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**Problem**: 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 4.76 kJ•mol-1 at 2000. K and - 65.63 kJ•mol-1 at 3000. K. Determine the value of K (the thermodynamic equilibrium constant) at each temperature.K at 2000. K = _____K at 3000. K = _____Assuming that delta H°rxn, is independent of temperature, determine the value of Δ H°rxn from these data.ΔH°rxn = ______ kJ mol-1

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The following equation represents the decomposition of a generic diatomic element in its standard state.

1/2 X_{2}(g) → X(g)

Assume that the standard molar Gibbs energy of formation of X(g) is 4.76 kJ•mol^{-1} at 2000. K and - 65.63 kJ•mol^{-1} at 3000. K. Determine the value of K (the thermodynamic equilibrium constant) at each temperature.

K at 2000. K = _____

K at 3000. K = _____

Assuming that delta H°_{rxn}, is independent of temperature, determine the value of Δ H°_{rxn} from these data.

ΔH°_{rxn} = ______ kJ mol^{-1}

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