PLEASE BE SURE TO SHOW ALL OF YOUR WORK. Consider the reaction between hydrazine

ID: 899624 • Letter: P

Question

PLEASE BE SURE TO SHOW ALL OF YOUR WORK.

Consider the reaction between hydrazine (N2H4) and oxygen (O2):

N2H4 (l) + O2 (g) NO2 (g) + H2O (g)

a. Be sure the equation is balanced before attempting any type of stoichiometric calculation!

b. If 45.0 grams of hydrazine is reacted with 45.0 grams of O2, which is the limiting reagent?

c. How many grams of NO2 are produced from the reaction of 45.0 grams of the limiting reagent (in ‘b’)?

d. If 38.6 g of NO2 are obtained from the reaction in part ‘b’, what is the percent yield?

Balanced equation

N2H4 (l) + 3O2 (g) ---> 2NO2 (g) + 2H2O (g)

m = 45 g of N2H4

m = 45 g of O2

find limiting reactant

MW of N2H4 = 32.0452

MW of O2 = 31.988

mol = 45/32.04= 1.404

mol of O2 = 45/31.988 = 1.406

since ration is 1:3, the limiting reacatant is O2

c. How many grams of NO2 are produced from the reaction of 45.0 grams of the limiting reagent (in ‘b’)?

find NO2 production

1 mol of Hydrazine = 2 mol o fNO2

1.404 mol of hydrazine = 2*1.406 = 2.81 mol of NO2 will be produced

MW of NO2 = 46

mass = mol*MW = 2.81*46 = 129.26 grams of NO2 will be produced

d. If 38.6 g of NO2 are obtained from the reaction in part ‘b’, what is the percent yield?

m = 38.6 g of NO2 obtained...

find %yield

% yield = real/theoretical * 100% = 38.6 / 129.26 * 100 = 29.86%

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