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

Question

Consider the reaction equilibrium: 2SO2(g)+O2(g)2SO3(g); Δ Ho=-198 kJ On the basis of Le-Chateliers 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

Δ ng=-vc Δ Ho=-vc Takes place with decrease in number of mole or pressure, hence increase in pressure shifts equilibrium in forward side. Takes place with evolution of heat or increase in temperature, hence decrease in temperature shifts this equilibrium in forward side.

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-Chateliers 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

$Δ n_{g} = - v c$
$Δ H^{o} = - v c$
Takes place with decrease in number of mole or pressure, hence increase in pressure shifts equilibrium in forward side.
Takes place with evolution of heat or increase in temperature, hence decrease in temperature shifts this equilibrium in forward side.

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