At the temperature T (K) for the reaction X_2 | vedclass

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(B) The relationship between Gibbs energy change,enthalpy change,and entropy change is given by: $\Delta G = \Delta H - T\Delta S$. We know that $\Del

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$1000x + T(2R - y) \ J \ mol^{-1}$

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(B) The relationship between Gibbs energy change,enthalpy change,and entropy change is given by: $\Delta G = \Delta H - T\Delta S$. We know that $\Delta H = \Delta U + \Delta n_g RT$. For the reaction $X_2O_{4(l)} \rightarrow 2XO_{2(g)}$,the change in the number of moles of gas is $\Delta n_g = 2 - 0 = 2$. Given $\Delta U = x \ kJ \ mol^{-1} = 1000x \ J \ mol^{-1}$ and $\Delta S = y \ J \ K^{-1} \ mol^{-1}$. Substituting these values into the enthalpy equation: $\Delta H = 1000x + 2RT$. Now,substituting $\Delta H$ into the Gibbs energy equation: $\Delta G = (1000x + 2RT) - T(y)$. Rearranging the terms,we get: $\Delta G = 1000x + T(2R - y) \ J \ mol^{-1}$.

At the temperature $T$ $(K)$ for the reaction $X_2O_{4(l)} \rightarrow 2XO_{2(g)}$,$\Delta U = x \ kJ \ mol^{-1}$ and $\Delta S = y \ J \ K^{-1} \ mol^{-1}$. The Gibbs energy change for the reaction is (Assume $XO_2$ is an ideal gas):

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