calculate the mass of sulfur in 6.0 g of Iron (III) sulfate
iron(III) sulfate = Fe2(SO4)3
6.0g/molar mass Fe2(SO4)3 = moles Fe2(SO4)3.
moles S = 3 times that.
grams S = moles S x atomic mass S.
To calculate the mass of sulfur in 6.0 g of Iron (III) sulfate, we'll need to determine the molar mass of Iron (III) sulfate and then find the ratio of sulfur to Iron (III) sulfate in the compound.
1. Determine the molar mass of Iron (III) sulfate (Fe2(SO4)3):
- The molar mass of Fe is 55.845 g/mol (from the periodic table).
- The molar mass of S is 32.06 g/mol.
- The molar mass of O is 16.00 g/mol.
Thus, the molar mass of Iron (III) sulfate can be calculated as:
(2 x molar mass of Fe) + (3 x molar mass of S) + (12 x molar mass of O)
= (2 x 55.845 g/mol) + (3 x 32.06 g/mol) + (12 x 16.00 g/mol)
2. Calculate the molar mass of Iron (III) sulfate:
= 111.69 g/mol + 96.18 g/mol + 192.00 g/mol
= 399.87 g/mol
3. Find the molar ratio of sulfur to Iron (III) sulfate:
- In Iron (III) sulfate (Fe2(SO4)3), there are 3 sulfur atoms in 1 formula unit.
Therefore, the molar ratio of sulfur to Iron (III) sulfate is 3:1.
4. Calculate the mass of sulfur in 6.0 g of Iron (III) sulfate:
- First, find the number of moles of Iron (III) sulfate:
Moles = Mass / Molar mass
Moles = 6.0 g / 399.87 g/mol
- Next, use the molar ratio to determine the moles of sulfur:
Moles of sulfur = Moles of Iron (III) sulfate x (3/1)
- Finally, calculate the mass of sulfur:
Mass = Moles of sulfur x Molar mass of sulfur
Plug in the values to find the mass of sulfur.
Determine the mass of sulfur in 6.0 g of Iron (III) sulfate following the steps mentioned above.