NaCl + NH3+CO2+H2O--> NaHCO3 + NH4Cl
if 9.93g of NaCl reacts with excesses of the other reactants and 4.31g of NaHCO3 is isolated, what is the percent yield of the reaction?
Given :
Reaction :
NaCl + NH3+CO2+H2O-- > NaHCO3 + NH4Cl
Mass of NaCl = 9.93 g
Actual mass of NaHCO3 isolated = 4.31 g
Calculation of moles of NaCl
Moles of NaCl = Mass of NaCl / molar mass of NaCl
= 9.93 g / 58.443 g per mol
= 0.1699 mol
Calculation of moles of NaHCO3 by using moles of NaCl
Mol ratio of NaHCO3 : NaCl is 1 : 1
Number of moles of NaHCO3 = Number of moles of NaCl x 1 mol NaHCO3 / 1 mol NaCl
= 0.1699 mol NaHCO3
Calculation of mass (Theoretical yield) of NaHCO3
= Moles of NaHCO3 x molar mass of NaHCO3
= 0.1699 mol NaHCO3 x 84.0059 g per mol
= 14.27 g
Calculation of percent yield :
Percent yield = (Actual mass / theoretical mass ) x 100
= (4.31 g / 14.27 g ) x 100
= 0.3020 x 100
= 30.2 %
Percent yield = 30.2 %
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