Question

Assertion :Assertion : If reaction quotient, $Q_c$ for a particular reaction is greater than $K_c$ the reaction will proceed in the direction of reactants. Reason: Reason : Reaction quotient is defined in the same way as the equilibrium constant $K_c$ except that the concentrations in $Q_c$ are not necessarily equilibrium values.

• A. If both the assertion and reason are true and reason is the correct explanation of assertion.
• B. If both the assertion and reason are true but reason is not the correct explanation of assertion.
• C. If assertion is true but reason is false.
• D. If both assertion and reason are false.

Answer 1

The correct option is B If both the assertion and reason are true but reason is not the correct explanation of assertion.

$\left(I\right)$ For equilibrium $K_C=Q_C$ so, if $Q_C>K_C$ then $Q_C$ will decrease as the reaction progress until it becomes equal to $K_C$, As a result of this the reaction will progress in backward direction (i.e in direction of reactants).

$\left(II\right)$ Reaction quotient $Q_C$ is defined in same way as the equilibrium constant $K_C$ except the concentrations taken are not necessarily the equilibrium value.