Some very effective rocket fuels are composed of lightweight liquids. The fuel
composed of dimethylhydrazine \(\left[\left(\mathrm{CH}_{3}\right)_{2}
\mathrm{~N}_{2} \mathrm{H}_{2}\right]\) mixed with dinitrogen tetroxide was
used to power the Lunar Lander in its missions to the moon. The two components
react according to the following equation:
\(\left(\mathrm{CH}_{3}\right)_{2} \mathrm{~N}_{2} \mathrm{H}_{2}(l)+2
\mathrm{~N}_{2} \mathrm{O}_{4}(l) \longrightarrow 3 \mathrm{~N}_{2}(g)+4
\mathrm{H}_{2} \mathrm{O}(g)+2 \mathrm{CO}_{2}(g)\)
If \(150 \mathrm{~g}\) dimethylhydrazine reacts with excess dinitrogen tetroxide
and the product gases are collected at \(27^{\circ} \mathrm{C}\) in an evacuated
250-L tank, what is the partial pressure of nitrogen gas produced and what is
the total pressure in the tank assuming the reaction has \(100 \%\) yield?