A $17\mathrm{.}3mL$ of dimethylformamide $(C_3{H}_{7}NO)$ was introduced into a $5\mathrm{.}00L$ vessel containing $C{l}_2$ and

$N_2$ gases. The temperature was held at $155C$ and the dimethylformamide totally evaporated.

Knowing that the partial pressure of $C{l}_2$ and $N_2$ are $8\mathrm{.}12$ atm and $3\mathrm{.}47$ atm, respectively, calculate

the partial pressure of the dimethylformamide and the total pressure in the container.

$($dimethylformamide: $d=0\mathrm{.}994\frac{g}{m}L)$