Question

A fuel mixture used in the early days of rocketry consisted of two liquids, hydrazine (N2H4) and dinitrogen tetroxide (N2O4) which ignite on contact to form nitrogen gas and water vapor.

How many grams of nitrogen gas form when 1.00 x 10^2 g of N2H4 and 2.00 x 10^2 g of N2O4 are mixed?

So, I tried solving this but not sure what they mean by "mixed". The balanced chemical equation is:

2 N2H4 + N2O4 = 3 N2 + 4 H2O

From 1.00 x 10^2 g of N2H4, 131.09 g N2 are formed. From 2.00 x 10^2 g of N2O4, 182.65 g N2 are formed. So do I add these numbers to get the answer?

Answer 1

The correct answer is the smallest amount of N2 from the calculation of the reagents, since it corresponds to the limit reagent, which is the one consumed in its entirety. So:

m N2 = 131.09 g

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