Question:Calculate the value of the equilibrium constant \({K_P}\) for the reaction \(2NO(g) + C{l_2}(g) \rightleftharpoons 2NOCl(g)\) from these equilibrium pressures: NO, \(0.050atm;C{l_2},0.30atm;NOCl,1.2atm\)

Equilibrium is the state in which market supply and demand balance each other, and as a result prices become stable

We need to calculate equilibrium pressure constant for following reaction

\(2NO(g) + C{l_2}(g) \rightleftharpoons 2NOCl(g)\])

this is a reverse reaction so it should be written with a double arrow. Equilibrium constant is calculated like this:

\({K_p} = \frac{{p(NOCl)_{eq}^2}}{{p{{\left( {C{l_2}} \right)}_{eq}} \cdot p(NO)_{eq}^2}}\)

Theis pressure of the compound in the equilibrium. We are given all the data in the task:

\(\begin{array}{*{20}{c}}{p{{(NOCl)}_{eq}} = 1.2{\rm{atm}}}\\{p{{\left( {C{l_2}} \right)}_{eq}} = 0.30{\rm{atm}}}\\{p{{(NO)}_{eq}} = 0.050{\rm{atm}}}\end{array}\)

We calculate\(\begin{array}{*{20}{c}}{{K_p} = \frac{{{{1.2}^2}}}{{0.30 \cdot {{0.050}^2}}}}\\{K = 1920}\end{array}\)