A mixture of 0.06906 mol of CH4, 0.01224 mol of H2S, 0.08482 mol of CS2, and 0.01029 mol of H2 is placed in a 1.0-L steel pressure vessel at 1314 K. The following equilibrium is established:1 CH4(g) + 2 H2S(g) 1 CS2(g) + 4 H2(g)At equilibrium 0.007138 mol of H2 is found in the reaction mixture.(a) Calculate the equilibrium partial pressures of CH4, H2S, CS2, and H2.Peq(CH4) = Peq(H2S) = Peq(CS2) = Peq(H2) = (b) Calculate KP for this reaction.KP =

Given that : Initial moles of CH4=0.06906 molInitial moles of H2S=0.01224 molInitial moles of…

Answered: A mixture of 0.06906 mol of CH4,…

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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Question

A mixture of 0.06906 mol of CH₄, 0.01224 mol of H₂S, 0.08482 mol of CS₂, and 0.01029 mol of H₂ is placed in a 1.0-L steel pressure vessel at 1314 K. The following equilibrium is established:

1 CH₄(g) + 2 H₂S(g) 1 CS₂(g) + 4 H₂(g)

At equilibrium 0.007138 mol of H₂ is found in the reaction mixture.

(a) Calculate the equilibrium partial pressures of CH₄, H₂S, CS₂, and H₂.

P_eq(CH₄) =

P_eq(H₂S) =

P_eq(CS₂) =

P_eq(H₂) =

(b) Calculate K_P for this reaction.

K_P =