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Chemistry HW, help!?
Hydrazine (N2H4) and hydrogen peroxide (H2O2) have been used as rocket propellants. They react according to the following equation:
7H2O2 + N2H4 → 2HNO3 + 8H2O
a) When 65 kg of hydrazine react, how many grams of nitric acid can be formed?
? × 10 g
b) When 180 mL of hydrogen peroxide (d = 1.41 g/mL) react, how many grams of water can be formed?
?g
c) How many grams of hydrazine will be required to react with 766 g hydrogen peroxide?
?g
d) How many grams of water can be produced when 158 g hydrazine combine with 127 g hydrogen peroxide?
?g
e) How many grams of the excess reactant in part (d) are left unreacted?
?g
1 Answer
- chumpLv 57 years ago
Ovi,
Can I make a suggestion? Post each of these questions separately. You will get much faster responses. We get points for answering each post. Nobody is going to answer all five questions for the 2 pts. when they can find 1 question for 2 pts. And be sure to give best answer pts to your responders.
So I will answer the first question: All calculations should between substances in a chemical reaction should be done with moles of those substances. Thus 65 kg of hydrazine (N2H4) is 65000 g / 32 g/mol = 2031.25 moles of N2H4. The mole ratio N2H4 : HNO3 is 1 : 2 so twice as many moles of HNO3 will be produced or 4062.5 moles of HNO3. Converted to grams by 4062.5 x 83 g/mol = 337187.5 g = 337.2 kg
