At 1400 K, K. = 2.5 x 10 for the reaction CH(g) + 2 H,S(g) CS2(g) + 4 H2(g). A 10.0 L reaction vessel at 1400 K contains 2.0 mol of CH4, 3.0 mol of CS,, 3.0 mol of H,, and 4.0 mol of H2S. Is the reaction mixture at equilib- rium? If not, in which direction does the reaction proceed to reach equilibrium? %3D
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Can you please answer question 13.64 and show all of the steps to the solution
![**Chemical Equilibrium Problems**
**13.64**
At 1400 K, \( K_c = 2.5 \times 10^{-3} \) for the reaction \( \text{CH}_4(g) + 2 \text{H}_2\text{S}(g) \rightleftharpoons \text{CS}_2(g) + 4 \text{H}_2(g) \). A 10.0 L reaction vessel at 1400 K contains 2.0 mol of \( \text{CH}_4 \), 3.0 mol of \( \text{CS}_2 \), 3.0 mol of \( \text{H}_2 \), and 4.0 mol of \( \text{H}_2\text{S} \). Is the reaction mixture at equilibrium? If not, in which direction does the reaction proceed to reach equilibrium?
**13.65**
The first step in the industrial synthesis of hydrogen is the reaction of steam and methane to give synthesis gas, a mixture of carbon monoxide and hydrogen:
\[ \text{H}_2\text{O}(g) + \text{CH}_4(g) \rightleftharpoons \text{CO}(g) + 3 \text{H}_2(g) \quad K_c = 4.7 \text{ at } 1400 \, K \]
A mixture of reactants and products at 1400 K contains 0.035 M \( \text{H}_2\text{O} \), 0.050 M \( \text{CH}_4 \), 0.15 M \( \text{CO} \), and 0.20 M \( \text{H}_2 \). In which direction does the reaction proceed to reach equilibrium?
**13.66**
Phosphine (\( \text{PH}_3 \)) decomposes at elevated temperatures, yielding gaseous \( \text{P}_2 \) and \( \text{H}_2 \):
\[ 2 \text{PH}_3(g) \rightleftharpoons \text{P}_2(g) + 3 \text{H}_2(g) \quad K_p = 398 \text{ at } 873 \, K \]
If the initial partial pressures are \( P_{\text{PH}_3} = 0](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6e830786-058e-49dd-8798-047547f22476%2F4864ffdd-5506-4932-bb5f-f0f03dfb018c%2Fsq4r7jf.jpeg&w=3840&q=75)
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