± Percent Yield 1.84 g H2 is allowed to react with 10.2 g N2, producing 2.91 g N
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Question
± Percent Yield 1.84 g H2 is allowed to react with 10.2 g N2, producing 2.91 g NH3 The Haber-Bosch process is a very important industrial process. In the Haber-Bosch process, hydrogen gas reacts with nitrogen gas to produce ammonia according to the equation Part A What is the theoretical yield in grams for this reaction under the given conditions? Express your answer to three significant figures and include the appropriate units 2H2 (g) + N2 (g) 2NH3 (g) The ammonia produced in the Haber-Bosch process has a wide range of uses, from fertilizer to pharmaceuticals However, the production of ammonia is difficult, resulting in lower yields than those predicted from the chemical equation Hints alueUnits Submit My Answers Give Up Part B What is the percent yield for this reaction under the given conditions? Express your answer to three significant figures and include the appropriate units Hints Hint 1. The definition of percent yield (click to open)Explanation / Answer
A)
Molar mass of N2 = 28.02 g/mol
mass of N2 = 10.2 g
we have below equation to be used:
number of mol of N2,
n = mass of N2/molar mass of N2
=(10.2 g)/(28.02 g/mol)
= 0.364 mol
Molar mass of H2 = 2.016 g/mol
mass of H2 = 1.84 g
we have below equation to be used:
number of mol of H2,
n = mass of H2/molar mass of H2
=(1.84 g)/(2.016 g/mol)
= 0.9127 mol
we have the Balanced chemical equation as:
N2 + 3 H2 ---> 2 NH3
1 mol of N2 reacts with 3 mol of H2
for 0.364 mol of N2, 1.0921 mol of H2 is required
But we have 0.9127 mol of H2
so, H2 is limiting reagent
we will use H2 in further calculation
Molar mass of NH3 = 1*MM(N) + 3*MM(H)
= 1*14.01 + 3*1.008
= 17.034 g/mol
From balanced chemical reaction, we see that
when 3 mol of H2 reacts, 2 mol of NH3 is formed
mol of NH3 formed = (2/3)* moles of H2
= (2/3)*0.9127
= 0.6085 mol
we have below equation to be used:
mass of NH3 = number of mol * molar mass
= 0.6085*17.03
= 10.36 g
Answer: 10.4 g
b)
% yield = actual mass*100/theoretical mass
= 2.91*100/10.36
= 28.1 %
Answer: 28.1 %
Feel free to comment below if you have any doubts or if this answer do not work
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