Be sure to answer all parts.

Consider the formation of ammonia in two experiments.

$($a$)$ To a $1\mathrm{.}00$L container at $727\backslash$deg C$,1\mathrm{.}30$ mol of N$2$ and $1\mathrm{.}65$ mol of H$2$ are added. At equilibrium, $0\mathrm{.}100$ mol of NH$3$ is present. Calculate the equilibrium concentrations of N$2$ and H$2$ and find Kc for the reaction:

$2$ NH$3($g$)$ N$2($g$)+3$ H$2($g$)$

$[$N$2]$eq $=$ M

$[$H$2]$eq $=$ M

Kc $=$

$($b$)$ In a different $1\mathrm{.}00$L container at the same temperature, equilibrium is established with $8\mathrm{.}34\backslash$times $102$ mol of NH$3,1\mathrm{.}50$ mol of N$2,$ and $1\mathrm{.}25$ mol of H$2$ present. Calculate Kc for the reaction:

NH$3($g$)$

$1$

$2$

N$2($g$)+$

$3$

$2$

H$2($g$)$

Kc $=$