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 grams
1.505 × 1023 ÷ (6.02 × 1023) × 12.0 = 3.00 grams Carbon
There are 1.9 grams of Carbon. The molar mass of carbon is approximately 12 grams per mole. This means there are ~0.158 moles of carbon. Since 1 mole of carbon contains Avogadro's number of atoms (~6.022 x 10^23 atoms), then 0.158 moles would contain ~9.53 x 10^22 atoms.
divide by the atomic mass and times it by advogadro's number.
Decane has 10 carbon atoms and 22 hydrogen atoms.
The gram atomic mass of carbon is 12.011. Therefore, 1.1 grams constitutes 1.1/12.011 or about 0.0908 moles of carbon. The number of atoms is then 0.0908 X Avogadro's Number or 5.5 X 1022 atoms, to the justified number of significant digits.
1.7 grams * (1mole/ 12.011 grams) * (6.023x 10^23 atoms/ 1 mole) =8.525 * 10^ 22 atoms carbon round to 2 sig. figs
Mass of 1 Helium atom is 4 amu and mass of 1 Carbon atom is 12 amu. So there are 10 helium atoms and 10 carbon atoms
To find the mass of 4350000 atoms of carbon, first calculate the molar mass of carbon (12.01 g/mol). Then, divide the molar mass by Avogadro's number to find the mass of one carbon atom. Finally, multiply the mass of one carbon atom by 4350000 to find the total mass of 4350000 carbon atoms.
The molar mass of carbon-12 (12C) is 12 g/mol. Therefore, one mole of carbon-12 atoms has a mass of 12 grams. Since there are 6.022 x 10^23 atoms of carbon-12, the mass of 6.022 x 10^23 atoms of carbon-12 is also 12 grams, based on Avogadro's number and the molar mass of carbon-12.
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.
100 atoms of C-12(12g/6.022x10^23) = 1.993x10^-21g
There are 6.022 x 10^23 atoms in 1 mole of carbon. The molar mass of carbon is 12 g/mol. Therefore, in 72.0 g of carbon, there are (72.0 g / 12 g/mol) * 6.022 x 10^23 atoms = 3.61 x 10^24 atoms of carbon.
10% of 1505 = 10% * 1505 = 0.1 * 1505 = 150.5
The gram atomic mass of carbon is 12.011 grams. This, by definition, is the mass of Avogadro's number of carbon atoms. Regarding the specified number of atoms as 7.40 X 1017, their mass is accordingly 12.011(7.40 X 1017)/(6.022 X 1023) = 1.48 X 10-5, to the justified number of significant digits (limited to 3 by "7.40".)
The answer is 6,2729.10e+26 carbon atoms.
To convert 1.5 grams of carbon to the number of carbon atoms, you would need to use Avogadro's number, which is the number of atoms in one mole of a substance (6.022 x 10^23 atoms/mol), and the molar mass of carbon (12.01 g/mol). By dividing the given mass of carbon (1.5 g) by the molar mass of carbon, you can convert the grams to moles, and then use Avogadro's number to calculate the number of carbon atoms.
There are 1.9 grams of Carbon. The molar mass of carbon is approximately 12 grams per mole. This means there are ~0.158 moles of carbon. Since 1 mole of carbon contains Avogadro's number of atoms (~6.022 x 10^23 atoms), then 0.158 moles would contain ~9.53 x 10^22 atoms.
divide by the atomic mass and times it by advogadro's number.