The reaction, CO(g) + 3H₂(g)CH₄(g) + H₂O(g) is at equilibrium at 1300 K in a 1L flask. It also contain 0.30 mol of CO, 0.10 mol of H₂ and 0.02 mol of H₂O and an unknown amount of CH₄ in the flask. Determine the concentration of CH₄ in the mixture. The equilibrium constant, K_c for the reaction at the given temperature is 3.90.

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Solution

Let the concentration of methane at equilibrium be x.

It is given that K_c= 3.90.

Therefore,

Hence, the concentration of CH₄ at equilibrium is 5.85 × 10^–2 M.

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The reaction, CO(g) + 3H₂(g) CH₄(g) + H₂O(g) is at equilibrium at 1300 K in a 1L flask. It also contain 0.30 mol of CO, 0.10 mol of H₂ and 0.02 mol of H₂O and an unknown amount of CH₄ in the flask. Determine the concentration of CH₄ in the mixture. The equilibrium constant, K_cfor the reaction at the given temperature is 3.90.

The reaction, $C O (g) + 3 H_{2} (g) \leftrightarrow C H_{4} (g) + H_{2} O (g)$ is at equilibrium at 1300 K in a 1L flask. It also contain 0.30 mol of CO, 0.10 mol of $H_{2}$ and 0.02 mol of $H_{2} O$ and an unknown amount of $C H_{4}$ in the flask. Determine the concentration of $C H_{4}$ in the mixture.
The equilibrium constant, $K_{c}$ for the reaction at the given temperature is 3.90.