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Question

Calculate the equilibrium constant (Kp) for the reaction, C(s)+CO2(g)2CO(g), at 1300K from the following data:
C(s)+H2O(g)CO(g)+H2(g);Kp(1300K)=3.9 atm

H2(g)+CO2(g)CO(g)+H2O(g);Kp(1300K)=0.623 atm

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Solution

C(s)+H2O(g)CO(g)+H2(g);Kp(1300K)=3.9 atm (1)

H2(g)+CO2(g)CO(g)+H2O(g);Kp(1300K)=0.623 atm (2)

So, the resultant reaction is forming adding of reactions 1 and 2

The given temperature and condition are the same so the equilibrium constant are multiplying 1 and 2

so Kp = 3.9×0.623Kp = 3.9 \times 0.623 Kp = 3.9×0.623 atm = 2.42 atm

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