Answer to Question #161097 in General Chemistry for Karrie

Question

Hydrazine, N₂H₄, reacts with oxygen to form nitrogen gas and water. If 2.05 g of N₂H₄ reacts with excess oxygen and produces 0.450 L of N₂, at 295 K and 1.00 atm, what is the percent yield of the reaction?

Answer 1

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

actual yield by PV = nRT

1×0.450L = n×0.0821×295

n = 0.01858 moles

theoretical yield by

2.05 g N₂H₄ × $\frac{1moleN_2H_4}{32gN_2H_4}$ ×$\frac{1moleN_2}{1moleN_2H_4}$

= 0.064 moles

% yield = (0.01858/0.064) × 100

% yield = 0.2903×100

%yield = 29.03%