At the temperature T (K) for the reaction: X_ | vedclass

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

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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 $\Delta G = \Delta H - T\Delta S$. Enthalpy change is related to internal energy change by $\Delta H = \Delta U + \Delta n_gRT$. For the reaction $X_2O_{4(l)} \rightarrow 2XO_{2(g)}$,the change in the number of moles of gaseous species is $\Delta n_g = 2 - 0 = 2$. Substituting $\Delta H$ into the Gibbs equation: $\Delta G = \Delta U + \Delta n_gRT - T\Delta S$. Given $\Delta U = x \ kJ \ mol^{-1} = 1000x \ J \ mol^{-1}$ and $\Delta S = y \ J \ K^{-1} \ mol^{-1}$,we get: $\Delta G = 1000x + 2RT - Ty$. Factoring out $T$,we obtain: $\Delta G = 1000x + T(2R - y) \ J \ mol^{-1}$.

At the temperature $T$ $(K)$ for the reaction: $X_2O_{4(l)} \rightarrow 2XO_{2(g)}$,given $\Delta U = x \ kJ \ mol^{-1}$ and $\Delta S = y \ J \ K^{-1} \ mol^{-1}$. The Gibbs energy change for the reaction is: (Assume $X_2O_4$ and $XO_2$ are ideal gases)

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