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The reaction quotient ' \( Q_{C}{ }^{\prime} \) is useful in predicting the direction of the reaction. Which of the
following is incorrect?
Options:
following is incorrect?
Solution:
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Verified Answer
The correct answer is:
If \( Q_{C}>K_{C} \), forward reaction is favoured
$Q_{C}>K_{C}$, reverse reaction is favored. The product concentration is more than
the equilibrium concentration. The reactant concentration is less than the equilibrium concentration.
If $Q_{C} < K_{C}$ forward reaction is favored.
If $Q_{C}=K_{C}$ the reaction is at equilibrium that is dynamic. Both forward and
reverse reactions continue to occur.
Hence, the correct options are $C$ and $D$
the equilibrium concentration. The reactant concentration is less than the equilibrium concentration.
If $Q_{C} < K_{C}$ forward reaction is favored.
If $Q_{C}=K_{C}$ the reaction is at equilibrium that is dynamic. Both forward and
reverse reactions continue to occur.
Hence, the correct options are $C$ and $D$
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