Question

Assertion :Assertion : The equilibrium constant for the reverse reaction is equal to the inverse of the equilibrium constant for the forward reaction. Reason: Reason : The value of equilibrium constant is independent of initial concentrations of the reactants and products.

• 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.

$\left(1\right)$ Let, the reaction is :-

$aA+bB\rightleftharpoons cC+dD$

$K_C=\frac{{\left[D\right]}^d{\left[C\right]}^c}{{\left[A\right]}^a{\left[B\right]}^b}\to \left(I\right)$

for the reverse reaction :-

$cC+dD\rightleftharpoons aA+bB$

$K_C^{{}^{\prime }}=\frac{{\left[A\right]}^a{\left[B\right]}^b}{{\left[C\right]}^c{\left[D\right]}^d}\to \left(II\right)$

$\left(I\right)$ & $\left(II\right)$ $\Rightarrow K_c^{{}^{\prime }}=1/K_c$

Equilibrium constant of a reaction depends on the temperature of the reaction as can be seen by vant Hoff's equation. It is independent of the initial concentrations of reactants and products and it is a constant value for a particular reaction at given temperature.

vart Hoff's eqn is :-

$\frac{dlnK}{dT}=\frac{△H}{{RT}^2}$