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A gram atom of an element is the mass in grams of Avogadro's Number, about 6.022 X 1023, of atoms of the element.
A gram atom of an element is the mass in grams of Avogadro's Number, about 6.022 X 1023, of atoms of the element.
1 atomgram of a chemical element has 6,02214129(27)×1023 atoms. 1 atomgram=atomic weight of a chemical element exprimed in grams.
4.21 × 1023 atoms ÷ (6.02 × 1023 atoms) × 30.97 grams = 21.66 grams P
8.90 X 1023 lead atoms (1 mole Pb/6.022 X 1023)(207.2 grams/1 mole Pb) = 306 grams of lead =============
The molar mass of any element is its atomic weight (amu) in grams, and 1 mol of any element is 6.022 x 1023 atoms. Therefore, the mass in grams of 6.022 x 1023 atoms of N = 14.01g N.
A gram atom of an element is the mass in grams of Avogadro's Number, about 6.022 X 1023, of atoms of the element.
A gram atom of an element is the mass in grams of Avogadro's Number, about 6.022 X 1023, of atoms of the element.
1 atomgram of a chemical element has 6,02214129(27)×1023 atoms. 1 atomgram=atomic weight of a chemical element exprimed in grams.
14 grams of nitrogen have 6.023 x 1023 atoms So 2.2 grams will have (6.023 x 1023 x 2.2)/14 = 29.15 x 1023 atoms
Molar mass of an element is the atomic weight on the periodic table in grams. 1 mole of atoms of an element is 6.022 x 1023 atoms. To find the mass of one atom of an element, divide the element's molar mass by 6.022 x 1023 atoms.Example:Sodium, Na, has a molar mass of 22.989770g/mol (atomic weight in grams)1 mole Na atoms = 6.022 x 1023 atomsSolution:22.989770g/mol x 1mol/6.022 x 1023 atoms = 3.818 x 10-23g/atom
16.3 grams ÷ 32.1 grams × (6.02 × 1023) = 3.06 × 1023 atoms S
6.02 x 1023 atoms of an element is one mole of that element. The mole, based on Avagadro's number, is defined as the number of Carbon atoms that would have a mass of 12 grams. This is a scaling factor related to atomic mass. Krypton has an atomic mass of 83.8, so if a mole of an unknown element is 83.8 grams, then that element is Krypton.
You can use atomic weight to calculate the number of atoms in a given sample of an element. # g of sample element x (6.02 x 1023 / atomic weight in grams) = # of atoms
It depends on the substance. If you have for example, 12 grams of Carbon-12. Then you have 1 mole of carbon 12 which is 6.02 * 1023 molecules of the element, which is equal to 12 grams. One mole of a compound or element is equal to that element's atomic mass in grams.
4.21 × 1023 atoms ÷ (6.02 × 1023 atoms) × 30.97 grams = 21.66 grams P
Atomic mass: 207.2 grams.455 moles × (6.02 × 1023) = 2.74 × 1023 atoms of lead