At 1565K, the equilibrium constant for the reactions: (1) 2H2O(g) <----> 2H2(g) +O2(g) and (2) 2CO2(g)...

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Question

At 1565K, the equilibrium constant for the reactions: (1) 2H2O(g) <----> 2H2(g) +O2(g) and (2) 2CO2(g)...

At 1565K, the equilibrium constant for the reactions:

(1) 2H₂O_(g) <----> 2H_2(g) +O_2(g)

and

(2) 2CO_2(g) <----> 2CO_(g) +O_2(g)

are 1.6*10^{^-11} and 1.3*10^{^-10}, respectively.

a. what is the value of the equilibrium constant for the reaction: (3) CO_2(g) + H_2(g) <----> H₂O_(g) + CO_(g)

at this temperature?

b. demonstrate how the calculations of equilibrium constants matches the calculations of dG⁰_r when adding two reactions or more ;

determine dG⁰_r for reactions (1) and (2) and use these values in order to calculate dG⁰_r and K₃ for reaction (3)

science chemistry

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Answer 1

Answer #1

If the reaction is reversed then the equilibrium constant (K) value is becomes 1/K.

If the reaction is multiply with 1/2 the the value of equilibrium constant is become square root of K .

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Answer 2

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At 1565K, the equilibrium constant for the reactions: (1) 2H2O(g) <----> 2H2(g) +O2(g) and (2) 2CO2(g)...

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At 1565K, the equilibrium constant for the reactions: (1) 2H2O(g) <----> 2H2(g) +O2(g) and (2) 2CO2(g)...

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Add Answer to: At 1565K, the equilibrium constant for the reactions: (1) 2H2O(g) <----> 2H2(g) +O2(g) and (2) 2CO2(g)...

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At 1565K, the equilibrium constant for the reactions: (1) 2H2O(g) <----> 2H2(g) +O2(g) and (2) 2CO2(g)...