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.

We are given;

We are required to identify the theoretical yield of the reaction, the excess reactant and the rate limiting reagent.

N₂ + 3H₂ → 2NH₃

From the reaction 1 mole of nitrogen reacts with 3 moles of Hydrogen gas.

Moles of Nitrogen gas

Moles = Mass ÷ Molar mass

Molar mass of nitrogen gas = 28.0 g/mol

Moles of Nitrogen gas = 100 g ÷ 28 g/mol 3.57 moles

Moles of Hydrogen gas

Molar mass of Hydrogen gas = 2.02 g/mol

Moles = 100 g ÷ 2.02 g/mol

          = 49.50 moles

1 mole of nitrogen reacts to from 2 moles of ammonia gas

Therefore;

Moles of ammonia gas produced = Moles of nitrogen × 2

                                                       = 3.57 moles × 2

                                                       = 7.14 moles

But; molar mass of Ammonia gas is = 17.03 g/mol

Therefore;

Mass of ammonia gas produced = 7.14 moles × 17.03 g/mol

                                                      = 121.59 g

                                                     = 121.60 g

Thus, the theoretical amount of ammonia gas produced is 121.60 g

b

explanation:

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