A 0.5962g sample of iron ore is dissloved in acid producing Fe3+. Though a series of reactions, the iron precipitates as the Fe(OH)3. The precipitates is heated, forming solid Fe2O3. What is the mass % of iron in the sample if the analysis produced 0.3210g Fe2O3?
figure the percent iron in Fe2O3..
percent= 2*atomicmassFe/formulamassFe2O3
then, percent in the sample
= percentabove*.3210/.5962
To find the mass percentage of iron in the sample, you need to divide the mass of iron by the mass of the sample and then multiply by 100 to express the result as a percentage.
First, you need to determine the mass of iron in the 0.3210g of Fe2O3. To do this, you need to understand the stoichiometry of the reaction between Fe(OH)3 and Fe2O3.
The balanced chemical equation for the conversion of Fe(OH)3 to Fe2O3 is:
2 Fe(OH)3 → Fe2O3 + 3 H2O
From the equation, we can see that the molar ratio between Fe(OH)3 and Fe2O3 is 2:1. This means that 2 moles of Fe(OH)3 will produce 1 mole of Fe2O3.
Since we know the molar mass of Fe2O3 (159.688 g/mol), we can now calculate the number of moles of Fe2O3 using its mass:
Number of moles of Fe2O3 = mass of Fe2O3 / molar mass of Fe2O3
Number of moles of Fe2O3 = 0.3210g / 159.688 g/mol
Next, we can use the stoichiometry from the balanced equation to determine the number of moles of Fe(OH)3:
Number of moles of Fe(OH)3 = 2 * Number of moles of Fe2O3
Now that we know the number of moles of Fe(OH)3, we can find the mass of Fe(OH)3:
Mass of Fe(OH)3 = Number of moles of Fe(OH)3 * molar mass of Fe(OH)3
Mass of Fe(OH)3 = (2 * Number of moles of Fe2O3) * molar mass of Fe(OH)3
Finally, we can calculate the mass percentage of iron in the sample:
Mass % of iron = (Mass of Fe / Mass of sample) * 100
Mass % of iron = (Mass of Fe(OH)3 - Mass of Fe2O3 / Mass of sample) * 100
Plug in the known values into the equation and perform the calculations to find the mass percentage of iron in the sample.