Question 18 (2 points)
In the equation below, Nitrogen gas (N2) and Hydrogen gas (H2) react to produce Ammonia (NH3).
If 6.30 grams of Hydrogen reacts completely with nitrogen, how many grams of ammonia will be produced?
The molar mass of Hydrogen gas (H2)is 2.0 grams/mol.
The molar mass of Ammonia (NH3) is 17.0 grams/mol.
If you are unsure how to convert from grams to grams, please see the example problem linked HERE.
a
35.7 grams of NH3
b
38.5 grams of NH3
c
143 grams of NH3
d
80.3 grams of NH3
To solve this problem, we need to first determine the amount of Nitrogen gas (N2) that reacts with the given amount of Hydrogen gas (H2), and then use stoichiometry to find the amount of Ammonia (NH3) produced.
1. Calculate the moles of Hydrogen gas (H2):
6.30 grams H2 x (1 mol H2 / 2.0 grams H2) = 3.15 mol H2
2. Since the reaction is balanced with a 1:1 ratio between Hydrogen gas and Nitrogen gas, the number of moles of Nitrogen gas reacting will be the same as Hydrogen gas:
Moles of N2 = 3.15 mol
3. Calculate the molar mass of Ammonia (NH3):
Molar mass of NH3 = 17.0 grams/mol
4. Use the mole ratio from the balanced chemical equation to find the moles of Ammonia (NH3) produced:
Moles of NH3 = 3.15 mol
5. Convert moles of NH3 to grams of NH3:
3.15 mol NH3 x (17.0 grams NH3 / 1 mol NH3) = 53.55 grams NH3
Therefore, when 6.30 grams of Hydrogen gas reacts completely, 53.55 grams of Ammonia will be produced.
The closest answer choice is:
b) 38.5 grams of NH3