Chapter 17.1, Problem 7PP

Solution

Interpretation:

Equilibrium concentration of a given product and reactant is to be calculated.

Concept introduction:

Equilibrium constant is the ratio of the equilibrium concentration of reactant and product in a balanced chemical equation.

$A\rightleftharpoons B+C$

$K_{eq}=\frac{[B][C]}{[A]}$

[] brackets determine the concentration of the species involve in the reaction.

The equilibrium concentration of $COC{l}_2$ is 1.829M.

Equilibrium constant is the ratio of the molar concentration of product and reactant in the balanced chemical equation.

It is expressed by $K_{eq}$.

Value of equilibrium constant tells about relative stabilities of various reactant and product

Calculating equilibrium concentration of the reaction

$COC{l}_2(g)\rightleftharpoons CO(g)+C{l}_2(g)$

$K_{eq}=\frac{[CO(g)][C{l}_2(g)]}{[COC{l}_2(g)]}$ ------------------------eq (1)

$\begin{array}{l}{K}_{eq}=8.2\times {10}^{-2}\\ [CO][C{l}_2]=0.150M\\ [COC{l}_2]=?\end{array}$

Insert the value in eq (1)

$\begin{array}{l}8.2\times {10}^{-2}=\frac{0.150M}{[CoC{l}_2]}\\ 0.082=\frac{0.150M}{[COC{l}_2]}\\ [COC{l}_2]=\frac{0.150M}{0.082}=1.829M\\ \end{array}$

So, equilibrium concentration of $[COC{l}_2]$ is 1.829M.

The equilibrium concentration of $COC{l}_2$ is 1.829M.