**Equilibrium Constant Calculation****Problem Statement:**What is the equilibrium constant (\(K_c\)) for the reaction below, if the reaction mixture initially contains 0.775 M CH\(_4\) and 0.789 M H\(_2\)S, and the equilibrium concentration of H\(_2\) was found to be 0.769 M?\[ \text{CH}_4(g) + 2\text{H}_2\text{S}(g) \rightleftharpoons \text{CS}_2(g) + 4\text{H}_2(g) \]**Your Answer:**[Text Box for Answer]**Explanation:**To find the equilibrium constant \(K_c\), we use the expression based on the balanced chemical equation. The expression for \(K_c\) is derived from the concentrations of the products raised to the power of their coefficients, divided by the concentrations of the reactants raised to the power of their coefficients:\[ K_c = \frac{[\text{CS}_2][\text{H}_2]^4}{[\text{CH}_4][\text{H}_2\text{S}]^2} \]**Note:** Substitute the equilibrium concentrations into the expression to compute \(K_c\).

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What is the the equilibrium constant (Kc) for the reaction below, if the reaction mixture initially contains 0.775 M CH4 and 0.789 M H₂S, and the equilibrium concentration of H₂ was found to be 0.769 M? CH4(g) + 2H2S(g) = CS2(g) +4 H2(g) Your Answer: Answer

What is the the equilibrium constant (Kc) for the reaction below, if the reaction mixture initially contains 0.775 M CH4 and 0.789 M H₂S, and the equilibrium concentration of H₂ was found to be 0.769 M? CH4(g) + 2H2S(g) = CS2(g) +4 H2(g) Your Answer: Answer

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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