1/2N2 + 1/2O2 --> NO
dGfo = +86.58 kJ/mol.
dG = -RTlnKp
86,580 = -8.314*298*lnK
K = approx 10^-16
With a + sign for dG and the VERY small Kp, it is obvious that not much N2 will react with O2 to produce NO.
The standard free energy change, delta f G, for the formation of NO (g) from its elements is +86.58 kJ/mol at 25 degrees C. Calculate Kp at this temperature for the equilibrium
1/2 N2(g) + 1/2 O2(g) = NO(g)
Comment on the sign of delta G and the magnitude of Kp.
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