# Chemistry

posted by
**BOB**
.

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?