (g) d) an equal mixture of CO(g) and Cl 2 (g) with almost no COCl 2 (g) 5. There is not enough information to determine anything about the equilibrium mixture. Class 14 Page 2 Group Work
3 Heterogeneous Equilibria 1. Which of the following reactions involve heterogeneous equilibria? (There is more than one correct answer.) (a) CO(g) + 2H2(g) CH3OH(g) (b) PCl3(g) + Cl2(g) PCl5(g) (c) 2H2S(g) + 3O2(g) 2H2O(g) +2SO2(g) (d) NiO(s) + CO(g) Ni(s) +CO2(g) (e) BaSO4(s) Ba 2+ (aq) + SO4 2 (aq) Write equilibrium expressions for Keq for each of the reactions. 2. The value of K c for this reaction is 1.10 at 25 C. What is the value of K p for this reaction at the same temperature? 4CuO(s) + CH 4 (g) CO 2 (g) + 4Cu(s) + 2H 2 O(g) a) 658 b) 37.2 c) 26.9 d) 4.63 e) Class 14 Page 3 Group Work
4 Equilibrium: Reaction Quotient 1. The equilibrium constant for the following reaction at 150 C is IBr(g) Br2(g)+ I2(g) If there are 0.02 moles of I2, 0.05 moles of Br2 and 0.30 moles of IBr then a) the system is at equilibrium. b) the system is not at equilibrium and the products will react to produce more IBr(g) in order to get to equilibrium. (The reaction will proceed to the left.) c) the system is not at equilibrium and the reactant (IBr) will react to produce more Br2(g) and I2(g) in order to get to equilibrium. (The reaction will proceed to the right.) d) the system can never get to equilibrium. Show all calculations and explain your reasoning. HINT Evaluate Q (the reaction quotient) for this set of concentrations. What does Q tell you about the extent and direction of a reaction? 2. Consider the following reaction at a constant temperature for which K eq = 2.7. CO(g) + H 2 O(g) CO 2 (g) + H 2 (g) If mole of CO, mole of H 2 O, mole of CO 2 and mole of H 2 are introduced into a 2 L vessel, which of the following statements will be true? a) The system is at equilibrium and no change will occur. b) The system is not at equilibrium and will proceed to the right to achieve equilibrium. c) The system is not at equilibrium and will proceed to the left to achieve equilibrium. d) The system is not at equilibrium and it cannot achieve equilibrium. e) The system is at equilibrium, but the addition of a catalyst will cause the reaction to proceed to the right. Class 14 Page 4 Group Work
5 Equilibrium Problems 1. A mixture of mol of CO 2, mol of H 2, and mol of H 2 O is placed in a 1.0 L vessel. The following equilibrium is established: CO 2 (g) + H 2 (g) CO(g) + H 2 O(g) At equilibrium, [CO 2 ] = M. Calculate the equilibrium concentrations of H 2, CO, and H 2 O. [H 2 ] [CO] [H 2 O] a) b) c) d) At temperatures near 800 o C, steam passed over hot coke (a form of carbon obtained from coal), reacts to form CO and H 2 : C(s) + H 2 O(g) CO(g) + H 2 (g) The mixture of gases that results is an important industrial fuel called water gas. When equilibrium is achieved at 800 o C, [H 2 ] = 4.0 x 10 2 M, [CO] = 4.0 x 10 2, and [H 2 O] = 1.0 x 10 2 M. Calculate K c at this temperature a) 0.16 b) c) 4.0 d) 6.25 e) There is not enough information to answer this question. Class 14 Page 5 Group Work
6 3. A mixture of g of H 2 and g of Br 2 is heated in a 2.00 L vessel at 700 K. These substances react as follows: H 2 (g) + Br 2 (g) 2 HBr(g) At equilibrium the vessel is found to contain g of H 2. a) Calculate the equilibrium concentrations of H 2, Br 2, and HBr. [H 2 ] [Br 2 ] [HBr] a) b) c) d) b) Calculate K c. a) b) 14.3 c) 15.2 d) e) Class 14 Page 6 Group Work
7 Le Chatelier s Principle 1. Considering the following equilibrium situation: 2N2O(g) + O2(g) 4NO(g) How will the amount of NO present at equilibrium be affected when other disturbances occur? (Write increase, decrease, or no change.) (a) Adding N2O(g) to the system. (b) Removing O2(g). (c) Increasing the volume of the container. (d) Adding a catalyst. 2. For the following reaction, ΔH = 2816 kj: 6 CO 2 (g) + 6 H 2 O(l) C 6 H 12 O 6 (s) + 6 O 2 (g) Which of the following statements about this equilibrium are true? A. Increasing P CO2 will cause it to shift to the left. B. Increasing temperature will cause it to shift to the left. C. Decreasing the total pressure at constant temperature will have no effect. D. Removing part of the C 6 H 12 O 6 will cause it to shift to the right. E. Adding a catalyst will cause it to shift to the left. Class 14 Page 7 Group Work
