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

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 119AP

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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 )
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1. A process is spontaneous in the direction that moves it away from equilibrium toward equilibrium
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