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.

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

step-by-step explanation:

whole numbers, zero or greater

its going to be mutualism cuz they both benefit from the relationship.

~batmans wife dun dun