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For the reaction, 2SO2(g) +O2->2SO3(g) D...

For the reaction, `2SO_2(g) +O_2->2SO_3(g)` `DeltaH = -57.2 kJ mol^(-1) and K_(e) = 1.7 xx 10^(16)`
Which of the following statement is INCORRECT?

A

The equilibrium constant decreases as the temperature increases

B

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

C

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

D

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

Text Solution

Verified by Experts

The correct Answer is:
C
Given
`DeltaH = -57.2 kJ//mol`
`K_(c) = 1.7 xx 10^(16)`
(1) From `K darr = Ae^(-(DeltaH)/(RTuarr))` as T increases, K decreases
(2) Equilibrium constant is not a affected by change in volume.
(3) Although `K_(c)` is large but it doesn’t mean reaction go for completion.
(4) Equilibrium will shift in forward direction as pressure increases.
Hence (3) is incorrect.
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