JEE MAIN - Chemistry (2019 - 10th April Evening Slot - No. 10)
For the reaction,
2SO2(g) + O2(g) = 2SO3(g), $$\Delta $$H = –57.2 kJ mol–1 and KC = 1.7 × 1016
Which of the following statement is incorrect ?
2SO2(g) + O2(g) = 2SO3(g), $$\Delta $$H = –57.2 kJ mol–1 and KC = 1.7 × 1016
Which of the following statement is incorrect ?
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.
Explanation
Equilibrium constant has no relation with
catalyst.
Catalyst only affects the rate with which a reaction proceeds.
Here we use catalyst V2O5 to speed up the reaction.
Catalyst only affects the rate with which a reaction proceeds.
Here we use catalyst V2O5 to speed up the reaction.
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