A single gram Atomic Mass of iron is usually considered to be the functional equivalent of a mole of metallic iron, because iron atoms do not form well characterized polyatomic entities with themselves. Therefore, 0.26 "mole" of iron contains 0.26 X Avogadro's Number of atoms, or 1.6 X 1023 atoms, to the justified number of significant digits.
4,80 moles of Fe contain 28,9062761136.10e23 atoms.
It depends on the mass of iron. 1 mole Fe = 55.845g = 6.022 x 1023 atoms Fe
the answer is there number of atoms
10 milligrams iron (1 gram/1000 milligrams)(1 mole Fe/55.85 grams)(6.022 X 1023/1 mole Fe) = 1.1 X 1020 atoms of iron ===================
There would be approximately 1.03 x 10^18 iron atoms in 169 milligrams of iron.
4,80 moles of Fe contain 28,9062761136.10e23 atoms.
It depends on the mass of iron. 1 mole Fe = 55.845g = 6.022 x 1023 atoms Fe
To determine the number of iron atoms in a 23.0 g iron block, you would first calculate the number of moles of iron using the molar mass of iron (55.85 g/mol). Then, you would use Avogadro's number (6.022 x 10^23 atoms/mol) to convert moles of iron to atoms.
the answer is there number of atoms
Known/Given:1 mole of Fe = 55.845g Fe (its atomic weight in grams)1 mole of Fe = 6.022 x 1023 atoms Fe (from Avogadro's number)Convert grams Fe to moles Fe.600.0g Fe x 1mol Fe/55.845g Fe = 10.74mol FeConvert moles Fe to atoms Fe.10.74mol Fe x 6.022 x 1023atoms Fe/1mol Fe = 6.468 x 1024atoms Fe
To find the number of moles, you need to divide the number of atoms by Avogadro's number, which is about 6.022 x 10^23 atoms/mol. So, 5.98 x 10^24 atoms of iron would be approximately 9.93 moles of iron.
10 milligrams iron (1 gram/1000 milligrams)(1 mole Fe/55.85 grams)(6.022 X 1023/1 mole Fe) = 1.1 X 1020 atoms of iron ===================
There are approximately 3.25 x 10^24 iron atoms in 354 g of iron. This calculation is done by converting the mass of iron to moles using the molar mass of iron, and then using Avogadro's number to convert moles to atoms.
To determine the number of atoms present in 400g of iron, we need to first calculate the number of moles of iron using its molar mass (55.85 g/mol). Next, we can use Avogadro's number (6.022 x 10^23 atoms/mol) to convert moles to atoms. Finally, multiply the number of moles by Avogadro's number to find the total number of atoms in 400g of iron.
Both a mole of magnesium Mg and a mole of iron Fe contain Avogadro's number of atoms of each element, which is approximately 6.022 x 10^23. This makes them both representative samples of their respective elements in terms of the number of atoms present.
Two atoms in 2 atoms of Fe (this dose not make sense pleas edit)
The density of iron, Fe, at room temperature is 7.874 g/cm3. So 1cm3 of iron has a mass of 7.874g. 1 mole iron = 55.845g Fe = 6.022 x 1023 atoms Fe. 7.874g Fe x 6.022 x 1023 atoms Fe/55.845g Fe = 8.491 x 1022 atoms Fe