The Equilibrium Constant $K_{c}$ For a Chemical Reaction $a A+b B \rightleftharpoons c C$

Short Answer

The equilibrium constant $K_{c}$ for a chemical reaction $a A+b B \rightleftharpoons c C$ is given by $K_{c}=\frac{[C]^{c}}{[A]^{a}[B]^{b}}$ , where $[A]$ , $[B]$ , and $[C]$ are the equilibrium concentrations of $A, B$ , and $C$ . For the reaction $\mathrm{H}_{2}+\mathrm{I}_{2} \rightleftharpoons 2 \mathrm{HI}$ , equilibrium concentrations were calculated to be $\left[\mathrm{H}_{2}\right]=0.0057,\left[\mathrm{I}_{2}\right]=0.0059$ , and $[\mathrm{HI}]=0.013$ . What is $K_{c}$ for this reaction?