A 0.5962g sample of iron ore is dissolved in acid producing Fe3+. Through a series of reactions, the iron precipitates as the Fe(OH)3. The precipitate is heated, forming solid Fe2O3. What is the mass % of iron in the sample if the analysis produced 0.3210g Fe2O3?
atomic mass of iron, Fe = 55.845 g/mol
molar mass of Fe2O3 = 159.69 g/mol
Iron content in sample of Fe2O3
= 0.3210*(55.845/159.69)
= 0.11226 g
Percentage of iron in ore
= 0.11226 g/ 0.5962 g
= 18.83%
Well, well, well, looks like we're doing some chemistry calculations here! Let's dive into it and find the answer while keeping the chemistry fun.
First, we need to determine the moles of Fe2O3 produced. To do that, let's turn to a trusty friend called the molar mass! The molar mass of Fe2O3 is approximately 159.68 g/mol.
So, using the given mass of Fe2O3 (0.3210 g), we can calculate the moles of Fe2O3 with the equation:
moles = mass / molar mass
moles = 0.3210 g / 159.68 g/mol ≈ 0.002011 mol
Now, let's consider the reaction that produced Fe2O3. The balanced equation for the reaction is:
2 Fe(OH)3 → Fe2O3 + 3 H2O
According to the equation, two moles of Fe(OH)3 yield one mole of Fe2O3. So, the moles of Fe(OH)3 will be twice the moles of Fe2O3:
moles of Fe(OH)3 = 2 * 0.002011 mol ≈ 0.004022 mol
Since Fe(OH)3 and Fe are in a 1:1 molar ratio, the moles of Fe in the original sample will be the same as the moles of Fe(OH)3.
Now, let's find the mass of Fe in the sample. We know the moles of Fe is approximately 0.004022 mol. The molar mass of Fe is approximately 55.845 g/mol.
mass of Fe = moles of Fe * molar mass of Fe
mass of Fe = 0.004022 mol * 55.845 g/mol ≈ 0.2246 g
Finally, let's calculate the mass percentage of iron in the sample. We'll use the equation:
mass % = (mass of Fe / mass of the sample) * 100%
mass % = (0.2246 g / 0.5962 g) * 100% ≈ 37.7%
So, the mass percentage of iron in the sample is approximately 37.7%. Ta-da!
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To find the mass percentage of iron in the sample, we need to determine the mass of iron in the Fe2O3 formed.
The molar mass of Fe2O3 is 159.69 g/mol.
First, we need to calculate the number of moles of Fe2O3 formed:
molar mass of Fe2O3 = 159.69 g/mol
mass of Fe2O3 formed = 0.3210 g
moles of Fe2O3 formed = mass of Fe2O3 formed / molar mass of Fe2O3
moles of Fe2O3 formed = 0.3210 g / 159.69 g/mol
Next, we need to calculate the moles of Fe atoms in Fe2O3 since each mole of Fe2O3 contains 2 moles of Fe:
moles of Fe atoms = 2 × moles of Fe2O3 formed
Now, let's find the molar mass of Fe:
molar mass of Fe = 55.845 g/mol
Once we know the moles of Fe atoms, we can determine the mass of Fe:
mass of Fe = moles of Fe atoms × molar mass of Fe
Finally, we can calculate the mass percentage of iron in the sample:
mass % of Fe = (mass of Fe / mass of the sample) × 100
Let's calculate the values:
moles of Fe2O3 formed = 0.3210 g / 159.69 g/mol
moles of Fe atoms = 2 × moles of Fe2O3 formed
mass of Fe = moles of Fe atoms × molar mass of Fe
mass % of Fe = (mass of Fe / mass of the sample) × 100
To find the mass % 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 sample.
First, we need to calculate the molar mass of Fe2O3. Iron (Fe) has a molar mass of 55.845 g/mol, and oxygen (O) has a molar mass of 16.00 g/mol. Since Fe2O3 has two Fe atoms and three O atoms, the molar mass of Fe2O3 is:
Molar mass of Fe2O3 = (2 * molar mass of Fe) + (3 * molar mass of O)
= (2 * 55.845 g/mol) + (3 * 16.00 g/mol)
= 111.69 g/mol + 48.00 g/mol
= 159.69 g/mol
Next, we need to calculate the number of moles of Fe2O3 using its mass. The mass of Fe2O3 is given as 0.3210 g:
Number of moles of Fe2O3 = mass of Fe2O3 / molar mass of Fe2O3
= 0.3210 g / 159.69 g/mol
Now, we can calculate the number of moles of Fe using the balanced equation:
2 Fe2O3 -> 2 Fe + 3 O2
From the balanced equation, we can see that 2 moles of Fe2O3 produce 2 moles of Fe. So the number of moles of Fe is also calculated as:
Number of moles of Fe = Number of moles of Fe2O3
Finally, we can calculate the mass % of iron in the sample by dividing the mass of Fe by the initial mass of the sample and multiplying by 100:
Mass % of iron = (mass of Fe / initial mass of the sample) * 100
Since the initial mass of the sample is given as 0.5962 g, we can substitute the values into the equation and calculate the mass % of iron.