Equilibrium point of any reaction is characterized by a single number: K eq is the equilibrium constant for the reaction
Lecture 19 Equilibrium Constant Equilibrium oint of any reaction is characterized by a single number: K eq is the equilibrium constant for the reaction In general: ja + kb R + qs K eq [ R] [ S] [ A] [
More informationCHM 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
More informationJanuary 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
More informationCHEMICAL 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
More informationWrite 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
More informationChapter 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,
More informationCHEM 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
More informationGas Phase Equilibrium
Gas Phase Equilibrium Chemical Equilibrium Equilibrium Constant K eq Equilibrium constant expression Relationship between K p and K c Heterogeneous Equilibria Meaning of K eq Calculations of K c Solving
More informationCHEM 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
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 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
More information91166 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
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 informationQuiz 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
More information1.6 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.
More informationEquilibrium 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
More informationEQUILIBRIUM. Opposing reactions proceed at equal rates Concs. of reactants & products do not change over time
EQUILIBRIUM Opposing reactions proceed at equal rates Concs. of reactants & products do not change over time Examples: vapor pressure above liquid saturated solution Now: equilibrium of chemical reactions
More informationSection 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
More informationChemical 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
More informationSolubility 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.
More informationChem 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.
More informationUnit 2 Pre-Test Reaction Equilibrium
Unit 2 Pre-Test Reaction Equilibrium Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Consider the following equilibrium system: 2HF(g) F 2(g) + H 2 (g)
More informatione) 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
More informationWhat 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
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 informationChemistry 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
More informationChapter 6: Chemical Equilibrium
Chapter 6: Chemical Equilibrium 6.1 The Equilibrium Condition 6.2 The Equilibrium Constant 6.3 Equilibrium Expressions Involving Pressures 6.4 The Concept of Activity 6.5 Heterogeneous Equilibria 6.6 Applications
More informationEquilibrium Written Response
Equilibrium Written Response January 1998 2. Consider the following equilibrium: CS2 (g) + 3Cl2 (g) CCl4 (g) + S2Cl2 (g) ΔH = -238 kj a) Sketch a potential energy diagram for the reaction above and label
More informationThermodynamics 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
More informationEquilibrium Simulation
Equilibrium Simulation Imagine the two large beakers (2000 ml) are actually the same space...we have just separated them to help us keep track of reactants and products. Imagine the size of the transfer
More informationCHEMICAL 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
More information3. Indicate the mass action expression for the following reaction: 2X(g) + Y(g) 3W(g) + V(g) a) [X] 2 [Y][W] 3 [V] [W] 3 [V] [X] 2 [Y] [3W][V] [2X][Y]
1. Which of the following statements concerning equilibrium is not true? a) A system that is disturbed from an equilibrium condition responds in a manner to restore equilibrium. b) Equilibrium in molecular
More informationUnit 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
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 informationChapter 15 Equilibrium
