If concentration quotient, Q is greater than $K_{c}$ , the net reaction is taking place in

forward direction

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backward direction

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both directions

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cannot determine

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Solution

The correct option is B backward direction
The value of the reaction quotient Q is greater than the value of the equilibrium constant K. Hence, the concentration of products is much higher than the equilibrium concentration of products and the concentration of reactants is much smaller than the equilibrium concentration of reactants. Hence, the equilibrium will shift in the backward direction.

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The reaction quotient (Q) for the reaction.

$N_{2 (g)} + 3 H_{2 (g)} ⇌ 2 N H_{3 (g)}$ is given by

$Q = \frac{[N H_{3}]^{2}}{[N_{2}] [H_{2}]^{3}}$ . The reaction will proceed from right to left if : ( $K_{c}$ is the equilibrium constant)

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