Question

A reaction occurs between ammonia and carbon dioxide in the following chemical reaction: 2NH4 + CO2 → (NH2)2CO + H2O

In the process, 637.2 g of NH, are treated with 1142 g of CO2. Calculate the percent yield if 1000. g of (NH2)2CO are actually obtained.

Answer 1

number of moles of NH4 = 637.2 g / 18.038 g/mol = 35.3 mole

number of moles of CO2 = 1142g / 44.01 g/mol = 25.9 mole

from the balanced equation we can say that

2 mole of NH4 require 1 mole of CO2 so

35.3 mole of NH4 will require 17.65 mole of CO2

but we have 25.9 mole of CO2 so NH4 is limiting reactant

from the balanced equation we can say that

2 mole of NH4 produces 1 mole of (NH2)2CO so

35.3 mole of NH4 will produce 17.65 mole of (NH2)2CO

1 mole of (NH2)2CO = 60.0553 g

17.65 mole of (NH2)2CO = 1059.9 g

Therefore, theoretical yield of (NH2)2CO = 1059.9g

percent yield = (actual yield / theoretical yield)*100

100 = (actual yield / 1059.9)*100

Therefore, actual yield = 1059.9 g