At a certain temperature, 0.350 mol CH₄ and 0.676 mol H₂S are placed in a 2.50 L container.\[ \text{CH}_4(g) + 2 \text{H}_2\text{S}(g) \rightleftharpoons \text{CS}_2(g) + 4 \text{H}_2(g) \]At equilibrium, 10.4 g CS₂ is present. Calculate \( K_c \).\[ K_c = 0.0574 \]Incorrect---The image contains a chemical equilibrium problem where methane (CH₄) and hydrogen sulfide (H₂S) react to form carbon disulfide (CS₂) and hydrogen gas (H₂). Given moles of CH₄ and H₂S, and the mass of CS₂ at equilibrium, you are to calculate the equilibrium constant \( K_c \). An attempt has been made with a calculation yielding 0.0574, which is marked "Incorrect."

Answered: At a certain temperature, 0.350 mol CH,…

At a certain temperature, 0.350 mol CH, and 0.676 mol H,S are placed in a 2.50 L container. CH, (g) + 2 H,S(g) = CS,(g) + 4 H, (g) At equilibrium, 10.4 g CS, is present. Calculate K.. 0.9574

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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At a certain temperature, 0.350 mol CH₄ and 0.676 mol H₂S are placed in a 2.50 L container.

\[ \text{CH}_4(g) + 2 \text{H}_2\text{S}(g) \rightleftharpoons \text{CS}_2(g) + 4 \text{H}_2(g) \]

At equilibrium, 10.4 g CS₂ is present. Calculate \( K_c \).

\[ K_c = 0.0574 \]

Incorrect

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The image contains a chemical equilibrium problem where methane (CH₄) and hydrogen sulfide (H₂S) react to form carbon disulfide (CS₂) and hydrogen gas (H₂). Given moles of CH₄ and H₂S, and the mass of CS₂ at equilibrium, you are to calculate the equilibrium constant \( K_c \). An attempt has been made with a calculation yielding 0.0574, which is marked "Incorrect."

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