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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 =============
1 mole has 12.01 grams and has 6.022 x 1023 atoms. There are 6 carbon atoms in a glucose molecule so that times six would give you a total of 72.06 grams out of the 180.156 (molar mass for glucose). Carbon makes up about 40 percent of the total glucose mass so the final answer would be it would be around 2.4088 x 1023 atoms of carbon in one gram. Times that by 4 and you'll get 9.6352 x 1023 atoms of carbon in four gram of glucose.
To convert mass to atoms:Find the atomic mass of the element in the substance. You can find atomic masses on the periodic table. Ex. Lithium's atomic mass is 6.9 grams (round if you need to)Then find the mass of the substance in grams. Ex. you have 18.2 grams of a sample of Lithium.The mass of the sample is multiplied by 6.02 * 1023 and divided by the atomic mass.Ex.mass of sample in grams * (6.02 * 1023 atoms) / (atomic mass) = # atoms in grams18.2 grams * (6.02 * 1023 atoms) / (6.9 grams) = 1.59* 1024 atomsThe number 6.02 * 1023 is Avogadro's Constant which is the amount of atoms (or molecules) in one mole.
1 atomgram of a chemical element has 6,02214129(27)×1023 atoms. 1 atomgram=atomic weight of a chemical element exprimed in grams.
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.
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 =============
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
To convert atoms to grams, you need to take the number of atoms, divide it by Avogadro's Constant, then multiply it by the atomic mass.Atoms ÷ (6.02 × 1023) × Atomic mass = Mass in grams1.505 × 1023 ÷ (6.02 × 1023) × 12.0 = 3.00 grams Carbon
16. 2 grams aluminum (1 mole Al/26.98 grams)(6.022 X 1023/1 mole Al) = 3.62 X 1023 atoms of aluminum -------------------------------------------
Atomic mass of Ag: 107.9 grams5.00 grams × (6.02 × 1023 atoms) / (107.9 grams) = 2.79 × 1022 atoms Ag
Atomic mass of carbon: 12.0 grams1.90 grams × (6.02 × 1023 atoms) / (12.0 grams) = 9.53 × 1022 atoms C
3.011 x 1023 atoms of carbon will weigh about 6 grams One mole of carbon atoms weighs 12.011 grams, and there are 6.022 x 1023 atoms in a moles. So you have half as many atoms, so the mass would be half as much or 6.0055 grams to be precise.
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 × 1023.10.6 grams Mg / (24.3 grams) × (6.02 × 1023 atoms) = 2.63 × 1023 atoms
1 mole K atoms = 39.0983g K (atomic weight in grams)1 mole K atoms = 6.022 x 1023 atoms K (Avogadro's number)Convert known atoms to moles.1.72 x 1023 atoms K x (1mol K/6.022 x 1023 atoms K) = 0.286mol KConvert moles to mass in grams.0.286mol K x (39.0983g K/1mol K) = 11.2g K
3.40 X 1022 atoms helium (1 mole He/6.022 X 1023)(4.003 grams/1 mole He) = 0.226 grams ===========