Avogadros number (approximately). The atomic weight of iron is 55.845. Avogadros number , the number of atoms in a mole of an element, or the number of molecules in a mole of a compound is 6.023 X 1023
Amount of Fe = (2.71x1024)/(6.02x1023) = 4.50mol The atomic mass of Fe is 55.8 Mass of Fe = 4.50 x 55.8 = 251g
Fe, or iron, has a molar mass of 55.845 grams per mole. This means that 0.2 moles is equal to 11.2 grams of iron.
The number of particles (atoms or molecules) in a substance is known as Avogadro's constant and is 6.02 x 1023 particles per mole. The mole is the amount of a substance that contains the same number of particles as the number of atoms in 12 grams of carbon-12. If we consider uranium 238 as the largest isotopic component of natural uranium, and as it consists of atoms not molecules, then 1 kilogram contains 1000/238 moles (1000 grams the mass, 238 the relative atomic mass), ie 4.20 moles. so the number of atoms will be 4.20 x 6.02 x 1023, or 2.529 x 1024 atoms.
Amount of Fe = 55.845/55.845 = 1mol There is 1 mol of Fe in a 55.845g sample. 1 mol of Fe contains 6.02 x 1023 atoms (avogadro constant). Therefore there are 6.02 x 1023 atoms in 55.845g of iron.
One mole of any mono-atomic element contains (by definition) 6.022*10+23 atoms. please calculate from there by multiplying - 11,14.1023 atoms.
To calculate the number of atoms in 13.2 grams of iron, you first need to determine the molar mass of iron, which is approximately 55.85 g/mol. Then, you can use Avogadro's number (6.022 x 10^23 atoms/mol) to convert grams to atoms. Therefore, there are about 4.49 x 10^22 atoms in 13.2 grams of iron.
For this problem, the atomic mass is required. Take the mass in grams and divide it by the atomic mass. Then multiply it by Avogadro's constant, 6.02 × 1023.5.0 grams Fe / (55.9 grams) × (6.02 × 1023 atoms) = 5.38 × 1022 atoms
1 mole Fe = 6.022 x 1023 atoms Fe1 mole Fe = 55.845g Fe (atomic weight in grams)Convert grams Fe to moles Fe.400g Fe x (1mol Fe/55.845g Fe) = 7.16mol FeConvert moles Fe to atoms Fe.7.16mol Fe x (6.022 x 1023atoms Fe/1mol Fe) = 4.31 x 1024 atoms Fe
To find the number of atoms we need to find number of moles of Fe in 312.0 grams. Molar weight of Fe = 56 Number of moles of Fe in 312 grams = 312/56 =5.571 moles. 1 mole of Fe has Avogadro number of atoms. So 5.571 moles of Fe has atoms = 5.571 * Avogadro number. Avogadro number = 6.022 * 10^23 So total atoms = 5.571 * 6.022 * 10^23 = 33.548 * 10^23 * means multiply, ^ means raised to power.
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 determine the number of atoms in 10g of Fe, you first need to calculate the number of moles of Fe using its molar mass (55.85 g/mol). Then, you can use Avogadro's number (6.022 x 10^23 atoms/mol) to find the number of atoms in those moles of Fe. Finally, multiply the number of moles by Avogadro's number to get the total number of atoms in 10g of Fe.
For this you need the atomic mass of Fe. Take the number of grams and divide it by the atomic mass. Multiply by one mole for units to cancel..410 grams Fe / (55.9 grams) = .00733 moles Fe
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 ===================
4,80 moles of Fe contain 28,9062761136.10e23 atoms.
Amount of Fe = (2.71x1024)/(6.02x1023) = 4.50mol The atomic mass of Fe is 55.8 Mass of Fe = 4.50 x 55.8 = 251g
3.0 g Fe x 1 mole Fe/55.8 g = 0.054 moles Fe2.0 g S x 1 mole S/32 g = 0.063 moles STherefore there are more molecules of S than of Fe since one mole of either = 6.02x10^23 atoms.
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