theoretical yield of the reaction is 121.38 g of NH₃ (ammonia)
limiting reactant is N₂ (nitrogen)
excess reactant is H₂ (hydrogen)
Explanation:
We have the following chemical reaction:
N₂ + 3 H₂ → 2 NH₃
Now we calculate the number of moles of each reactant:
number of moles = mass / molar weight
number of moles of N₂ = 100 / 28 = 3.57 moles
number of moles of H₂ = 100 / 2 = 50 moles
From the chemical reaction we see that 3 moles of H₂ are reacting with 1 moles of N₂, so 50 moles of H₂ are reacting with 16.66 moles of N₂ but we only have 3.57 moles of N₂ available, so the limiting reactant will be N₂ and the excess reactant will be H₂.
Knowing the chemical reaction and the limiting reactant we devise the following reasoning:
if 1 mole of N₂ produce 2 moles of NH₃
then 3.57 moles of N₂ produce X moles of NH₃
X = (3.57 × 2) / 1 = 7.14 moles of NH₃
mass = number of moles × molar weight
mass of NH₃ = 7.14 × 17 = 121.38 g
theoretical yield of the reaction is 121.38 g of NH₃
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limiting reactant
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