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Question

Consider a reaction:
2A (g)+3B (g)3C (g)+2D (g)
When the pressure is increased :

A
Equilibrium is shifted in forward direction
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B
Equilibrium is shifted in backward direction
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C
No change in equilibrium.
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D
None of the above
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Solution

The correct option is C No change in equilibrium.
The equilibrium reaction is
2A (g)+3B (g)3C (g)+2D (g).

The total number of moles of reactants is equal to the total number of moles of products .i.e. Δng=ngproductsngreactants=(3+2)(2+3)=0
As the number of moles are equal, both in reactants and products side, therefore pressure has no effect on the equilibrium.
So the equilibrium will remain unchanged.

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