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Question

Calculate the equilibrium constant ($${K}_{p}$$) for the reaction, $$C(s)+C{ O }_{ 2 }(g)\rightleftharpoons 2CO(g)$$, at $$1300K$$ from the following data:
$$C(s)+{ H }_{ 2 }O(g)\rightleftharpoons CO(g)+{ H }_{ 2 }(g);{ K }_{ p }(1300K)=3.9\ atm$$
$${ H }_{ 2 }(g)+C{ O }_{ 2 }(g)\rightleftharpoons CO(g)+{ H }_{ 2 }O(g);{ K }_{ p }(1300K)=0.623\ atm$$


Solution

the result reaction is forming adding of reaction 1 and 2 
so the and the given temprature and condition are same so equlibrium constant are multiplt 1 and 2 
so $$Kp  =  3.9 \times 0.623 $$   atm = 2.42 atm

Chemistry

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