$A + B ⇋ C + D$

The above reversible reaction is in equilibrium. What will be the effect on chemical equilibrium if the concentration of D is decreased in the system?

A backward reaction will be favoured.

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Equilibrium will shift to increase the reactant concentration.

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Equilibrium will shift to increase the product concentration.

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A forward reaction will be favoured.

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Solution

The correct options are
C
Equilibrium will shift to increase the product concentration.

D
A forward reaction will be favoured.

According to Le Chatelier's principle if there is a change in concentration, pressure or temperature of a system in equilibrium then the system will readjust itself to counteract the change and attain the equilibrium.

In the given equation, the concentration of the product is decreasing when we are decreasing the concentration of D in the system. According to Le Chatelier's principle, the system will readjust itself to increase the product concentration. Hence, a forward reaction will be favoured.

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A + B⇋C + D The above reversible reaction is in equilibrium. What will be the effect on chemical equilibrium if the concentration of D is decreased in the system?

$A + B ⇋ C + D$

The above reversible reaction is in equilibrium. What will be the effect on chemical equilibrium if the concentration of D is decreased in the system?