For the reaction,
\(\mathrm{2SO_2(g)+O_2(g)\rightleftharpoons 2SO_3(g)}\), \(\Delta H=-57.2\ \mathrm{kJ\,mol^{-1}}\) and \(K_C=1.7\times10^{16}\)
Which of the following statement is incorrect ?
\(\mathrm{2SO_2(g)+O_2(g)\rightleftharpoons 2SO_3(g)}\), \(\Delta H=-57.2\ \mathrm{kJ\,mol^{-1}}\) and \(K_C=1.7\times10^{16}\)
Which of the following statement is incorrect ?
Show Hint
- The equilibrium will shift in forward direction as the pressure increase.
- The addition of inert gas at constant volume will be not affect the equilibrium constant.
- The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is required.
- The equilibrium constant decreases as the temperature increase.
The Correct Option is C
Solution and Explanation
(2) Adding an inert gas at constant volume changes no concentrations, and \(K\) depends only on temperature. Correct.
(3) A large \(K_C\) shows the extent of the reaction (thermodynamics), not its rate. The reaction can still be very slow, which is why a catalyst (\(V_2O_5\)) is used. Incorrect.
(4) The reaction is exothermic (\(\Delta H<0\)), so \(K\) decreases when temperature rises. Correct.
The incorrect statement is (3).
Answer: (3) The equilibrium constant is large suggestive of reaction going to completion and so no catalyst is required.
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