Hydrazine, N2H4, once used as a rocket propellant, reacts with ...

[clippers!]

Question 1

If the percent yield for the following reaction is 75.0%, and 35.0 g of NO2 are consumed in the reaction, how many grams of nitric acid, HNO3(aq) are produced?

3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)

◦ 24.0 g
◦ 42.6 g
◦ 31.9 g
◦ 53.9 g

Question 2

Hydrazine, N2H4, once used as a rocket propellant, reacts with oxygen in the following equation.

N2H4(g) + O2(g) → N2(g) + 2 H2O(g)

The reaction, at 50% yield, produces 4.0 moles of N2.  What was the mass of hydrazine used?  Assume that O2 is in excess.
◦ 32.0 g
◦ 64 g
◦ 0.063 g
◦ 260 g

[stallen]

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[clippers!]

Thanks for the timely response, appreciate it

[mcarey591]

Wow, this really help