mols Fe = 3.01E22/6.022E23 = ?
Then grams = mols x atomic mass.
Then grams = mols x atomic mass.
The molar mass of an element is the mass of one mole of that element. To calculate the molar mass of Fe^2+, we consider the atomic mass of iron (Fe).
The atomic mass of iron (Fe) is 55.845 grams/mol.
Since Fe^2+ has lost two electrons, its molar mass will be half of the atomic mass of iron (Fe).
Molar mass of Fe^2+ = (55.845 g/mol)/2 = 27.9225 g/mol.
Now, we can calculate the mass of 3.01 x 10^22 Fe^2+ ions:
Mass = (Number of ions) x (Molar mass)
= (3.01 x 10^22 ions) x (27.9225 g/mol)
= 8.4 x 10^23 g.
Therefore, the mass of 3.01 x 10^22 iron (II) ions (Fe^2+) is approximately 8.4 x 10^23 grams.
1. Find the atomic mass of iron (Fe) from the periodic table, which is approximately 55.85 grams per mole (g/mol).
2. Calculate the molar mass of Fe^2+ by adding the mass of two electrons (since it has a +2 charge) to the atomic mass of Fe.
- The mass of an electron is approximately 9.11 x 10^-28 grams.
- So, the molar mass of Fe^2+ would be 55.85 g/mol + 9.11 x 10^-28 grams + 9.11 x 10^-28 grams.
3. Now that we have the molar mass of Fe^2+, we can calculate the mass of 3.01 x 10^22 Fe^2+ ions using the following steps:
- Multiply the number of ions (3.01 x 10^22) by the molar mass of Fe^2+.
- The units will be (3.01 x 10^22 ions) * (molar mass of Fe^2+ / 1 ion). The "ions" unit cancels out, leaving you with grams as the unit.
Solving this equation will give you the mass of 3.01 x 10^22 Fe^2+ ions.