Question

A closed system contains the following reaction at STP: $C{l}_2$(g) + $2N{O}_2$(g) $\rightleftharpoons 2N{O}_{2}Cl$(g). What is the equilibrium constant expression for this reaction?

• A. $K_{eq}=\frac{[N{O}_{2}Cl{]}^2}{\left[C{l}_2\right]\left[N{O}_2\right]}$
• B. $K_{eq}=\frac{\left[C{l}_2\right][N{O}_2{]}^2}{\left[N{O}_{2}Cl\right]}$
• C. $K_{eq}=\frac{\left[C{l}_2\right][N{O}_2{]}^2}{[N{O}_{2}Cl{]}^2}$
• D. $K_{eq}=\frac{[N{O}_{2}Cl{]}^2}{\left[C{l}_2\right][N{O}_2{]}^2}$
• E. $K_{eq}=\frac{[N{O}_{2}Cl{]}^2}{\left[C{l}_2{]}^2\right[N{O}_2{]}^2}$

Answer 1

The correct option is D $K_{eq}=\frac{[N{O}_{2}Cl{]}^2}{\left[C{l}_2\right][N{O}_2{]}^2}$

The equilibrium constant expression is $K_{eq}=\frac{[N{O}_{2}Cl{]}^2}{\left[C{l}_2\right][N{O}_2{]}^2}$
The equilibrium constant is the ratio of the product of equilibrium concentrations (mol/L) of products to the product of equilibrium concentrations of reactants, with the concentration of each substance raised to the power equal its stoichiometric coefficient in the balanced chemical equation.