Answer:
Theoretical yield = 122.4 g
Hydrogen is in excess.
Nitrogen is limiting reactant.
Explanation:
Given data:
Mass of hydrogen = 100 g
Mass of nitrogen = 100 g
Theoretical yield of reaction = ?
What is excess reactant = ?
What is limiting reactant = ?
Chemical equation:
N₂+ 3H₂ → 2NH₃
Number of moles of N₂:
Number of moles = Mass /molar mass
Number of moles = 100 g / 28 g/mol
Number of moles = 3.6 mol
Number of moles of H₂:
Number of moles = Mass /molar mass
Number of moles = 100 g / 2g/mol
Number of moles = 50 mol
Now we will compare the moles of NH₃ with hydrogen and nitrogen .
H₂ : NH₃
3 : 2
50 : 2/3×50= 33.3 mol
N₂ : NH₃
1 : 2
3.6 : 2 × 3.6 = 7.2 mol
The number of moles of NH₃ produced by nitrogen are less it will be limiting reactant.
Theoretical yield of reaction:
Mass of NH₃ = moles × molar mass
Mass = 7.2 mol × 17 g/mol
Mass = 122.4 g
