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 atmChemistry

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