The reaction of 9.15 g of carbon with excess O2 yields 8.25 g of CO2. What is the percent yield of this reaction?
Molar mass of C = 12.01 g/mol
mass(C)= 9.15 g
use:
number of mol of C,
n = mass of C/molar mass of C
=(9.15 g)/(12.01 g/mol)
= 0.7619 mol
Balanced chemical equation is:
C + O2 ---> CO2
Molar mass of CO2,
MM = 1*MM(C) + 2*MM(O)
= 1*12.01 + 2*16.0
= 44.01 g/mol
According to balanced equation
mol of CO2 formed = (1/1)* moles of C
= (1/1)*0.7619
= 0.7619 mol
use:
mass of CO2 = number of mol * molar mass
= 0.7619*44.01
= 33.53 g
% yield = actual mass*100/theoretical mass
= 8.25*100/33.53
= 24.6 %
Answer: 24.6 %
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