Concept:In an exothermic reaction, heat is released as a product. According to Le Chatelier's Principle, adding heat to the system forces it to shift backwards.
Formula:$$ \text{Reactants} \rightleftharpoons \text{Products} + \text{Heat} $$
Solution:- By increasing the temperature, you are artificially adding "Heat" to the product side of the equilibrium.
- To relieve this applied stress, the system must consume the excess heat.
- It does this by shifting the reaction to the left (the endothermic direction).
- This breaks down products and forms more reactants, thus shifting to the Reactant side.
Why other options are incorrect:Shifting to the product side would happen if temperature was decreased (removing heat). The equilibrium definitely changes, ruling out C and D.
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