Determine the equilibrium constant Kp at 25C for the reaction: N2 (g) + 3H2 (g)

Question

Determine the equilibrium constant Kp at 25C for the reaction: N2 (g) + 3H2 (g) <--> 2NH3 (g) Gf(NH3) = -16.6kJ/mol
A) 1.52x10^-6 B) 2.60 C) 8.28x10^-2 D) 13.4 E) 6.60x10^5
Pretty sure it's E but don't know how to get it. Determine the equilibrium constant Kp at 25C for the reaction: N2 (g) + 3H2 (g) <--> 2NH3 (g) Gf(NH3) = -16.6kJ/mol
A) 1.52x10^-6 B) 2.60 C) 8.28x10^-2 D) 13.4 E) 6.60x10^5
Pretty sure it's E but don't know how to get it. Determine the equilibrium constant Kp at 25C for the reaction: N2 (g) + 3H2 (g) <--> 2NH3 (g) Gf(NH3) = -16.6kJ/mol
A) 1.52x10^-6 B) 2.60 C) 8.28x10^-2 D) 13.4 E) 6.60x10^5
Pretty sure it's E but don't know how to get it.

Explanation / Answer

To calculate the equilibrium constant Kp at 25C for the given reaction use the following expression:

Delta G = - RT ln K= -2.303 RT log K

R= 8.314 J/(K*mol), T= 25 C = 298 K and Gf(NH3) = -16.6kJ/mol or - 16600 J / mol

Then;

Delta G - RT ln K

-16600 J /mol = -8.314 J/(K*mol) * 298 K log Kp

In Kp = (-166600 J/ mol ) / - *8.314 J/(K*mol) * 298 K

In Kp = 6.70

Kp = e^6.70 = 812.40

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