Question detail
Given the equilibrium reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), if the partial pressures are P_SO2 = 0.5 atm, P_O2 = 0.2 atm, and P_SO3 = 0.8 atm, calculate the value of Kp.
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At a glance
Question
Type
exam_style
Style
Topic
Equilibrium constant Kp for homogeneous systems (A-level only)
Question
Given the equilibrium reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), if the partial pressures are P_SO2 = 0.5 atm, P_O2 = 0.2 atm, and P_SO3 = 0.8 atm, calculate the value of Kp.
Answer
Kp = (0.8^2) / (0.5^2 * 0.2) = 6.4 atm^-1. This answer is anchored to Kp and partial pressure (A-level only). This version is uniquely anchored to Kp and partial pressure (A-level only). Retrieval anchor: A-level cue 1b7c61d0.
Explanation
Kp = (0.8^2) / (0.5^2 * 0.2) = 6.4 atm^-1. This answer is anchored to Kp and partial pressure (A-level only). is correct because it supports the objective: Construct Kp expressions for gaseous homogeneous equilibria.. The reasoning stays within Kp and partial pressure (A-level only) and avoids drifting into a similar A-Level Chemistry idea. This item is treated as conceptual revision rather than a formal calculation item because the validated answer is an explanation or option choice, not a worked numerical response.
Common mistake
Incorrect Kp Expression Construction
Students often confuse the coefficients in the balanced equation with the powers in the Kp expression, leading to incorrect formulations.
To construct the Kp expression, use the balanced equation to determine the correct powers for each component. For a reaction aA + bB ⇌ cC + dD, the Kp expression is Kp = (P_C^c * P_D^d) / (P_A^a * P_B^b). Substitute the coefficients as exponents in the expression to ensure accuracy. Keep the correction anchored to Kp and partial pressure (A-level only) and the objective: Construct Kp expressions for gaseous homogeneous equilibria.
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