Question

The reaction has kp = 45.9 at 763 k. A particular equilibrium mixture at that temperature contains gaseous HI at a partial pressure of 3.00 atm and hydrogen gas at a partial pressure of 0.800 atm. What is the partial pressure of I₂?

Answer 1

To calculate the partial pressure of I2, use the equilibrium constant expression for the reaction H2(g) + I2(g) = 2HI(g) by plugging in the given values of partial pressures of HI and H2 and solve for P_I2.

Step-by-step explanation:

The student is asking about the equilibrium partial pressures of gases involved in a chemical reaction based on the given equilibrium constant (Kp) and the partial pressures of certain gases at equilibrium. To find the partial pressure of I2 given that Kp = 45.9 at 763 K and there are known partial pressures of HI and H2 at equilibrium, we use the reaction:

H2(g) + I2(g) = 2 HI(g)

At equilibrium, the expression for Kp is:

Kp = (P_HI)^2 / (P_H2 * P_I2)

By plugging in the given values and solving for P_I2 (partial pressure of I2), we calculate the unknown partial pressure. Remember to use consistent units and the correct stoichiometry in the equilibrium expression.