A 0.5962g sample of iron ore is dissolved in HCLO4. All the iron present is oxidize to FE3+ the solution is filtered to remove solid matrix material and make basic with addition of ammonium hydroxide. the iton ppt as FE(OH)3.xH2O gel. the ppt is collected in a cistern crucible was ignited to produce FE2SO3 what is the wt % of the iron in the sample if the analysis produce 0.3210g of FE2O3
To find the weight percent of iron in the sample, we need to calculate the mass of iron in the FE2O3 and then divide it by the mass of the original sample.
1. Calculate the molar mass of FE2O3:
- The molar mass of iron (Fe) is 55.845 g/mol.
- The molar mass of oxygen (O) is 16.00 g/mol.
- Since FE2O3 contains two iron atoms and three oxygen atoms, the molar mass of FE2O3 is 2 * 55.845 + 3 * 16.00 = 159.685 g/mol.
2. Calculate the moles of FE2O3:
- The mass of FE2O3 obtained in the analysis is 0.3210 g.
- Divide the mass by the molar mass of FE2O3 to find the number of moles: 0.3210 g / 159.685 g/mol = 0.0020119 mol.
3. Determine the moles of iron (Fe):
- Since FE2O3 has a 2:3 ratio of iron to FE2O3, there are twice as many moles of iron: 0.0020119 mol * 2 = 0.0040238 mol.
4. Convert moles of iron to grams:
- Multiply the number of moles of iron by the molar mass of iron: 0.0040238 mol * 55.845 g/mol = 0.2246 g.
5. Calculate the weight percent of iron:
- Divide the mass of iron by the mass of the original sample and multiply by 100%: 0.2246 g / 0.5962 g * 100% = 37.7%.
Therefore, the weight percent of iron in the sample is 37.7%.