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: Theoretical yield is 121.60 g of NH₃ Excess reactant is H₂ Rate limiting reactant is N₂ Explanation:

We are given;

100 g of Nitrogen 100 g of hydrogen

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

We first write the equation for the reaction between nitrogen and hydrogen;

N₂ + 3H₂ → 2NH₃

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

Secondly we determine the moles of nitrogen gas given and hydrogen gas given;

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

From the mole ratio given by the equation, 1 mole of nitrogen requires 3 moles of Hydrogen gas. Thus, 3.57 moles of Nitrogen gas requires (3.57 * 3) 10.71 moles of Hydrogen gas. This means, Nitrogen gas is the rate limiting reagent and hydrogen gas is the excess reactant. Third calculate the theoretical yield of the reaction.

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