4.3x10^16 atoms He x 1 mole He/6.02x10^23 atoms x 4 g/mole He = answer (do the math)
6.021023x
Yes. To find out the mass of a mole of atoms of any given element, see the atomic mass given on the periodic table. A mole of carbon atoms has a mass of 12.011 grams. A mole of sulfur atoms has a mass of 32.06 grams.
1 atomgram of a chemical element has 6,02214129(27)×1023 atoms. 1 atomgram=atomic weight of a chemical element exprimed in grams.
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The atomic mass is the mass in grams of one mole of the atoms concerned. Thus, 5 X 132.9 = 664.5 grams.
What is the mass, in grams, of 2 × 1012 atoms of potassium?
To convert grams into atoms, you have to convert them into moles first. Get the molar mass and multiply it by the number of moles to get the atoms.
you take the atomic mass of the atom (or molecule) and you have the mass in grams
Simple: the atomic weight expressed in grams. Example for dysprosium - 162,500 grams.
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
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.
Atomic mass of Ag: 107.9 grams5.00 grams × (6.02 × 1023 atoms) / (107.9 grams) = 2.79 × 1022 atoms Ag
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. AuCl3= 303.5 grams5.00 grams AuCl3 / (303.5 grams) × (6.02 × 1023 atoms) = 9.92 × 1021 atoms
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 × 1023.3.86 grams S / (32.1 grams) × (6.02 × 1023 atoms) = 7.24 × 1022 atoms
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 × 1023.1000 grams C / (12.0 grams) × (6.02 × 1023 atoms) = 5.02 × 1025 atoms
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6.021023x