The Haber process is used to synthesize ammonia from hydrogen and nitrogen. How much hydrogen is required to produce 42.8 kg of ammonia?
N2 + 3H2 ==> 2NH3
mols NH3 = grams/molar mass = 42800/17 = ?
Using the coefficients in the balanced equation, convert mols NH3 to mols H2.
Now convert mols H2 to grams. g = molx x molar mass.
To determine the amount of hydrogen required to produce 42.8 kg of ammonia using the Haber process, we need to use the balanced chemical equation for the reaction.
The balanced chemical equation for the Haber process is as follows:
N2 + 3H2 -> 2NH3
From this equation, we can see that for every 1 mole of nitrogen (N2) that reacts, 3 moles of hydrogen (H2) are required to produce 2 moles of ammonia (NH3).
Step 1: Determine the molar mass of ammonia (NH3)
The molar mass of ammonia (NH3) can be calculated by adding up the atomic masses of each element.
Molar mass of NH3 = 1(1.01) + 3(1.01) = 17.03 g/mol
Step 2: Determine the molar mass of hydrogen (H2)
Since hydrogen gas (H2) exists as a diatomic molecule, we multiply the atomic mass of hydrogen by 2.
Molar mass of H2 = 2(1.01) = 2.02 g/mol
Step 3: Convert the mass of ammonia to moles
Divide the given mass of ammonia (42.8 kg) by its molar mass to convert it to moles.
Number of moles of NH3 = (42.8 kg) / (17.03 g/mol) = 2512.16 mol
Step 4: Determine the moles of hydrogen required
From the balanced chemical equation, we know that for every 2 moles of ammonia produced, 3 moles of hydrogen are required.
So, to find the moles of hydrogen needed, we can use the following ratio:
3 moles H2 / 2 moles NH3
Number of moles of H2 = (2512.16 mol of NH3) x (3 mol of H2 / 2 mol of NH3) = 3768.24 mol
Step 5: Convert the moles of hydrogen to grams
Multiply the number of moles of hydrogen by its molar mass to convert it to grams.
Mass of H2 = (3768.24 mol) x (2.02 g/mol) = 7609.65 g
Therefore, to produce 42.8 kg of ammonia, approximately 7609.65 grams (or 7.6 kg) of hydrogen would be required.
To determine the amount of hydrogen required to produce 42.8 kg of ammonia using the Haber process, we need to know the balanced chemical equation for the reaction.
The balanced chemical equation for the synthesis of ammonia (NH3) from hydrogen (H2) and nitrogen (N2) is:
N2 + 3H2 → 2NH3
From the balanced equation, we can see that 3 moles of hydrogen are required to produce 2 moles of ammonia.
To calculate the amount of hydrogen needed, we will use the molar mass of hydrogen, which is 2.016 grams/mole.
Step 1: Calculate the molar mass of ammonia (NH3).
The molar mass of NH3 = (1 mol of N) + (3 mol of H)
= (14.007 g/mol) + (3 * 2.016 g/mol)
≈ 17.031 g/mol
Step 2: Convert the given mass of ammonia (42.8 kg) to moles.
42.8 kg * (1000 g/1 kg) * (1 mol/17.031 g) ≈ 2511.96 mol
Step 3: Determine the moles of hydrogen required.
From the balanced equation, we know that 2 moles of ammonia require 3 moles of hydrogen.
If 2 moles of ammonia require 3 moles of hydrogen, then 2511.96 moles of ammonia will require:
(3 moles of H)/(2 moles of NH3) * 2511.96 moles of NH3 ≈ 3767.94 moles of H
Step 4: Convert the moles of hydrogen to grams.
3767.94 mol * 2.016 g/mol ≈ 7598.30 g
Therefore, approximately 7598.30 grams (or 7.5983 kg) of hydrogen is required to produce 42.8 kg of ammonia using the Haber process.