Chemistry

The key is to track how the partial pressures of all species change as the reaction reaches equilibrium, then use the equilibrium expression. Start by setting up an ICE table with mole fractions (since you know the initial ratio), convert those to partial pressures using the total pressure, and account for how many moles are consumed and produced. Once you have equilibrium partial pressures, plug them into $K_P = \frac{P_{NH_3}^2}{P_{N_2} \cdot P_{H_2}^3}$ to find your answer.

The key is to track how the partial pressures of all species change as the reaction reaches equilibrium, then use the equilibrium expression. Start by setting up an ICE table with mole fractions (since you know the initial ratio), convert those to partial pressures using the total pressure, and account for how many moles are consumed and produced. Once you have equilibrium partial pressures, plug them into $K_P = \frac{P_{NH_3}^2}{P_{N_2} \cdot P_{H_2}^3}$ to find your answer.