Question

Please help ASAP:

If 100.0g of nitrogen is reacted with 100.0g of hydrogen, what is the theoretical yield of the reaction? What is the excess reactant? What is the limiting reactant? Show your work.

Answer 1

Theoretical yield = 122.4 g

Hydrogen is in excess.

Nitrogen is limiting reactant.

Step-by-step 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