The reaction A2 + B2 2 AB has an equilibrium constant of Kc = 4 For each of the parts below, where A is shaded and B is unshaded: i. Determine if the reaction is at equilibrium, by calculating Q. If the reaction is not at equilibrium, predict which direction the reaction ii. would proceed to reach equilibrium (i.e. towards the products or towards the reactants). ji. Explain why this would happen. iv. If we draw a graph of AG vs Reaction Progress what would that look like? a.

The reaction A2 + B2 2 AB has an equilibrium constant of Kc = 4 For each of the parts below, where A is shaded and B is unshaded: i. Determine if the reaction is at equilibrium, by calculating Q. If the reaction is not at equilibrium, predict which direction the reaction ii. would proceed to reach equilibrium (i.e. towards the products or towards the reactants). ji. Explain why this would happen. iv. If we draw a graph of AG vs Reaction Progress what would that look like? a.

Chemistry

10th Edition

ISBN:9781305957404

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

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Dinitrogen tetraoxide is a colorless gas that dissociates into nitrogen dioxide, a reddish brown gas. N₂O4(g) → 2NO₂(g) At equilibrium: 1. The forward reaction, N₂O4(g) → 2NO₂(g) A. Continues to happen. B. Stops. C. Cannot tell without additional information. 2. Change in the concentration of N₂04 A. Continues to happen. B. Stops. C. Cannot tell without additional information.
O KINETICS AND EQUILIBRIUM Calculating an equilibrium constant from a partial equilibrium... 0/5 Ammonia will decompose into nitrogen and hydrogen at high temperature. An industrial chemist studying this reaction fills a 75.0 L tank with 21. mol of ammonia gas, and when the mixture has come to equilibrium measures the amount of hydrogen gas to be 6.3 mol. Calculate the concentration equilibrium constant for the decomposition of ammonia at the final temperature of the mixture. Round your answer to 2 significant digits. K = 0 II
NH3(g) + H2O(l) → NH2 + + H3O+ t The equilibrium constant is 1 x 10 -34. Is this reaction likely to take place? Why? Choose the best answer below. a. Yes, because the equilibrium constant is very small and equilibrium will lie far to the left. b. Yes, because the equilibrium constant is very small and equilibrium will lie far to the right. c. No, because the equilibrium constant is very small and equilibrium will lie far to the right. ☐ d. No, because the equilibrium constant is very small and equilibrium will lie far to the left. Click Submit to complete this assessment.
MAI Van JL.cas-Cudo Lab Assignment #3 E.mheducation.com Saved # 3 6 Be sure to answer all parts. Consider the following equilibrium system involving SO2, Cl2, and SO,Cl, (sulfuryl dichloride): SO2(g) + Cl2(g) = SO,C(g) Predict how the equilibrium position would change if the following changes were to occur. The temperature remains constant in each case. (a) Cl, gas is added to the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. ((More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.) (b) SO,Cl, is removed from the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. (More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.) (c) SO, is removed from the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. (More…
The decomposition of PCl5 occurs by the equilibrium process PCl5(g) = PCl3(g) + Cl2(g) DH, = 92.5 kJ mol–1 If the reaction is initially at equilibrium, explain what happens when the temperature is lowered. Select one: a. The equilibrium shifts left b. The concentration of Cl2(g) will increase c. No change d. The equilibrium shifts right
I. 2NOCl (g)< < > 2NO(g) + Cl2(g) K= 1.6X 10-5 II. 2NO (g) < > N2(g) + O2(g) K= 1.0 X 1031 Which of the following will you choose to generate the most amount of NO? (Think which of the reactions will favor the formation of NO.)a.Forward reaction of IIb.Forward reaction of Ic.Reverse reaction of Id.Reverse reaction of II
The initial concentrations of four species involved in an equilibrium are: [Cl2] = 1.40 M, [HCl] = 0.100 M, [O2] = 0.300 M and [H2O] = 0.500 M. Is the reaction at equilibrium? If not, in what direction must the reaction shift for the equilibrium to be reached? Set up Kc in terms of the initial amounts and x as done in class. Do not try to solve for x. Set it up so x is positive. 4 HCl(g) + O2(g) <====> 2 Cl2(g) + 2 H2O(g) Kc = 52 At equil? ______ Direction? _______ Expression ____________
Consider the following system at equilibrium at 698 K: 2 HI (g)=H2 (g) + I2 (g) When some H2 (g) is added to the equilibrium system at constant temperature: The reaction must: A. Run in the forward direction to reestablish equilibrium. B. Run in the reverse direction to reestablish equilibrium. C. Remain the same. It is already at equilibrium. The concentration of I, will: A. Increase. B. Decrease. C. Remain the same. Submit Answer Retry Entire Group 9 more group attempts remaining
In an experiment, 1.000 mol H2 and 1.000 mol I2 are mixed in a 1.00-L container, and the reaction forms HI. If Kc = 54.3 for this reaction, what is the equilibrium concentration of HI? I2(g) + H2(g) ↔ 2HI(g) a. 1.572 b. 0.226 c. 0.399 d. 0.786 e. 0.899
Consider the following system at equilibrium at 800 K:2H2(g) + S2(g) = 2H2S(g) + 69.3 kcalIf the TEMPERATURE on the equilibrium system is suddenly increased: The reaction must: A. Run in the forward direction to reestablish equilibrium. B. Run in the reverse direction to reestablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of S2 will: A. Increase. B. Decrease. C. Remain the same.
f the value of Q is greater than K for an equilibrium reaction then a. a catalyst is necessary to achieve equilibrium. b. the reaction will proceed to the right until equilibrium is established. c. the reaction will proceed to the left until equilibrium is extablished. d. the reaction will go left or right depending on the reaction stoichiometry. e. Both (a) and (d) are correct.
Consider the equilibrium reaction: Fe3+ + SCN1 [FeSCN2+]. The initial concentration of Fe3+ = 0.00200 M. The initial concentratin of SCN¹- = 0.00200 M. The equilibrium concentration of FeSCN2+ is 0.000583 M. What is the value of the equilibrium constant, Kc? Multiple Choice О О О О 345 146 290 686