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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.

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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

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