How many grams of copper atoms are needed to supply the same number of atoms as does 235 grams of iron?
225 g Fe = how many mols? That's 225/atomic mass Fe = estimated 4.0
So you want about 4.0 mols Cu atoms and that will be estimated 4.0 x atomic mass Cu = ?
To determine the number of grams of copper atoms needed to supply the same number of atoms as 235 grams of iron, we'll need to use the molar masses of copper and iron to convert grams to moles, and then use Avogadro's number to convert moles to atoms.
1. Find the molar mass of copper (Cu) and iron (Fe):
- The molar mass of copper (Cu) is approximately 63.55 grams/mole.
- The molar mass of iron (Fe) is approximately 55.845 grams/mole.
2. Convert grams of iron (Fe) to moles:
- Divide the given mass of 235 grams of iron by its molar mass (55.845 g/mol):
235 g Fe / 55.845 g/mol = 4.2 moles Fe
3. Use Avogadro's number to convert moles of iron (Fe) to atoms:
- Avogadro's number is approximately 6.022 x 10^23 atoms/mole.
- Multiply the number of moles of iron by Avogadro's number:
4.2 moles Fe * (6.022 x 10^23 atoms/mol) = 2.53 x 10^24 atoms Fe
4. Convert atoms of iron (Fe) to grams of copper (Cu):
- Divide the number of atoms of iron (Fe) by Avogadro's number:
(2.53 x 10^24 atoms Fe) / (6.022 x 10^23 atoms/mol) = 4.2 moles Fe
5. Use the molar mass of copper (Cu) to convert moles to grams:
- Multiply the number of moles of copper by its molar mass:
4.2 moles Cu * 63.55 g/mol = 266 grams Cu
Therefore, you would need approximately 266 grams of copper atoms to supply the same number of atoms as does 235 grams of iron.