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Problem 94

Calculate $\Delta G^{\circ}$ at 298 $\mathrm{K}$ for these reactions and predict the effect
on $\Delta G^{\circ}$ of lowering the temperature.
$$\begin{array}{l}{\text { a. } \mathrm{NH}_{3}(g)+\mathrm{HBr}(g) \longrightarrow \mathrm{NH}_{4} \mathrm{Br}(s)} \\ {\text { b. } \mathrm{CaCO}_{3}(s) \longrightarrow \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)} \\ {\text { c. } \mathrm{CH}_{4}(g)+3 \mathrm{Cl}_{2}(g) \longrightarrow \mathrm{CHCl}_{3}(g)+3 \mathrm{HCl}(g)} \\ {\quad\left(\Delta G_{\mathrm{f}}^{\circ} \text { for } \mathrm{CHCl}_{3}(g) \text { is }-70.4 \mathrm{kJ} / \mathrm{mol.}\right)}\end{array}$$

PART $\mathrm{A} : \Delta G^{\circ}=-105.4 \mathrm{kJ}$ and more negative
PART $\mathrm{B} : \Delta G^{\circ}=131.4 \mathrm{kJ} \mathrm{and}$ less positive
PART $\mathrm{C} : \Delta G^{\circ}=-305.8 \mathrm{kJ}$ and no significant change

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