Concept:This is an application of Le Chatelier's Principle regarding concentration changes in the Contact Process.
Formula:$$ 2\text{SO}_{2(g)} + \text{O}_{2(g)} \rightleftharpoons 2\text{SO}_{3(g)} \quad \Delta H = \text{-ive} $$
Solution:- According to Le Chatelier, adding more of a reactant creates an imbalance, forcing the system to consume the excess.
- By continuously adding more \( \text{SO}_2 \) (a reactant), the equilibrium is constantly shifted forward (to the right).
- This forward shift directly increases the production and yield of the \( \text{SO}_3 \) product.
Why other options are incorrect:Catalysts do not increase yield, only rate. Increasing temperature decreases yield (it's exothermic). Removing oxygen would shift the reaction backward, ruining yield.
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