Chapter 15. Chemical Equilibrium Sample Exercise 15.1 (p. 632) Write the equilibrium expression for K eq for these three reactions: a) 2 O 3(g) 3 O 2(g) b) 2 NO (g) + Cl 2(g) 2 NOCl (g) c) Ag + (aq) +
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 information1) 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
More informationEquilibrium. Forward and Backward Reactions. Hydrogen reacts with iodine to make hydrogen iodide: H 2 (g) + I 2 (g) 2HI(g)
Equilibrium Forward and Backward Reactions Hydrogen reacts with iodine to make hydrogen iodide: H 2 (g) + I 2 (g) 2HI(g) forward rate = k f [H 2 ][I 2 ] 2HI(g) H 2 (g) + I 2 (g) backward rate = k b [HI]
More informationChemical 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
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 information1.0 L container NO 2 = 0.12 mole. time
CHEM 1105 GAS EQUILIBRIA 1. Equilibrium Reactions - a Dynamic Equilibrium Initial amounts: = mole = 0 mole 1.0 L container = 0.12 mole moles = 0.04 mole 0 time (a) 2 In a 1.0 L container was placed 4.00
More informationC h a p t e r 13. Chemical Equilibrium
C h a p t e r 13 Chemical Equilibrium Chemical equilibrium is achieved when: the rates of the forward and reverse reactions are equal and the concentrations of the reactants and products remain constant
More informationUNIT II - REVIEW EQUILIBRIA. Part I - Multiple Choice. 1. In which of the following does the entropy decrease?
CHEMISTRY 12 UNIT II - REVIEW EQUILIBRIA Part I - Multiple Choice 1. In which of the following does the entropy decrease? A. NaCl (s) Na + (aq) + Cl (aq) B. 4 NO (g) + 6 H 2 O (g) 4 NH 3 (g) + 5 O 2 (g)
More informationEquilibrium Written Response
Equilibrium Written Response January 1998 2. Consider the following equilibrium: CS2 (g) + 3Cl2 (g) CCl4 (g) + S2Cl2 (g) H = -238 kj a) Sketch a potential energy diagram for the reaction above and label
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 informationCHEMICAL 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
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 informationChemical Equilibrium
Chemical Equilibrium What is equilibrium? Expressions for equilibrium constants, K eq ; Calculating K eq using equilibrium concentrations; Factors that affect equilibrium; Le Chatelier s Principle What
More informationa) Write the expression for the equilibrium constant, K eq
Chemistry 12 K eq Calculations Worksheet Name: Date: Block: 1. Given the equilibrium equation below: A 2(g) + B 2(g) 2AB (g) If, at equilibrium, the concentrations are as follows: [A 2] = 3.45 M, [B 2]
More information1. 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?
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)
More informationCalculations Involving the Equilibrium Constant K eq )
Calculations Involving the Equilibrium Constant K eq ) 1. Given the equilibrium equation below: A 2(g) + B 2(g) 2AB (g) If, at equilibrium, the concentrations are as follows: [A 2 ] = 3.45 M, [B 2 ] =
More informationEquilibrium Test Review
AP Chemistry Equilibrium Test Review Name..... Hour. Directions: Complete the following problems. 1. Consider the reaction system, CoO(s) + H(g) Co(s) + HO(g) The equilibrium constant expression is Note
More informationChemical Equilibrium. Professor Bice Martincigh. Equilibrium
Chemical Equilibrium by Professor Bice Martincigh Equilibrium involves reversible reactions Some reactions appear to go only in one direction are said to go to completion. indicated by All reactions are
More informationChapter 15: Chemical Equilibrium. Chem 102 Dr. Eloranta
Chapter 15: Chemical Equilibrium Chem 102 Dr. Eloranta Equilibrium State in which competing processes are balanced so that no observable change takes place as time passes. Lift Gravity Sometimes called
More informationCHEM Dr. Babb s Sections Lecture Problem Sheets
CHEM 116 - Dr. Babb s Sections Lecture Problem Sheets Kinetics: Integrated Form of Rate Law 61. Give the integrated form of a zeroth order reaction. Define the half-life and find the halflife for a general
More informationwhich has an equilibrium constant of Which of the following diagrams represents a mixture of the reaction at equilibrium?
