A $1\mathrm{.}000L$ container contains an equilibrium mixture of $H_{2(g)},I_{2(g)},$ and $H{I}_{(g)}$ at $721K.$ The

number of moles of each substance present is $1\mathrm{.}843{10}^{-3},1\mathrm{.}843{10}^{-3},$ and $1\mathrm{.}310{10}^{-2},$

respectively. Calculate the values of $K$ and $K_P$ for the reaction.

$H_{2(g)}+I_{2(g)}=>2H{I}_{(g)}$

$H_{2(g)}+I_{2(g)}=>2H{I}_{(g)},K=50\mathrm{.}5$

Calculate $K$ for

a$.,3H_{2(g)}+3I_{2(g)}=>6H{I}_{(g)}$

b$.,2H{I}_{(g)}=>H_{2(g)}+I_{2(g)}$