JEE Main 2003

Question

Consider the reaction equilibrium $2	ext{SO}_2(g) + 	ext{O}_2(g) ightleftharpoons 2	ext{SO}_3(g)$; $\Delta H^\circ = -198	ext{ kJ}$. On the basis of Le Chatelier's principle, the condition favourable for the forward reaction is A). increasing temperature as well as pressure B). lowering the temperature and increasing the pressure C). any value of temperature and pressure D). lowering of temperature as well as pressure

Edvaya · Accepted Answer

The correct answer is lowering the temperature and increasing the pressure. The given reaction is exothermic ($\Delta H^\circ < 0$). According to Le Chatelier's principle, lowering the temperature shifts the equilibrium in the forward direction to generate heat.
The reaction involves a decrease in the number of gaseous moles (3 moles of reactants form 2 moles of product). Therefore, increasing the pressure will shift the equilibrium forward to reduce the pressure.
Thus, lowering the temperature and increasing the pressure are favourable for the forward reaction.

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Chemistry > Physical Chemistry > Equilibrium

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