Chapter 9 Quiz: Chemical Equilibria 1. Which of the following statements is true regarding chemical equilibrium? I. The concentrations of reactants and products at equilibrium are constant, which means
More informationMULTIPLE 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
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 informationEquilibrium HW Holt May 2017
Equilibrium HW Holt May 2017 Answer Key p. 595 (PP 1-3, SR 1-10), p. 604 (SR 1-6); p. 616 (PP 1&2); p. 618 (PP 1&2); p. 620 (PP 1&2, SR 1-7) pp. 622-624 (2-11, 14-16, 27, 29, 32, 33, 34, 37, 39, 40 (review
More informationChapter 15 Equilibrium
Chapter 15. Chemical Equilibrium 15.1 The Concept of Equilibrium Chemical equilibrium is the point at which the concentrations of all species are constant. A dynamic equilibrium exists when the rates of
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 informationMULTIPLE 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
More informationUnit 8 Topic 7: Equilibrium CDO IB Chemistry SL
Unit 8 Topic 7: Equilibrium CDO IB Chemistry SL Assessment Statements 7.1 Dynamic Equilibrium 7.1.1 Outline the characteristics of chemical and physical systems in a state of equilibrium 7.2 The position
More informationCHEM 121b Exam 3 Spring 1999
Name SSN CHEM 121b Exam 3 Spring 1999 This exam consists of 10 multiple choice questions (each worth 3 points), and 5 written problems (points noted below for each). There are a total of 100 possible points.
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 informationPrinciples of Chemistry II Vanden Bout
Chemical Equilibria Why did the color stop changing? A. the reactants were all converted to products B. the reaction came to equilibrium C. the forward and backward reaction rates are the same D. B & C
More informationK 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
More informationCh 15 Chemical Equilibrium STUDY GUIDE Accelerated Chemistry SCANTRON. Name /98
Ch 15 Chemical Equilibrium STUDY GUIDE Accelerated Chemistry SCANTRON Name /98 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments by changing
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 informationThermodynamics 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
More informationExam 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
More informationEQUILIBRIA. e Q = a D B
I. Basis of Equilibrium. A. Q and equilibrium. EQUILIBRIA 1. Consider the general reaction bb + cc dd + ee a. Αs time elapses, [B] and [C] decrease causing the rate of the forward reaction to decrease.
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 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 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 informationSection 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)
More informationEquilibrium. 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.
More informationWrite a balanced reaction.. then write the equation.. then solve for something!!
