Chapter 8, Problem 18E

For the reaction shown, calculate how many moles of $N{H}_3$

form when each amount of reactant completely reacts.

${\text{3N}}_2{\text{H}}_4\left(l\right)\to 4{\text{NH}}_3\left(g\right)+{\text{N}}_2\left(g\right)$

a. $\text{5}{\text{.3 mol N}}_{\text{2}}{\text{H}}_{\text{4}}$

b. $\text{2}{\text{.28 mol N}}_2{\text{H}}_2$

c. $\text{5}\text{.8 }\times {\text{ 10}}^{-2}{\text{mol N}}_2{\text{H}}_4$

d. $\text{9}\text{.76 }\times {\text{ 10}}^7{\text{mol N}}_2{\text{H}}_4$