One of the components of the fuel mixture on the Apollo lunar module involved a reaction with hydrazine, N2H4, and dinitrogen tetraoxide, N2O4. If the balanced equation for this reaction is

_N2H4 (l) + _N2O4 (g) → _N2 (g) + _H2O (g),

1. what mass of N2 gas would result from the reaction of 750 kg of hydrazine and 500 kg of N2O4?

b. If there was only a 45.75% yield for the reaction how much N2 was produced?