Concept:Increasing the temperature of an exothermic reaction supplies excess heat, which the system counteracts by shifting in the endothermic (reverse) direction.
Formula:$$ 2\text{SO}_2 + \text{O}_2 \rightleftharpoons 2\text{SO}_3 + \text{Heat} $$
Solution:- Because heat is a product, adding heat pushes the reaction to the left (backwards).
- As the reaction shifts left, the product \( \text{SO}_3 \) is consumed and broken down.
- Simultaneously, the reactants \( \text{SO}_2 \) and \( \text{O}_2 \) are generated.
- Thus, \( \text{SO}_2 \) and \( \text{O}_2 \) increase while \( \text{SO}_3 \) decreases.
Why other options are incorrect:Option A violates the conservation of mass (everything cannot increase simultaneously). Option C describes a forward shift. Option D is impossible because \( \text{SO}_3 \) must be consumed to form the reactants.
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