2. (20 points) Hydrazine (N2H4) reacts with oxygen gas to form nitrogen gas and

Question

2. (20 points) Hydrazine (N2H4) reacts with oxygen gas to form nitrogen gas and water. Write a balanced chemical equation for this reaction. How many grams of nitrogen are theoretically produced when 19.5 g of hydrazine react with 18.7 g of oxygen? How many grams of the excess reactant remain? 15.6 g of nitrogen are actually produced. What is the percent yield for this reaction? Using the percent yield calculated in part (d), how many kilograms of water can actually be produced from 292 L of hydrazine in excess oxygen? (D2H4 1.02 g/mL) a. b. c. d. e.

Explanation / Answer

a)

N2H4 + O2 = N2 + H2O

balance

N2H4 + O2 = N2 + 2H2O

b)

mol of N2H4 = mass/MW = 19.5/32.05 = 0.6084

mol of O2 = mass/MW = 18.7/32 = 0.5844

raito is 1:1

0.5844 mol of O2 forms -_> 0.5844 mol of N2

mass = mol*MW = 0.5844*28= 16.36 g of N2

d

% yield= real/theoretical * 100% = 15.6/16.36*100 = 95.35 %

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