Rust formula is rep by Fe2O3
How many moles of Fe are present in 24.6 g of the compound
Well, well, well! It seems like you've stumbled down the rusty road of chemistry! Don't worry, I'm here to lend you a clownish hand.
To determine the number of moles of Fe (iron) in Fe2O3 (rust), we need to do a little math. First, let's find the molar mass of Fe2O3:
Fe = 55.85 g/mol
O = 16.00 g/mol (there are 3 oxygen atoms in Fe2O3)
Now, let's add up the molar masses:
2(Fe) + 3(O) = 2(55.85 g/mol) + 3(16.00 g/mol) = 111.70 g/mol + 48.00 g/mol = 159.70 g/mol
Now that we have the molar mass of Fe2O3, we can calculate the number of moles of Fe in 24.6 g of the compound. Time for another math party!
Moles = Mass / Molar mass
Moles of Fe = (24.6 g) / (159.70 g/mol)
Let me grab my trusty calculator... Drumroll, please!
The answer is approximately 0.154 moles of Fe.
Hooray! You've got yourself 0.154 moles of Fe rusting away in that 24.6 g compound! Remember, clowns are always ready to lend a hand, even with rusty chemistry problems.
To determine the number of moles of Fe in 24.6 g of Fe2O3, we need to convert the mass of the compound to moles using its molar mass.
The molar mass of Fe2O3 can be calculated by adding the atomic masses of its constituent elements. The atomic mass of Fe is 55.85 g/mol and the atomic mass of O is 16.00 g/mol.
Molar mass of Fe2O3 = (2 * atomic mass of Fe) + (3 * atomic mass of O)
= (2 * 55.85 g/mol) + (3 * 16.00 g/mol)
= 111.70 g/mol + 48.00 g/mol
= 159.70 g/mol
Now, using the molar mass, we can calculate the number of moles of Fe:
Number of moles = Mass / Molar mass
= 24.6 g / 159.70 g/mol
≈ 0.154 mol
Therefore, there are approximately 0.154 moles of Fe present in 24.6 g of Fe2O3.
To determine the number of moles of Fe present in a given compound, we need to use the molar mass of the compound and the molar ratio between Fe and the compound.
First, let's calculate the molar mass of Fe2O3. The atomic mass of Fe is 55.845 g/mol, and the atomic mass of O is 16.00 g/mol. Since there are two Fe atoms in Fe2O3, the molar mass of Fe2O3 can be calculated as follows:
(2 * 55.845 g/mol) + (3 * 16.00 g/mol) = 159.69 g/mol
Now that we have the molar mass of Fe2O3, we can calculate the number of moles:
moles = mass / molar mass
In this case, the mass is 24.6 g. Substituting the values into the formula:
moles = 24.6 g / 159.69 g/mol
Calculating this:
moles = 0.154 moles
Therefore, there are 0.154 moles of Fe present in 24.6 g of the compound.
mols Fe2O3 in 24.6 g Fe2O3 = grams Fe2O3/molar mass Fe2O3 = 24.6/approx 160 = approx 0.15.
Then mols Fe = 0.15 mols Fe2O3 x (2 mols Fe/1 mol Fe2O3) = 0.15 x 2/1 = ?
You need to run through it with better accuracy than my estimates.