Question

The conventional equilibrium constant expression $\left(K_c\right)$ for the system below is:$2ICl\left(s\right)\rightleftharpoons I_2\left(s\right)+C{l}_2\left(g\right)$

• A. $\frac{\left[I_2\right]\left[C{l}_2\right]}{[ICl{]}^2}$
• B. $\frac{\left[I_2\right]\left[C{l}_2\right]}{2\left[ICl\right]}$
• C. $\left[C{l}_2\right]$
• D. $\frac{\left(\right[I_2]+[C{l}_2\left]\right)}{2\left[ICl\right]}$

Answer 1

The correct option is C $\left[C{l}_2\right]$

The equilibrium constant, Kc, is the ratio of the equilibrium concentrations of products over the equilibrium concentrations of reactants each raised to the power equal to their stoichiometric coefficients and for solids and liquids it is taken as unity. Pure solids or liquids are excluded from the equilibrium expression because their effective concentrations stay constant throughout the reaction.
So, for the given reaction,
$K_c=\left[C{l}_2\right]$