Chapter 13 - Equilibrium Study Guide Purpose: This is a guide for your as you work through the chapter. The major topics are provided so that you can write notes on each topic and work the corresponding
More information6. 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
More informationChapter 13: Chemical Equilibrium
Chapter 13: Chemical Equilibrium 13.1 The Equilibrium Condition Equilibrium: a state in which no observable changes occur H 2 O (l) H 2 O (g) Physical equilibrium: no chemical change. N 2(g) + 3H 2(g)
More informationChapter 15 Equilibrium
Chapter 15. Chemical Equilibrium Common Student Misconceptions Many students need to see how the numerical problems in this chapter are solved. Students confuse the arrows used for resonance ( )and equilibrium
More informationAP Chapter 14: Chemical Equilibrium & Ksp
AP Chapter 14: Chemical Equilibrium & Ksp Warm-Ups (Show your work for credit) Name Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 14: Chemical Equilibrium & Ksp 2 Warm-Ups
More informationChemical 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
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 informationAP* Thermodynamics Free Response Questions page 1. Essay Questions
AP* Thermodynamics Free Response Questions page 1 Essay Questions 1991 The reaction represented above is a reversible reaction. BCl 3 (g) + NH 3 (g) Cl 3 BNH 3 (s) (a) Predict the sign of the entropy change,
More informationThermochemistry HW. PSI Chemistry
Thermochemistry HW PSI Chemistry Name Energy 1) Objects can possess energy as: (a) endothermic energy (b) potential energy A) a only B) b only C) c only D) a and c E) b and c (c) kinetic energy 2) The
More informationEquilibrium. Reversible Reactions. Chemical Equilibrium
Equilibrium Reversible Reactions Chemical Equilibrium Equilibrium Constant Reaction Quotient Le Chatelier s Principle Reversible Reactions In most chemical reactions, the chemical reaction can be reversed,
More informationH = DATA THAT YOU MAY USE. Units Conventional Volume ml or cm 3 = cm 3 or 10-3 dm 3 Liter (L) = dm 3 Pressure atm = 760 torr = 1.
DATA THAT YOU MAY USE Units Conventional S.I. Volume ml or cm 3 = cm 3 or 10-3 dm 3 Liter (L) = dm 3 Pressure atm = 760 torr = 1.013 10 5 Pa torr = 133.3 Pa Temperature C 0 C = 73.15 K PV L-atm = 1.013
More informationChemical Equilibrium. Chapter
Chemical Equilibrium Chapter 14 14.1-14.5 Equilibrium Equilibrium is a state in which there are no observable changes as time goes by. Chemical equilibrium is achieved when: 1.) the rates of the forward
More informationDownloaded 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
More information1. a. The rates of the forward and reverse reactions are equal at equilibrium.
CHATER THIRTEEN CHEMICAL EQUILIBRIUM For Review 1. a. The rates of the forward and reverse reactions are equal at equilibrium. b. There is no net change in the composition (as long as temperature is constant).
More informationChemistry F18 Solutions for Practice Final
Copyright RJZ 11/27/18 1 no unauthorized use allowed Chemistry 1250 - F18 Solutions for Practice Final This material is copyrighted. Any use or reproduction is not allowed except with the expressed written
More informationEquilibrium & 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
More informationPrimary Topics in Equilibrium
Primary Topics in Equilibrium Outline 1. Equilibrium Expression 2. Calculating Concentration Given K 3. Calculating K Given Concentration Review 1. Equilibrium Expression (only gas and aqueous do not include
More informationEquilibrium and Reversible Rxns. CHAPTER 14 Chemical Equilibrium. What happens? Stoichiometry
CHAPTER 14 Chemical Equilibrium 17-1 What happens? Stoichiometry How Fast? Kinetics applies to the speed of a reaction, the concentration of product that appears (or of reactant that disappears) per unit
More informationEquilibrium. Dynamic Equilibrium, Position of Equilibrium, Liquid-Vapor Equilibrium, Equilibrium Law January 2015
Equilibrium Dynamic Equilibrium, Position of Equilibrium, Liquid-Vapor Equilibrium, Equilibrium Law January 2015 Equilibrium Review What is equilibrium? Features of equilibrium the rate of the forward
More informationa. 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
More informationThermodynamics. 1. Which of the following processes causes an entropy decrease?
Thermodynamics 1. Which of the following processes causes an entropy decrease? A. boiling water to form steam B. dissolution of solid KCl in water C. mixing of two gases in one container D. beach erosion
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 information(i.e., equilibrium is established) leads to: K = k 1
CHEMISTRY 104 Help Sheet #8 Chapter 12 Equilibrium Do the topics appropriate for your lecture http://www.chem.wisc.edu/areas/clc (Resource page) Prepared by Dr. Tony Jacob Nuggets: Equilibrium Constant
More information