Consider the reaction equilibrium: 2 S O 2 ( g ) + O 2 ( g ) ⇌ 2 S O 3 ( g ) ; Δ H 0 = − 198 k J On the basis of Le-Chatelier's principle, the condition favourable for the forward reaction

Question

Consider the reaction equilibrium: 2 S O 2 ​ ( g ) + O 2 ​ ( g ) ⇌ 2 S O 3 ​ ( g ) ; Δ H 0 = − 198 k J On the basis of Le-Chatelier's principle, the condition favourable for the forward reaction is -

TestHub · Accepted Answer

The reaction 2 S O 2 ​ ( g ) + O 2 ​ ( g ) ⇌ 2 S O 3 ​ ( g ) has Δ H 0 = − 198 k J , indicating it is exothermic. According to Le Chatelier's principle, lowering the temperature shifts the equilibrium towards the exothermic (forward) reaction. The forward reaction also involves a decrease in the number of gas moles (3 moles to 2 moles), so increasing pressure favors the forward reaction. Thus, lowering temperature and increasing pressure are favorable.

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