**Equilibrium Constant Calculation (Kc):****Reaction:** \[ \text{CH}_4(g) + 2\text{H}_2\text{S}(g) \rightleftharpoons \text{C}_\text{S}_2(g) + 4\text{H}_2(g) \]**Initial Conditions:** - Initial concentration of \(\text{CH}_4\) = 0.50 M - Initial concentration of \(\text{H}_2\text{S}\) = 0.75 M**Equilibrium Condition:** - Equilibrium concentration of \(\text{H}_2\) = 0.44 M **Task:** Calculate the equilibrium constant (\(K_c\)) for the reaction using the given information.

Answered: Image /qna-images/answer/bf0d5857-0d00-4d6b-9e58-6a3cb99ed521.jpg

[11] Consider the following reaction: CH4(g) + 2H₂S(g) = CS2(g) + 4H2(g) A reaction mixture initially contains 0.50 M CH4 and 0.75 M H₂S. If the equilibrium concentration of H₂ is 0.44 M, find the equilibrium constant (Kc) for the reaction.

[11] Consider the following reaction: CH4(g) + 2H₂S(g) = CS2(g) + 4H2(g) A reaction mixture initially contains 0.50 M CH4 and 0.75 M H₂S. If the equilibrium concentration of H₂ is 0.44 M, find the equilibrium constant (Kc) for the reaction.

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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