Question

For which of the following reactions would you expect the extent of the forward reaction to increase with increasing temperatures? Explain.
a) NO(g)12 N2( g)+12O2( g)ΔTH=90.2 kJ mol1\mathrm{NO}(\mathrm{g}) \rightleftharpoons \frac{1}{2} \mathrm{~N}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \quad \Delta_{\mathrm{T}} H^{\circ}=-90.2 \mathrm{~kJ} \mathrm{~mol}{ }^{-1}

Solution

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We have to explain if the increase of the temperature will increase the extent of the forward reaction for the given reaction.
In exothermic reactions, ΔrH°\Delta _rH°<0, the energy is released and it can be viewed as a product of the reaction.

In an endothermic reaction,ΔrH°\Delta _rH°>0, the energy is needed for the reaction to go forward, and it can be viewed as a reactant in the reaction.
If we increase the temperature, the equilibrium will shift in the direction of the endothermic reaction.

If we decrease the temperature, the equilibrium will shift in the direction of the exothermic reaction.

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