The Haber process for ammonia synthesis is exothermic:

N2(g) + 3H2(g) 2NH3(g)

Change in H (degrees) = -92KJ

If the equilibrium is constant Kc for this process at 500 Degrees Celsius is 6.0 X 10^-2, what is its value at 300 Degrees Celsius.

I am not sure which equation I should be using to solve for Kc.

My book has the example equation of:

Kc= [C]^c *[D]^d / [A]^a * [B]^b

Where product is divided by reactants, but I don't think that is the correct equation when temperature is changing also.

N2(g) + 3H2(g) 2NH3(g)

Change in H (degrees) = -92KJ

If the equilibrium is constant Kc for this process at 500 Degrees Celsius is 6.0 X 10^-2, what is its value at 300 Degrees Celsius.

I am not sure which equation I should be using to solve for Kc.

My book has the example equation of:

Kc= [C]^c *[D]^d / [A]^a * [B]^b

Where product is divided by reactants, but I don't think that is the correct equation when temperature is changing also.

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