Define equilibrium constant.

The equilibrium constant expression for a gas reaction is ${\mathrm{K}}_{\mathrm{c}}=\frac{{\left[{\mathrm{NH}}_3\right]}^4{\left[{\mathrm{O}}_2\right]}^5}{{\left[\mathrm{NO}\right]}^4{\left[{\mathrm{H}}_2\mathrm{O}\right]}^6}$

Write the balanced chemical equation corresponding to this expression.

Write the equations for the conversion of ${\mathrm{K}}_{\mathrm{c}} \mathrm{to} {\mathrm{K}}_{\mathrm{p}}$ for each of the following reaction.

 $\mathrm{CO}\left(\mathrm{g}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)\rightleftharpoons {\mathrm{CO}}_2\left(\mathrm{g}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)$

Write the equations for the conversion of ${\mathrm{K}}_{\mathrm{c}} \mathrm{to} {\mathrm{K}}_{\mathrm{p}}$ for each of the following reaction.

 ${\mathrm{C}}_3{\mathrm{H}}_8\left(\mathrm{g}\right)+5{\mathrm{O}}_2\left(\mathrm{g}\right)\rightleftharpoons 3{\mathrm{CO}}_2\left(\mathrm{g}\right)+4{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$