A fuel mixture used in the early days of rocketry is composed of two liquids, N2H4 and N2O4, which ignite on contact to form N2 gas and H2O vapor. Balanced chemical equation: 2 N2H4(l) + N2O4(l) 3 N2(g) + 4 H2O(g) Suppose 101.0 g N2H4(l) is reacted with 201.4 g N2O4(l).

(a) Calculate the moles of N2 that N2H4 would form if it were the limiting reactant. Use proper significant figures, units and show all work.

(b) Calculate the moles of N2 that N2O4 would form if it were the limiting reactant. Use proper significant figures, units and show all work.

(c) What compound (N2H4 or N2O4) is the limiting reactant? Explain. (d) What is the theoretical yield of N2 in grams. Use proper significant figures, units and show all work. (e) If the actual yield of N2 is 46.20 g, what is the percent yield of the reaction? Use proper significant figures, units and show all work.