For the reaction, 2SO2(g) + O2(g) leftharpoons 2SO3(g), Δ H = -57.2 kJ mol-1 and Kc = 1.7 × 1016. Which of the following statement is INCORRECT?

Question

For the reaction, 2SO2(g) + O2(g) leftharpoons 2SO3(g), Δ H = -57.2 kJ mol-1 and Kc = 1.7 × 1016. Which of the following statement is INCORRECT? (A) The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is required (B) The equilibrium will shift in forward direction as the pressure increase (C) The equilibrium constant decreases as the temperature increases (D) The addition of inert gas at constant volume will not affect the equilibrium constant

Tardigrade Admin · Accepted Answer

In option (2)- Δ ng is -ve therfore increase in pressure will bring reaction in forward direction. In option (3)- as the reaction is exothermic therefore increase in temperature will decrease the equilibrium constant. In option (4)- Equillibrium constant changes only with temperature. Hence, option (2), (3) and (4) are correct therefore option (1) is incorrect choice.

Q. For the reaction, 2SO2​(g)+O2​(g)⇌2SO3(g), ΔH=−57.2kJmol−1 and Kc​=1.7×1016. Which of the following statement is INCORRECT?

The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is required

The equilibrium will shift in forward direction as the pressure increase

The equilibrium constant decreases as the temperature increases

The addition of inert gas at constant volume will not affect the equilibrium constant

Q. For the reaction,
$2 S O_{2} (g) + O_{2} (g) ⇌ 2 SO 3 (g),$
$Δ H = - 57.2 k J m o l^{- 1}$ and $K_{c} = 1.7 \times 1 0^{16}$ .
Which of the following statement is INCORRECT?