Answer:
NH₃ is the limiting reagent
Explanation:
Mass of ammonia = 132.0kg
Mass of carbon dioxide = 211.4kg
Mass of urea = 172.7kg
Unknown:
Limiting reagent = ?
Solution
First, we write the balanced stoichiometeric equation:
2NH₃ + CO₂ → CH₄N₂O + H₂O
The reactant that is present in short supply determines the amount of product that is formed in a reaction. This reactant is called the limiting reagent.
To establish the limiting reagent, we need to go find out what is happening at the start of the reaction:
Convert the masses of the reactants to moles.
Number of moles of NH₃ = [tex]\frac{mass}{molar mass}[/tex]
Molar mass of NH₃ = 14 + (3x1) = 17g/mol
Number of moles of NH₃ = [tex]\frac{132}{17}[/tex] = 7.765mole
Number of moles of CO₂ = [tex]\frac{mass}{molar mass}[/tex]
Molar mass of CO₂ = 12 + (2 x 16) = 44g/mol
Number of moles of CO₂ = [tex]\frac{211.4}{44}[/tex] = 4.805mole
From the reaction equation:
2 moles of NH₃ reacted with 1 mole of CO₂
so 7.765 mole of NH₃ will require [tex]\frac{7.765}{2}[/tex]mole, 3.883 of CO₂
But we are given 4.805mole of CO₂.
Therefore, CO₂ gas is in excess and NH₃ is the limiting reagent.
The limiting reactant for the synthesis of CH₄N₂O given the data is ammonia, NH₃
2NH₃ + CO₂ —> CH₄N₂O + H₂O
Molar mass of NH₃ = 17 g/mole
Mass of NH₃ from the balanced equation = 2 × 17 = 34 g = 0.034 Kg
Molar mass of CO₂ = 44 g/mole
Mass of CO₂ from the balanced equation = 1 × 44 = 44 g = 0.044 Kg
SUMMARY
From the balanced equation above,
0.034 Kg of NH₃ reacted with 0.044 Kg of CO₂
From the balanced equation above,
0.034 Kg of NH₃ reacted with 0.044 Kg of CO₂
Therefore,
132 Kg of NH₃ will react with = (132 × 0.044) / 0.034 = 170.8 of Kg of CO₂
From the calculation made above, we can see that only 170.8 of Kg of CO₂ out of 172.7 Kg given is needed to react completely with 132 Kg of NH₃.
Thus, NH₃ is the limiting reactant
Learn more about stoichiometry:
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