Consider the reaction equilibrium, 2SO2(g) + O2(g) leftharpoons 2SO3(g); Δ Ho = -198 kJ. On the basis of Le-Chatelier’s principle, the condition favourable for the forward reaction is

Question

Consider the reaction equilibrium, 2SO2(g) + O2(g) leftharpoons 2SO3(g); Δ Ho = -198 kJ. On the basis of Le-Chatelier’s principle, the condition favourable for the forward reaction is (A) Lowering of temperature as well as pressure (B) Increasing temperature as well as pressure (C) Lowering the temperature and increasing the pressure (D) Any value of temperature and pressure

Tardigrade Admin · Accepted Answer

It is an exothermic reaction hence low temperature and increasing pressure w ill favour forward reaction.

Q. Consider the reaction equilibrium, 2SO2(g)​+O2(g)​⇌2SO3(g)​;ΔHo=−198kJ. On the basis of Le-Chatelier’s principle, the condition favourable for the forward reaction is

Lowering of temperature as well as pressure

Increasing temperature as well as pressure

Lowering the temperature and increasing the pressure

Any value of temperature and pressure

It is an exothermic reaction hence low temperature and increasing pressure w ill favour forward reaction.

Q. Consider the reaction equilibrium,
$2 S O_{2 (g)} + O_{2 (g)} ⇌ 2 S O_{3 (g)}; Δ H^{o} = - 198 k J .$ On the basis of Le-Chatelier’s principle, the condition favourable for the forward reaction is