1. Some rocket engines use a mixture of hydrazine, N2 H4, and hydrogen peroxide, H2 O2, as the propellant. The reaction is given by the following equation.
N2H4 (l) + 2H202 (l) ---> N2 (g) + 4H2O (g)
Side question: Why does the need of (l) liquid or (g) or aq(which is aqueous, dissolving in water) need to be specified. I've been doing problems with these signs since I started balancing redox reactions several chapters in general chemistry.. it hasn't seemed to affect the final answer.
a. Which is the limiting reactant in this reaction when 0.750 mol N2H4 is mixed with 0.500 mol H2O2?
b. How much of the excess reactant, in moles, remains unchanged?
c. How much of each product, in moles, is formed/
My work:
a. answer: 0.750 mol N2H4 produces 3 mol H20 ( I just looked at the ratios of H20 produced from each amount. )
b. I don't know how to find that. (????)
c. I put 0.25 mol N2, and 1 mol H20 (from plug, but I don't see why you can't plug in 0.75 mol N2H4 to find this answer)
2007-12-25
15:48:12
·
6 answers
·
asked by
Anonymous
in
Chemistry