How many grams of H2 are needed to produce 11.80g of NH3?
Express your answer numerically in grams.
To find out how many grams of H2 are needed to produce 11.80g of NH3, we need to use the balanced chemical equation for the reaction.
The equation for the formation of ammonia (NH3) from hydrogen gas (H2) is:
N2 + 3H2 -> 2NH3
From the equation, we can see that 3 moles of hydrogen gas (H2) react to produce 2 moles of ammonia (NH3). Therefore, we need to convert the given mass of NH3 into moles and then use the molar ratio to find the corresponding mass of H2.
Step 1: Calculate the number of moles of NH3.
Using the molar mass of NH3 (17.03 g/mol), we can calculate the number of moles of NH3:
moles of NH3 = mass of NH3 / molar mass of NH3
moles of NH3 = 11.80 g / 17.03 g/mol
moles of NH3 ≈ 0.692 moles
Step 2: Use the molar ratio to find the number of moles of H2.
From the balanced equation, we know that the molar ratio of H2 to NH3 is 3:2. Therefore:
moles of H2 = moles of NH3 * (3 moles of H2 / 2 moles of NH3)
moles of H2 ≈ 0.692 moles * (3/2)
moles of H2 ≈ 1.038 moles
Step 3: Convert moles of H2 to grams.
To convert moles of H2 to grams, we need to know the molar mass of H2, which is 2.02 g/mol.
mass of H2 = moles of H2 * molar mass of H2
mass of H2 ≈ 1.038 moles * 2.02 g/mol
mass of H2 ≈ 2.1 g
Therefore, approximately 2.1 grams of H2 are needed to produce 11.80 grams of NH3.