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, and the amount of ammonia produced.
Question 1 options:
28.02 grams
17.04 grams
2.02 grams
hydrogen gas
nitrogen gas
12.13 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
1. The limiting reactant is the reactant that will be completely consumed in the reaction and determine the maximum amount of product that can be formed. To determine the limiting reactant, we need to convert the masses of the reactants to moles.
Molar mass of nitrogen gas (N2) = 28.02 grams/mole
Molar mass of hydrogen gas (H2) = 2.02 grams/mole
Moles of nitrogen gas = 10.0 grams / 28.02 grams/mole = 0.357 moles
Moles of hydrogen gas = 10.0 grams / 2.02 grams/mole = 4.95 moles
Using the balanced equation, we can see that the ratio of moles of nitrogen gas to ammonia is 1:2, and the ratio of moles of hydrogen gas to ammonia is 3:2. This means that 1 mole of nitrogen gas results in the formation of 2 moles of ammonia, and 3 moles of hydrogen gas results in the formation of 2 moles of ammonia.
Therefore, we can calculate the theoretical amount of ammonia that can be formed from the given moles of nitrogen gas and hydrogen gas.
Theoretical moles of ammonia from nitrogen gas = 0.357 moles of nitrogen gas x (2 moles of ammonia / 1 mole of nitrogen gas) = 0.714 moles
Theoretical moles of ammonia from hydrogen gas = 4.95 moles of hydrogen gas x (2 moles of ammonia / 3 moles of hydrogen gas) = 3.30 moles
Since the ratio of moles of ammonia from nitrogen gas to hydrogen gas is smaller than 1:3, the limiting reactant is nitrogen gas.
2. The excess reactant is the reactant that is not completely consumed in the reaction and is left over after the reaction is complete. In this case, hydrogen gas is the excess reactant because there is still some remaining after the reaction.
3. Molar mass of hydrogen gas = 2.02 grams/mole
4. Molar mass of nitrogen gas = 28.02 grams/mole
5. Molar mass of ammonia (NH3) = 17.04 grams/mole
6. The amount of ammonia produced can be calculated based on the limiting reactant. Since 1 mole of nitrogen gas produces 2 moles of ammonia, and we have 0.357 moles of nitrogen gas, the amount of ammonia produced can be calculated as follows:
Amount of ammonia produced = 0.357 moles of nitrogen gas x (2 moles of ammonia / 1 mole of nitrogen gas) x (17.04 grams/mole) = 12.19 grams
Therefore, the answers are:
1. The limiting reactant: nitrogen gas
2. The excess reactant: hydrogen gas
3. Molar mass of hydrogen gas: 2.02 grams/mole
4. Molar mass of nitrogen gas: 28.02 grams/mole
5. Molar mass of ammonia (NH3): 17.04 grams/mole
6. Amount of ammonia produced: 12.19 grams