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zanedog2018
18.07.2019 •
Chemistry
Hydrazine, n2h4 , reacts with oxygen to form nitrogen gas and water. n2h4(aq)+o2(g)⟶n2(g)+2h2o(l) if 2.65 g of n2h4 reacts with excess oxygen and produces 0.350 l of n2 , at 295 k and 1.00 atm, what is the percent yield of the reaction?
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Ответ:
The percent yield of the reaction is 17.41 %.
Explanation:
ForTo calculate the number of moles, we use the equation:
Given mass of
= 2.65 g
Molar mass of
= 32.04 g/mol
Putting values in above equation, we get:
![\text{Moles of }N_2H_4=\frac{2.65g}{32.04g/mol}=0.0827mol](/tpl/images/0105/5605/3c204.png)
ForTo calculate the number of moles, we use the equation given by ideal gas equation:
where,
P = pressure of the gas = 1 atm
V = Volume of gas = 0.350 L
n = Number of moles = ?
R = Gas constant =![0.0820\text{ L atm }mol^{-1}K^{-1}](/tpl/images/0105/5605/1e603.png)
T = temperature of the gas = 273 K
Putting values in above equation, we get:
Now, to calculate the experimental yield of
, we use the equation:
We are given:
Moles of nitrogen gas = 0.0144 moles
Molar mass of nitrogen gas = 28 g/mol
Putting values in above equation, we get:
Experimental yield of nitrogen gas = 0.4032 g
For the given chemical equation:By Stoichiometry of the reaction:
1 mole of
produces 1 mole of nitrogen gas.
So, 0.0827 moles of
will produce =
of nitrogen gas.
Now, to calculate the theoretical yield of nitrogen gas, we use equation 1:
Moles of nitrogen gas = 0.0827 mol
Molar mass nitrogen gas = 28 g/mol
Putting values in above equation, we get:
Theoretical yield of nitrogen gas = 2.3156 g
To calculate the percentage yield of nitrogen gas, we use the equation:Experimental yield of nitrogen gas = 0.4032 g
Theoretical yield of nitrogen gas = 2.3156 g
Putting values in above equation, we get:
Hence, the percent yield of the reaction is 17.41 %.
Ответ: