Can you explain the answer of this question below:Under the equilibrium condition for the reaction, the total pressure is 12 atm. The value of Kp is:A:16B:0.5C:2D:32The answer is a.

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If 50% of CO2 reacts: C(s) + CO2(g) --> 2CO(g) P(total) = 12 atm If half the CO2 reacted then CO2 is x/2 and CO is x, and Pt = 12. Then x/2 + x = 12 1.5x = 12 x = 8 P(CO2) = 4 atm P(CO) = 8 atm The initial pressure of CO2 is 8 atm. When half of it reacts then 4 atm is left and the pressure of CO is twice as great, which is 8 atm. Kp = P(CO)^2 / P(CO2) Kp = 8^2 / 4 Kp = 16

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Kp16

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16

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