Concept:Le Chatelier's Principle predicts how an equilibrium shifts in response to temperature changes, depending on whether the reaction is endothermic or exothermic.
Formula:$$ \Delta H < 0 \implies \text{Exothermic Reaction} $$
Solution:- The negative sign in \( \Delta H = -114 \text{ kJ/mol} \) indicates the forward reaction releases heat (exothermic).
- To maximize the yield of \( \text{NO}_2 \), the equilibrium must be shifted forward.
- Decreasing the temperature (removing heat) shifts an exothermic reaction forward to produce more heat.
- Therefore, it must be carried out at a logically low temperature.
Why other options are incorrect:High temperature would favor the reverse endothermic reaction, breaking down \( \text{NO}_2 \). It is fundamentally dependent on temperature.
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