Calculate the percentage of water in Aluminum bromide hexahydrate, AlBr3 •6H2O.
mm = molar mass
(6*mmH2O)/(mm AlBr3.6H2O)
Post your work if you need further help.
Why did the chemist become a stand-up comedian? Because they found they had a great "pH" of humor! Now, let's dive into the calculation.
To find the percentage of water, we need to know the molar mass of water and the molar mass of the compound AlBr3 •6H2O.
The molar mass of water (H2O) is roughly 18.015 g/mol.
The molar mass of Aluminum bromide hexahydrate (AlBr3 •6H2O) is roughly (269.8 + (6 * 18.015)) g/mol.
Now let's calculate the percentage of water in Aluminum bromide hexahydrate:
Percentage of water = (molar mass of water / molar mass of AlBr3 •6H2O) * 100
Percentage of water = (18.015 / (269.8 + (6 * 18.015))) * 100
Now, if my calculations go smoothly, the percentage of water should be approximately 52.9%.
Remember, my specialty is humor, not precise calculations. So take these numbers with a pinch of sodium chloride, or in simpler terms, salt!
To calculate the percentage of water in Aluminum bromide hexahydrate, AlBr3 • 6H2O, follow these steps:
Step 1: Determine the molar mass of the compound
The molar mass is the sum of the atomic masses of all the atoms in the compound.
The atomic masses are as follows:
Aluminum (Al) = 26.98 g/mol
Bromine (Br) = 79.90 g/mol
Hydrogen (H) = 1.01 g/mol
Oxygen (O) = 16.00 g/mol
To calculate the molar mass of Aluminum bromide (AlBr3), you multiply the atomic mass of each element by the number of atoms present and add them up:
Al: 1 atom × 26.98 g/mol = 26.98 g/mol
Br: 3 atoms × 79.90 g/mol = 239.70 g/mol
Total molar mass of AlBr3 = 26.98 g/mol + 239.70 g/mol = 266.68 g/mol
For water (H2O), the molar mass is calculated as:
H: 2 atoms × 1.01 g/mol = 2.02 g/mol
O: 1 atom × 16.00 g/mol = 16.00 g/mol
Total molar mass of H2O = 2.02 g/mol + 16.00 g/mol = 18.02 g/mol
Since there are 6 moles of water (H2O) in AlBr3 • 6H2O, we multiply the molar mass of H2O by 6:
Total molar mass of 6H2O = 6 × 18.02 g/mol = 108.12 g/mol
Step 2: Calculate the percentage of water
The percentage of water is calculated by dividing the molar mass of water (H2O) by the molar mass of the entire compound (AlBr3 • 6H2O), and then multiplying by 100.
Percentage of water = (molar mass of 6H2O / molar mass of AlBr3 • 6H2O) × 100
= (108.12 g / 374.80 g) × 100
= 28.84%
Therefore, the percentage of water in Aluminum bromide hexahydrate, AlBr3 • 6H2O, is approximately 28.84%.
To calculate the percentage of water in Aluminum bromide hexahydrate (AlBr3 •6H2O), you need to determine the molar mass of the water and the total molar mass of the compound.
Molar mass of water (H2O):
- Hydrogen (H) has a molar mass of 1.008 g/mol (2 atoms)
- Oxygen (O) has a molar mass of 16.00 g/mol (1 atom)
Therefore, the molar mass of water (H2O) is (2 * 1.008) + 16.00 = 18.016 g/mol.
Molar mass of Aluminum bromide hexahydrate (AlBr3 •6H2O):
- Aluminum (Al) has a molar mass of 26.98 g/mol (1 atom)
- Bromine (Br) has a molar mass of 79.90 g/mol (3 atoms)
- Water (H2O) has a molar mass of 18.016 g/mol (6 molecules)
Therefore, the molar mass of Aluminum bromide hexahydrate (AlBr3 •6H2O) is (26.98 + (3 * 79.90)) + (6 * 18.016) = 375.16 g/mol.
To calculate the percentage of water:
1. Determine the molar mass of water (H2O) and Aluminum bromide hexahydrate (AlBr3 •6H2O).
2. Calculate the mass of water in one mole of Aluminum bromide hexahydrate by multiplying the molar mass of water (H2O) by 6.
Mass of water = 18.016 g/mol * 6 = 108.096 g/mol.
3. Divide the mass of water by the total molar mass of Aluminum bromide hexahydrate and multiply by 100 to get the percentage of water.
Percentage of water = (108.096 g/mol / 375.16 g/mol) * 100 = 28.8%.
Therefore, the percentage of water in Aluminum bromide hexahydrate is approximately 28.8%.