25- 2 H2S(g) → 2 H2(g) + S2(g) When heated, hydrogen sulfide gas decomposes according to the equation above. A 3.40 g sample of H2S(g) is introduced into an evacuated rigid 1.25 L container. The sealed container is heated to 483 K, and 3.72x10-2 mol of S2(g) is present at equilibrium. (a) Write the expression for the equilibrium constant, Ke, for the decomposition reaction represented above. (b) Calculate the equilibrium concentration, in mol·L-l, of the following gases in the container at 483 K. (i) H2(g) (ii) H2S(g) (c) Calculate the value of the equilibrium constant, Ke, for the decomposition reaction at 483 K.

25- 2 H2S(g) → 2 H2(g) + S2(g) When heated, hydrogen sulfide gas decomposes according to the equation above. A 3.40 g sample of H2S(g) is introduced into an evacuated rigid 1.25 L container. The sealed container is heated to 483 K, and 3.72x10-2 mol of S2(g) is present at equilibrium. (a) Write the expression for the equilibrium constant, Ke, for the decomposition reaction represented above. (b) Calculate the equilibrium concentration, in mol·L-l, of the following gases in the container at 483 K. (i) H2(g) (ii) H2S(g) (c) Calculate the value of the equilibrium constant, Ke, for the decomposition reaction at 483 K.

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...

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