For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), if the equilibrium partial pressures are P(SO2) = 0.2 atm, P(O2) = 0.1 atm, and P(SO3) = 0.4 atm, what is the value of the equilibrium constant Kp?

• A. Kp = 1.0
• B. Kp = 4.0
• C. Kp = 2.0
• D. Kp = 0.5

Answer: (B)

Verified step by step guidance

1. Identify the balanced chemical equation for the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g).
2. Write the expression for the equilibrium constant Kp for the reaction. Kp is given by the formula: $\frac{{P({\mathrm{SO}}_3}^2}{{P({\mathrm{SO}}_2}^{2}P(O_2}$.
3. Substitute the given equilibrium partial pressures into the Kp expression: $\frac{{0.4}^2}{{0.2}^{2}0.1}$.
4. Calculate the numerator of the Kp expression: ${0.4}^2$.
5. Calculate the denominator of the Kp expression: ${0.2}^{2}0.1$.