Calculate the equilibrium constant for the decomposition of water 2h2o (l)  2h2 (g) + o2 (g) at 25°c, given that  g°f (h2o (l)) = - 237.2 kj/mol.

Question

Johnathon Werner

Chemistry

27 October, 23:27

Calculate the equilibrium constant for the decomposition of water 2h2o (l)  2h2 (g) + o2 (g) at 25°c, given that  g°f (h2o (l)) = - 237.2 kj/mol.

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Answers (1)

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Atlas · Answer 1

2.6 * 10^-42

Explanation:

From

∆G = - RTlnK

∆G = - 237.2 KJmol-1 or - 237.2*10^3 Jmol-1

R = 8.314 Jmol-1K-1

T = 25°C + 273 = 298K

-237.2*10^3 = 8.314 * 298 * ln K

ln K = - 237.2*10^3/2477.572

K = 2.6 * 10^-42