# Calculating Equilibrium Partial Pressures of Gases in a Reaction Mixture

## What are the equilibrium partial pressures of CH4, H2S, CS2, and H2 in the given reaction mixture?

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

## Equilibrium Partial Pressures Calculation:

To calculate the equilibrium partial pressures of CH4, H2S, CS2, and H2 in the given reaction mixture, we can use the mole ratios from the balanced equation and the ideal gas law. The equilibrium partial pressures are Peq(CH4) = 0.528 atm, Peq(H2S) = 0.111 atm, Peq(CS2) = 0.857 atm, and Peq(H2) = 1.205 atm.

**Explanation:** To calculate the equilibrium partial pressures of CH4, H2S, CS2, and H2 in the given reaction mixture, we can use the mole ratios from the balanced equation and the ideal gas law. The mole ratios are 1:2:1:4, meaning that for every 1 mole of CH4, 2 moles of H2S, 1 mole of CS2, and 4 moles of H2 are produced. The ideal gas law equation is PV = nRT, where P is the pressure in atm, V is the volume in L, n is the moles, R is the ideal gas constant (0.0821 L⋅atm/(mol⋅K)), and T is the temperature in Kelvin. We can rearrange the equation to solve for pressure: P = (n * R * T) / V. Plugging in the values into the equation, we can find the equilibrium partial pressures:

- Peq(CH4) = (0.01931 mol * 0.0821 L⋅atm/(mol⋅K) * 3330 K) / 1.0 L = 0.528 atm
- Peq(H2S) = (0.004038 mol * 0.0821 L⋅atm/(mol⋅K) * 3330 K) / 1.0 L = 0.111 atm
- Peq(CS2) = (0.02454 mol * 0.0821 L⋅atm/(mol⋅K) * 3330 K) / 1.0 L = 0.857 atm
- Peq(H2) = (0.03479 mol * 0.0821 L⋅atm/(mol⋅K) * 3330 K) / 1.0 L = 1.205 atm

Therefore, the equilibrium partial pressures of CH4, H2S, CS2, and H2 in the given reaction mixture are 0.528 atm, 0.111 atm, 0.857 atm, and 1.205 atm respectively.