Question

The Haber Process involves nitrogen gas combining with hydrogen gas to produce ammonia.

N2 + 3H2 → 2NH3

10.0 grams of nitrogen gas is reacted with 10.0 grams of hydrogen gas.

Find the following: the molar mass of reactants and products, the limiting reactant, the excess reactant, the amount of ammonia produced.

Question 1 options:


28.02 grams


12.16 grams


nitrogen gas


17.04 grams


hydrogen gas



2.02 grams

1.
The limiting reactant

2.
The excess reactant

3.
Molar mass of hydrogen gas

4.
Molar mass of nitrogen gas

5.
Molar mass of ammonia (NH3)

6.
Amount of ammonia produced

Answer 1

The limiting reactant: Nitrogen gas (N2)

The excess reactant: Hydrogen gas (H2)

Molar mass of hydrogen gas: 2.016 grams/mol

Molar mass of nitrogen gas: 28.02 grams/mol

Molar mass of ammonia (NH3): 17.04 grams/mol

To find the amount of ammonia produced we can use the concept of limiting reactant. The limiting reactant is the one that runs out first and limits the amount of product that can be formed. In this case, we have 10.0 grams of nitrogen gas and 10.0 grams of hydrogen gas.

To find the amount of ammonia produced, we need to find out which reactant is limiting.

N2 + 3H2 → 2NH3

1 mole of N2 and 3 mole of H2 required for 1 mole of NH3.

10.0 g N2 / 28.02 g/mol N2 = 0.357 moles N2

10.0 g H2 / 2.016 g/mol H2 = 4.96 moles H2

To find the amount of ammonia produced we will use the limiting reactant N2, and it's stoichiometry in the reaction.

0.357 moles N2 * 2 moles NH3 / 1 mole N2 = 0.714 moles NH3

And to find the mass of ammonia produced we can use the molar mass of NH3

0.714 moles NH3 * 17.04 g/mol NH3 = 12.16 grams

Amount of ammonia produced: 12.16 grams