Write a half-reaction for the oxidation of the manganese in MnCO3(s) to MnO2(s) in neutral groundwater where the carbonate-conta
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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 =
Molar mass of NH₃ = 14 + (3x1) = 17g/mol
Number of moles of NH₃ = = 7.765mole
Number of moles of CO₂ =
Molar mass of CO₂ = 12 + (2 x 16) = 44g/mol
Number of moles of CO₂ = = 4.805mole
From the reaction equation:
2 moles of NH₃ reacted with 1 mole of CO₂
so 7.765 mole of NH₃ will require 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.