Equilibrium Constant KP Calculation in a Gas Reaction

What are the equilibrium partial pressures of CH4, H2S, CS2, and H2 in the given reaction mixture at 1304 K? How is the equilibrium constant KP calculated for the reaction?

Equilibrium Partial Pressures Calculation

To calculate the equilibrium partial pressures of CH4, H2S, CS2, and H2 at 1304 K, we first need to use the given number of moles and the total volume of the vessel, which is 1.0 L. Equilibrium Partial Pressures: - Peq(CH4) = 0.06053 atm - Peq(H2S) = 0.05044 atm - Peq(CS2) = 0.07902 atm - Peq(H2) = 0.01316 atm These values are determined by using the ideal gas law and the number of moles provided for each gas in the reaction mixture.

Equilibrium Constant KP Calculation

To calculate the equilibrium constant KP for the given reaction, we use the formula: KP = (Peq(CS2) * Peq(H2)^4) / (Peq(CH4) * Peq(H2S)^2) Substitute the calculated equilibrium partial pressures into the formula: KP = (0.07902 * (0.01316)^4) / (0.06053 * (0.05044)^2) ≈ 23.43 Therefore, the equilibrium constant KP for the reaction at 1304 K is approximately 23.43.

← Chemical equilibrium calculation example with reactant concentration Molarity calculation for phosphoric acid solution →

More Posts: