A 0.5962g sample of iron ore is dissolved in percloric acid (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 calculate the weight percentage of iron in the sample, we need to determine the amount of iron present in the sample.
1. Calculate the moles of FE2O3 using its molar mass:
Molar mass of FE2O3 = (2 * atomic mass of Fe) + (3 * atomic mass of O)
= (2 * 55.845 g/mol) + (3 * 16.00 g/mol)
= 111.69 g/mol
moles of FE2O3 = mass of FE2O3 / molar mass of FE2O3
= 0.3210g / 111.69 g/mol
= 0.002875 moles
2. Since FE2O3 is formed from two moles of Fe, the moles of Fe in the sample would be twice the moles of FE2O3:
moles of Fe = 2 * moles of FE2O3
= 2 * 0.002875 moles
= 0.00575 moles
3. Calculate the weight of Fe in grams:
weight of Fe = moles of Fe * molar mass of Fe
= 0.00575 moles * 55.845 g/mol
= 0.321 g
4. Finally, calculate the weight percentage of Fe in the sample:
weight percentage of Fe = (weight of Fe / weight of sample) * 100%
= (0.321 g / 0.5962 g) * 100%
= 53.9%
Therefore, the weight percentage of iron in the sample is approximately 53.9%.