Question

In the given reaction : $A+2B\rightleftharpoons 2C$ moles each of $A$ and $B$ present in $10L$ of solution combine to form $1$ mole of $C$. Calculate $K_c$ for the reaction.

• A. 1.5
• B. 6.67
• C. 0.15
• D. 2.3

Answer 1

Answer: (B)

As $1$ mole of $C$ is formed at equilibrium,
$2x=1\Rightarrow x=0.5$
$\Rightarrow$ Equilibrium concentration of $A=1.5/10$
$B=1/10$ and $C=1/10$
$K_c=\frac{{\left[C\right]}^2}{\left[A\right]{\left[B\right]}^2}=\frac{{\left[1/10\right]}^2}{\left[1.5/10\right]{\left[1/10\right]}^2}=6.67$