What mass of carbon is contained in 3.17 x 10 exp.24 formula units of iron(III)carbonate?
To determine the mass of carbon in a given number of formula units of iron(III) carbonate, you need to know the molar mass of iron(III) carbonate and the number of moles of carbon in each formula unit.
1. Start by finding the molar mass of iron(III) carbonate (Fe2(CO3)3).
- The molar mass of iron (Fe) is 55.85 g/mol.
- The molar mass of carbon (C) is 12.01 g/mol.
- The molar mass of oxygen (O) is 16.00 g/mol.
So the molar mass of iron(III) carbonate is:
(2 * 55.85 g/mol (for Fe)) + (3 * (12.01 g/mol (for C) + 3 * 16.00 g/mol (for O))) = 291.86 g/mol.
2. Next, convert the given number of formula units of iron(III) carbonate to moles.
To convert formula units to moles, you need Avogadro's number, which states that 1 mole contains 6.022 x 10^23 formula units.
So, 3.17 x 10^24 formula units × (1 mol / 6.022 x 10^23 formula units) = 5.27 moles of iron(III) carbonate.
3. Finally, calculate the mass of carbon.
Since there are three carbon atoms in each formula unit of iron(III) carbonate, the mass of carbon can be calculated as:
5.27 moles of iron(III) carbonate × 3 moles of carbon / 1 mole of iron(III) carbonate × 12.01 g/mol (atomic mass of carbon) = 191.04 g.
Therefore, the mass of carbon in 3.17 x 10^24 formula units of iron(III) carbonate is approximately 191.04 grams.