For the reaction ,$2SO_{2}\left ( g \right )+O_{2}\left ( g \right )\rightleftharpoons 2SO_{3}\left ( g \right ),$$\Delta H=-57.2\; kJ\; mol^{-1}\; and$$K_{c}=1.7\times 10^{16}.$Which of the following statement is INCORRECT ?Option 1)The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is required .Option 2)The equilibrium will shift in forward direction as the pressure increases.Option 3)The equilibrium constant decreases as the temperature increases.Option 4)The addition of inert gas at constant volume will not affect the equilibrium constant.

Option 2 $\rightarrow$ $\Delta n_{g}=-ve$ so, increase in pressure will bring reaction in forward direction , it is correct.

Option 3$\rightarrow$ $\Delta H=-57.2$ means reaction is exothermic so, equlibrium constant decreases as the temperature increases.

Option 4$\rightarrow$ Equilibrium constant depend or change only with temperature .

Option2,3,4 is correct so, Option (1) is incorrect.

Option 1)

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

Option 2)

The equilibrium will shift in forward direction as the pressure increases.

Option 3)

The equilibrium constant decreases as the temperature increases.

Option 4)

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

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