Question

What is the value of Kp at 700 K if the partial pressures in an equilibrium mixture at 700 K are 1.31 atm of CO, 10.0 atm of H₂O, 6.12 atm of CO₂, and 20.3 atm of H₂?

a. 0.0025
b. 0.0050
c. 0.0102
d. 0.0205

Answer 1

The value of Kp at 700 K, calculated using the given partial pressures for the reaction H2(g) + CO2(g) = H₂O(g) + CO(g), is 0.1054. None of the provided answer choices match this calculated value.

Step-by-step explanation:

The value of Kp at 700 K for the equilibrium of H2(g) + CO2(g) = H₂O(g) + CO(g) can be determined using the equilibrium partial pressures given: 1.31 atm of CO, 10.0 atm of H₂O, 6.12 atm of CO₂, and 20.3 atm of H₂. The expression for Kp is based on the equation Kp = (PCO x PH2O) / (PH2 x PCO2). By plugging in the given values, we get:

Kp = (1.31 atm x 10.0 atm) / (20.3 atm x 6.12 atm)

Kp = (13.1 atm²) / (124.236 atm²)

Kp = 0.1054

Thus, none of the provided options (a. 0.0025, b. 0.0050, c. 0.0102, d. 0.0205) directly matches the calculated value of Kp, which is 0.1054. It seems there might be a mistake as none of the answer choices correspond to the calculated result.