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Problem 108

The salt ammonium nitrate can follow three modes …


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Problem 107

Consider the reaction that occurs during the Haber process:
$$\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)$$
The equilibrium constant is $3.9 \times 10^{5}$ at 300 $\mathrm{K}$ and $1.2 \times 10^{-1}$ at 500 $\mathrm{K} .$ Calculate $\Delta H_{\mathrm{rxn}}^{\circ}$ and $\Delta S_{\mathrm{rxn}}^{\circ}$ for this reaction.


$\Delta H^{\circ}=-93 \mathrm{kJ} / \mathrm{mol}$ and $\Delta S^{\circ}=-2.0 \times 10^{2} \mathrm{J} / \mathrm{mol} \cdot \mathrm{K}$



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