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?

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The Answer of 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?

The Equilibrium Constant KcK_{c}Kc​ For a Chemical Reaction aA+bB⇌cCa A+b B \rightleftharpoons c CaA+bB⇌cC

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