How many grams of iron(II) oxalate dihydrate, Fe(C2O4)·2H2O,mass can be produced when a student begins the synthesis with 3.238 g of ammonium iron(II) disulfate hexahydrate, (NH4)2Fe(SO4)2·6H2O?
The short way is this.
3.238 x (molar mass what of you want/molar mass of what you have) = ?
To determine the mass of iron(II) oxalate dihydrate that can be produced, we first need to calculate the theoretical yield of the compound. The theoretical yield is the maximum amount of product that can be obtained from the given reactant.
Here's how you can calculate it:
1. Determine the molar mass of ammonium iron(II) disulfate hexahydrate, [(NH4)2Fe(SO4)2·6H2O]:
- Molar mass of (NH4)2Fe(SO4)2 = (2 x Molar mass of NH4) + Molar mass of Fe + (2 x Molar mass of SO4)
- Molar mass of (NH4)2Fe(SO4)2 = (2 x 18.04 g/mol) + 55.85 g/mol + (2 x 32.06 g/mol)
- Molar mass of (NH4)2Fe(SO4)2 = 392.14 g/mol
2. Convert the given mass of ammonium iron(II) disulfate hexahydrate, [(NH4)2Fe(SO4)2·6H2O], to moles:
- Moles = Mass / Molar Mass
- Moles = 3.238 g / 392.14 g/mol
3. Determine the molar ratio between ammonium iron(II) disulfate hexahydrate and iron(II) oxalate dihydrate, Fe(C2O4)·2H2O:
- From the balanced chemical equation, the molar ratio between [(NH4)2Fe(SO4)2·6H2O] and Fe(C2O4)·2H2O is 1:1.
4. Use the molar ratio to calculate the moles of iron(II) oxalate dihydrate, Fe(C2O4)·2H2O:
- Moles of Fe(C2O4)·2H2O = Moles of (NH4)2Fe(SO4)2·6H2O
5. Calculate the mass of iron(II) oxalate dihydrate, Fe(C2O4)·2H2O, using its molar mass:
- Mass = Moles x Molar Mass
- Mass = Moles of Fe(C2O4)·2H2O x Molar Mass of Fe(C2O4)·2H2O
To get the final answer, you'll need to calculate the moles of Fe(C2O4)·2H2O using the given molar ratio and then multiply it by the molar mass of Fe(C2O4)·2H2O.