1. Which of the following is correct about the condition in equilibrium? A. The amount of the reactants and products will vary. B. Chemical reaction completely stops upon reaching equilibrium. C. Disruptions will be completely ignored when the chemical reaction is already in equilibrium. D. A chemical reaction in equilibrium is not static - rather, it is dynamic. 2. Which condition favors the reverse direction of a reversible reaction? A. Q > K B. Q = 0 C. Q = K D. Q < K 3. The reaction [2 NO: = N:O4 ], in general terms, is: A. Reversible B. Irreversible

1. Which of the following is correct about the condition in equilibrium? A. The amount of the reactants and products will vary. B. Chemical reaction completely stops upon reaching equilibrium. C. Disruptions will be completely ignored when the chemical reaction is already in equilibrium. D. A chemical reaction in equilibrium is not static - rather, it is dynamic. 2. Which condition favors the reverse direction of a reversible reaction? A. Q > K B. Q = 0 C. Q = K D. Q < K 3. The reaction [2 NO: = N:O4 ], in general terms, is: A. Reversible B. Irreversible

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 39A

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Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.
12.100 A reaction important in smog formation is O3(g)+NO(g)O2(g)+NO2(g)K=6.01034 (a) If the initial concentrations are [O3]=1.0106M,[NO]=1.0105M,[NO2]=2.5104M, and [O2]=8.2103M , is the system at equilibrium? If not, in which direction does the reaction proceed? (b) If the temperature is increased, as on a very warm day, will the concentrations of the products increase or decrease? (HINT: You may have to calculate the enthalpy change for the reaction to find out if it is exothermic or endothermic.)
In each of the reactions, how does the equilibrium respond to an increase in pressure? (a) 2SO 2 ( g )+ O 2 ( g ) 2SO 3 ( g ) (b) H 2 ( g )+ I 2 ( g )2HI( g ) (c) 3H 2 ( g )+ N 2 2NH 3 ( g )
5.22. True or false: If for a gas-phase reaction, then all equilibrium partial pressures of reactants and products must equal . Explain your choice.
1. A process is spontaneous in the direction that moves it away from equilibrium toward equilibrium
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
The following data are for the system A(g)2B(g) (a) How long does it take the system to reach equilibrium? (b) How does the rate of the forward reaction compare with the rate of the reverse reaction after 30 s? After 90 s?
In Section 13.1 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term closed system. and why is it necessary to have a closed system in order for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
. The reaction C2H2(g)+2Br2(g)C2H2Br4(g)is exothermic in the forward direction. Will an increase in temperature shift the position of the equilibrium toward reactants or products?
In Section 17.3 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term “closed system,” and why is it necessary for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
. Write the equilibrium expression for each of the following heterogeneous equilibria. a. 4Al(s)+3O2(g)2Al2O3(s)b. NH3(g)+HCl(g)NH4Cl(s)C. 2Mg(s)+O2(g)2MgO(s)