Answer:
320.04 grams of hydrazine.
Step-by-step explanation:
Please check the format when posting a question. As best I can tell, we are being asked to balance the following reaction:
N2H4 + H2O2 = N2 + H2O
[hydrazine + hydrogen peroxide = nitrogen + water]
a) Start with the most complec molecule, N2H4, and pencil in a "1" for the coefficient:
1N2H4 + H2O2 = N2 + H2O
b) Now find homes for the 2 N and 4 H atoms:
1N2H4 + H2O2 = 1N2 + 2H2O [both the 2N and 4H atoms are now accounted for in the 1N2 and 2H2O molecules]
c) The oxygen needed for the H2O must come from the H2O2 molecule. We need 2 O atoms for the products [2H2O]. Add a coefficient of 1 to the H2O2 to supply the two O atoms:
1N2H4 + 1H2O2 = 1N2 + 2H2O
The O atoms are now balanced, but the H2O2 now adds 2 more H atoms. The only possible place for them to come from is the H2O2, so lets change its coefficient to 2:
1N2H4 + 2H2O2 = 1N2 + 2H2O
d) The N atoms are accounted for. But the others:
Reactant Product
N 2 2
H 8 4
O 4 2
We're missing homes for 4 H and 2 O atoms in the products. That is the equivalent of 2 H2O molecules, so add 2 to the existing coefficient of 2:
1N2H4 + 2H2O2 = 1N2 + 4H2O
Now we have:
Reactant Product
N 2 2
H 8 8
O 4 5
The equation is balanced.
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Now we are asked how much hydrazine is needed to produce 10.0 moles of nitrogen gas.
The balanced equation tells us that we'll get 1 mole of N2 for every 1 mole of N2H4. That's a molar ratio of 1:1 (1 moles N2)/(1 mole N2H4)
That means we need 10 moles of hydrazine to produce 10 moles of N2.
Convert 10 moles hydrazine into grams:
Find the molar mass of hydrazine: 32.04 grams/mole
Multiply by 10 moles:
(10 moles hydrazine)*(32.04 grams/mole hydrazine) = 320.04 grams of hydrazine.