Question

Assertion :Equilibrium constant for the reverse reaction is the inverse of the equilibrium constant for the reaction in the forward direction. Reason: Equilibrium constant depends upon the way in which the reaction is written.

• A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
• B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
• C. Assertion is correct but Reason is incorrect
• D. Assertion is incorrect but Reason is correct

Answer 1

The correct option is A Both Assertion and Reason are correct and Reason is the correct explanation for Assertion

Factors affecting equilibrium constant :

Mode of representation of the reaction :

$A+B\to C+D$

The equilibrium constant for the reaction

$K_C=\frac{\left[C\right]\left[D\right]}{\left[A\right]\left[B\right]}$

If the reaction is reversed

$C+D\to A+B$

then,

$K_C^{{}^{\prime }}=\frac{\left[A\right]\left[B\right]}{\left[C\right]\left[D\right]}$

The two equilibrium constant related as $\to K_C=\frac{1}{K_C^{{}^{\prime }}}$