Question

Hydrazine, N, H, reacts with oxygen to form nitrogen gas and water. N, H(aq) + O2(g) —N,() + 2 H2O(1) If 2.35 g of N, H, reacts with excess oxygen and produces 0.850 L of N,, at 295 K and 1.00 atm, what is the percent yield of the reaction? percent yield:

Answer 1

according to balanced reaction  

32 g N2H4 gives 1 mole N2

2.35 g N2H4 gives 2.35 x 1 / 32 = 0.073 moles N2

theoretical yield of N2 = 0.073 moles

now calculate actual yield of N2 from given data

PV = nRT

n = PV / RT = 1.0 x 0.850 / 0.0821 x 295 = 0.850 / 24.21

n = 0.032

actual yield = 0.032 moles

% yield = (actual yield / theoretical yield) x 100

% yield = (0.032 / 0.073) x 100

% yield = 43.83 %