For a hypothetical reaction A_{2(g)} + B_{2(g | vedclass

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(A) $1$. Calculate $\Delta_r H$ at $200 \ K$ using the Gibbs-Helmholtz equation: $\Delta_r G = \Delta_r H - T \Delta_r S$. $20 	imes 10^3 \ J \ mol^{

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(A) $1$. Calculate $\Delta_r H$ at $200 \ K$ using the Gibbs-Helmholtz equation: $\Delta_r G = \Delta_r H - T \Delta_r S$. $20 	imes 10^3 \ J \ mol^{-1} = \Delta_r H - (200 \ K)(-20 \ J \ K^{-1} \ mol^{-1})$. $\Delta_r H = 20000 - 4000 = 16000 \ J \ mol^{-1} = 16 \ kJ \ mol^{-1}$. $2$. Use Kirchhoff's law to find $\Delta_r H$ at $400 \ K$: $\Delta_r H_{T_2} = \Delta_r H_{T_1} + \int_{T_1}^{T_2} \Delta_r C_p \ dT$. $\Delta_r H_{400} = 16000 + 20 	imes (400 - 200) = 16000 + 4000 = 20000 \ J \ mol^{-1} = 20 \ kJ \ mol^{-1}$.

For a hypothetical reaction $A_{2(g)} + B_{2(g)} \rightleftharpoons 2AB_{(g)}$,at $200 \ K$,$\Delta_r G$ and $\Delta_r S$ are $20 \ kJ \ mol^{-1}$ and $-20 \ J \ K^{-1} \ mol^{-1}$ respectively. If $\Delta_r C_p = 20 \ J \ K^{-1} \ mol^{-1}$,find $\Delta_r H$ at $400 \ K$ in $kJ \ mol^{-1}$.

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