Nitrogen gas reacts with hydrogen gas to produce ammonia via the following reaction:
N2 (g) + 3H2(g) →2NH3 (g)
How many grams of NH3 can be produced from 13.0 g of H2?
Express your answer with the appropriate units.
To find the number of grams of NH3 produced from 13.0 g of H2, we need to use stoichiometry.
From the balanced chemical equation, we can see that the mole ratio of H2 to NH3 is 3:2. This means that for every 3 moles of H2, 2 moles of NH3 are produced.
First, we need to determine the number of moles of H2 in 13.0 g of H2. To do this, we use the molar mass of H2.
Molar mass of H2 = 2.02 g/mol
Moles of H2 = (mass of H2) / (molar mass of H2)
= 13.0 g / 2.02 g/mol
= 6.44 mol
Now, using the mole ratio of H2 to NH3, we can determine the number of moles of NH3 produced.
Moles of NH3 = (moles of H2) * (2 moles NH3 / 3 moles H2)
= 6.44 mol * (2/3)
= 4.29 mol
Finally, we can find the mass of NH3 produced from the number of moles of NH3.
Molar mass of NH3 = 17.03 g/mol
Mass of NH3 = (moles of NH3) * (molar mass of NH3)
= 4.29 mol * 17.03 g/mol
= 73.01 g
Therefore, 13.0 g of H2 can produce 73.01 g of NH3.
To solve this problem, we need to use stoichiometry, which is a way to calculate the amounts of reactants and products in a chemical reaction.
First, let's consider the balanced equation:
N2(g) + 3H2(g) → 2NH3(g)
From the balanced equation, we can see that 3 moles of H2 react to produce 2 moles of NH3.
1. Calculate the moles of H2:
Given mass of H2 = 13.0 g
Molar mass of H2 = 2.016 g/mol (approximately)
Number of moles of H2 = mass of H2 / molar mass of H2
Number of moles of H2 = 13.0 g / 2.016 g/mol ≈ 6.45 mol
2. Use the stoichiometry ratio to determine the moles of NH3 produced:
From the balanced equation, we know that:
3 moles of H2 reacts to produce 2 moles of NH3
Using the stoichiometry ratio:
Number of moles of NH3 = (Number of moles of H2) × (2 moles of NH3 / 3 moles of H2)
Number of moles of NH3 = 6.45 mol × (2/3) ≈ 4.30 mol
3. Convert moles of NH3 to grams:
Molar mass of NH3 = 17.031 g/mol (approximately)
Mass of NH3 = number of moles of NH3 × molar mass of NH3
Mass of NH3 = 4.30 mol × 17.031 g/mol ≈ 73.30 g
So, approximately 73.30 grams of NH3 can be produced from 13.0 grams of H2.
To find the grams of NH3 produced from H2, we need to use stoichiometry. Stoichiometry is a way to calculate the quantities of reactants and products in a chemical reaction.
The balanced equation tells us that 3 moles of H2 reacts with 2 moles of NH3. We can convert the given mass of H2 to moles using its molar mass.
First, let's calculate the number of moles of H2:
Molar mass of H2 = 2 g/mol
Moles of H2 = Mass of H2 / Molar mass of H2
Moles of H2 = 13.0 g / 2 g/mol
Moles of H2 = 6.5 mol
According to the balanced equation, 3 moles of H2 react to produce 2 moles of NH3. From this ratio, we can determine the moles of NH3:
Moles of NH3 = (2/3) * Moles of H2
Moles of NH3 = (2/3) * 6.5 mol
Moles of NH3 = 4.33 mol
Finally, we can convert the moles of NH3 to grams using its molar mass:
Molar mass of NH3 = 17 g/mol (N2) + 3(1 g/mol) (H2)
Molar mass of NH3 = 17 g/mol + 3 g/mol
Molar mass of NH3 = 20 g/mol
Grams of NH3 = Moles of NH3 * Molar mass of NH3
Grams of NH3 = 4.33 mol * 20 g/mol
Grams of NH3 = 86.6 g
Therefore, 13.0 g of H2 can produce 86.6 g of NH3.