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Q.
In the given reaction : $A + 2B \rightleftharpoons 2C$ moles each of $A$ and $B$ present in $10\, L$ of solution combine to form $1$ mole of $C$. Calculate $K_c$ for the reaction.
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 $C = 1/10$
$K_{c}=\frac{\left[C\right]^{2}}{\left[A\right]\left[B\right]^{2}}=\frac{\left[1/10\right]^{2}}{\left[1.5 / 10\right]\left[1 / 10\right]^{2}}=6.67$
