When 27.7 g of acetylene reacts with hydrogen, 25.0 g of ethane
is produced. What is the percent yield of C2H6 for the
reaction?
C2H2(g)+2H2(g)→C2H6(g)
Molar mass of C2H2,
MM = 2*MM(C) + 2*MM(H)
= 2*12.01 + 2*1.008
= 26.036 g/mol
mass of C2H2 = 27.7 g
mol of C2H2 = (mass)/(molar mass)
= 27.7/26.04
= 1.064 mol
Balanced chemical equation is:
C2H2(g)+2H2(g)→C2H6(g)
According to balanced equation
mol of C2H6 formed = moles of C2H2
= 1.064 mol
Molar mass of C2H6,
MM = 2*MM(C) + 6*MM(H)
= 2*12.01 + 6*1.008
= 30.068 g/mol
mass of C2H6 = number of mol * molar mass
= 1.064*30.07
= 31.99 g
% yield = actual mass*100/theoretical mass
= 25*100/31.99
= 78.15 %
Answer: 78.2 %
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