Nitrogen gas reacts with hydrogen gas to produce ammonia via the following reaction:
N2 (g) + 3H2(g) →2NH3 (g)
How many grams of H2 are needed to react with 3.80 g of N2?
Express your answer with the appropriate units
To solve this problem, we need to use the stoichiometry of the reaction. From the balanced equation, we can see that 3 moles of hydrogen gas (H2) are required to react with 1 mole of nitrogen gas (N2).
1 mole of N2 has a molar mass of 14.01 g/mol, so 3.80 g of N2 is equal to 3.80 g / 14.01 g/mol = 0.271 mol of N2.
Therefore, we need 3 times that amount of H2, so we need 0.271 mol × 3 = 0.813 mol of H2.
The molar mass of H2 is 2.02 g/mol, so 0.813 mol of H2 is equal to 0.813 mol × 2.02 g/mol = 1.64 g of H2.
Therefore, 1.64 grams of H2 are needed to react with 3.80 g of N2.
To determine the amount of H2 required to react with 3.80 g of N2, we must first calculate the molar masses of N2 and H2.
The molar mass of N2 is:
N2 = 2*14.01 g/mol
N2 = 28.02 g/mol
The molar mass of H2 is:
H2 = 2*1.01 g/mol
H2 = 2.02 g/mol
Next, we can use stoichiometry to determine the ratio between N2 and H2 in the balanced chemical equation.
From the balanced equation, we can see that 1 mole of N2 reacts with 3 moles of H2. Therefore, the ratio of moles is 1:3.
Now, we can convert the grams of N2 to moles using the molar mass of N2:
moles of N2 = mass / molar mass
moles of N2 = 3.80 g / 28.02 g/mol
moles of N2 ≈ 0.136 mol
Since the ratio of N2 to H2 is 1:3, we can multiply the moles of N2 by the mole ratio to find the moles of H2:
moles of H2 = moles of N2 * (3 moles of H2 / 1 mole of N2)
moles of H2 = 0.136 mol * 3
moles of H2 ≈ 0.408 mol
Finally, we can convert moles of H2 to grams using the molar mass of H2:
grams of H2 = moles of H2 * molar mass
grams of H2 = 0.408 mol * 2.02 g/mol
grams of H2 ≈ 0.825 g
Therefore, approximately 0.825 grams of H2 are needed to react with 3.80 grams of N2.
To find out how many grams of H2 are needed to react with 3.80 g of N2, we need to use stoichiometry. Stoichiometry allows us to determine the amount of one substance needed to react with another based on the balanced equation.
Looking at the balanced equation:
N2 (g) + 3H2(g) → 2NH3 (g)
We can see that for every 1 mole of N2, we need 3 moles of H2 to react and produce 2 moles of NH3.
Step 1: Convert grams of N2 to moles of N2.
To do this, we need the molar mass of N2, which is approximately 28.02 g/mol.
Moles of N2 = Mass of N2 / Molar mass of N2
Moles of N2 = 3.80 g / 28.02 g/mol ≈ 0.1358 mol
Step 2: Use the mole ratio from the balanced equation to find moles of H2.
From the balanced equation, we know that 1 mole of N2 reacts with 3 moles of H2.
Moles of H2 = Moles of N2 × (3 moles of H2 / 1 mole of N2)
Moles of H2 = 0.1358 mol × (3 mol H2 / 1 mol N2) ≈ 0.4074 mol
Step 3: Convert moles of H2 to grams of H2.
To do this, we need the molar mass of H2, which is approximately 2.02 g/mol.
Mass of H2 = Moles of H2 × Molar mass of H2
Mass of H2 = 0.4074 mol × 2.02 g/mol ≈ 0.823 g
Therefore, approximately 0.823 grams of H2 are needed to react with 3.80 grams of N2.