The reaction N2 + 3 H2----> 2 NH3 is used to produce ammonia. When 450.0 g of hydrogen was reacted with nitrogen, the percent yield you achieved was 30.8%. What was the mass of ammonia produced?
Molar mass of H2 = 2.016 g/mol
mass of H2 = 450 g
mol of H2 = (mass)/(molar mass)
= 450/2.016
= 223.2143 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)*223.2143
= 148.8095 mol
Molar mass of NH3 = 1*MM(N) + 3*MM(H)
= 1*14.01 + 3*1.008
= 17.034 g/mol
mass of NH3 = number of mol * molar mass
= 148.8095*17.034
= 2534.8214 g
% yield = actual mass*100/theoretical mass
30.8= actual mass*100/2534.8214
actual mass= 781 g
Answer: 781 g
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