1.) Answer the following:
2NH3(g)+ 5F2(g) =N2F4(g) +6HF(g)
Calculate
a. the stoichiometric ratio of moles NH3 to moles F2
b. the actual NH3 to F2 mole ratio when 0.235 mol NH3 is mixed with 0.368 mol F2
c. the limiting reactant (NH3 to F2) for the mixture in (b)
d. the theoretical yield, in moles, of N2F4 for the mixture in (b)

2.) Use the given equation to solve the problems
3Fe(g) + 4H2O = Fe3O4 (g) +4H2 (g)
a. How many moles of Fe would be required to react with 2.0 mol of H20?
b. How many moles of Fe3O4 can be produced from 6.0 mol of Fe?
c. How many grams of Fe3O4, can be produced from 10.00 g of Fe?
d. If you have 10.00g of Fe, how many grams of H2O will be needed for a complete reaction?
e. When 50.00g of Fe is reacted with excess H2O, 57.89 g of Fe3O4 is produced. What is the percentage yield of Fe3O4?

Thank you very much.