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Posted by on Friday, April 25, 2014 at 1:09am.

The following equation represents the decomposition of a generic diatomic element in its standard state.
(1/2)X2(g)--->X(g)
Assume that the standard molar Gibbs energy of formation of X(g) is 5.45 kJ·mol–1 at 2000. K and –64.30 kJ·mol–1 at 3000. K. Determine the value of K (the thermodynamic equilibrium constant) at each temperature.
at 2000K K=___
at 3000K K=___
Assuming that ΔH°rxn is independent of temperature, determine the value of ΔH°rxn from these data.
ΔH°rxn=___
I know i have to use:
∆G_rxn = - R∙T∙ln(K)
and,
K = e^{ - ∆G_r /(R∙T) } but I can't seem to get the correct answer am I missing somthing?

  • Chemistry - , Friday, April 25, 2014 at 1:16am

    That looks ok to me.

  • Chemistry - , Wednesday, March 4, 2015 at 10:39pm

    Don't forget to convert from kJ to J or vice versa.

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