1 N204(l) + 2 N2H4(l) --> 3 N2(g) + 4 H2O(g)

Question

If you start with: 5.0 x 10^4 g hydrazine (N2H4) "in the tank":

1) How many moles of nitrogen can be created (assuming 100% yield)?
2) How many moles of water can be produced?
2) What mass of dinitrogen tetroxide (N2O4) is needed? What volume of N2O4 is needed? (density = 1.44 g/cm^3)

Answer 1

Each of your 1,2,3 questions are separate stoichiometry problems. Here is an example of a stoichiometry problem. Just follow the steps.
http://www.jiskha.com/science/chemistry/stoichiometry.html
Post your work if you get stuck.