Consider the following statement about the equilibrium, 2 SO 2(g)+ O 2(g) leftharpoons 2 SO 3(g) ; Δ H°=-198 kJ I. On decreasing the temperature as well as pressure equilibrium shifts in forward direction. II. On increasing temperature and pressure equilibrium shifts in forward direction. III. On decreasing the temperature and increasing the pressure, equilibrium will shift in forward direction. Choose the correct statement.

Question

Consider the following statement about the equilibrium, 2 SO 2(g)+ O 2(g) leftharpoons 2 SO 3(g) ; Δ H°=-198 kJ I. On decreasing the temperature as well as pressure equilibrium shifts in forward direction. II. On increasing temperature and pressure equilibrium shifts in forward direction. III. On decreasing the temperature and increasing the pressure, equilibrium will shift in forward direction. Choose the correct statement. (A) I and II (B) Only II (C) Only III (D) I, II and III

Tardigrade Admin · Accepted Answer

For the given reaction, 2 SO 2(g)+ O 2(g) leftharpoons 2 SO 3(g) text ; the value of Δ n and Δ H=- ve. Therefore, according to the Le-Chatelier's principle, the increase in pressure and decrease in temperature, shifts the equilibrium in forward direction. Thus, option (c) is correct.

I and II

Only II

Only III

I, II and III

For the given reaction, 2SO2​(g)+O2​(g)⇌2SO3​(g); the value of Δn and ΔH=− ve. Therefore, according to the Le-Chatelier's principle, the increase in pressure and decrease in temperature, shifts the equilibrium in forward direction. Thus, option (c) is correct.

For the given reaction,
$2 S O_{2} (g) + O_{2} (g) ⇌ 2 S O_{3} (g);$
the value of $Δ n$ and $Δ H = -$ ve. Therefore, according to the Le-Chatelier's principle, the increase in pressure and decrease in temperature, shifts the equilibrium in forward direction.
Thus, option (c) is correct.