Molar mass of CArBON 13 = 105.7758 g/mol
The molar mass of 13C = 25.0107 g/mol
13.0 amu
13.003355u
13 grams.
Because the sum of protons, neutrons and electrons masses in sulfur atom is higher than in a carbon atom.
no The mole contain a number of atoms equal to number of atoms in 12 g of carbon-12. The atomic mass unit is equal to one-twelfth the mass of a carbon-12 atom or 1,660538921(73)×10−27 kg.
The atomic mass, in grams, is the mass of one mole of atoms.
The atomic mass is grams/mole So when you have e.g. 12 grams of carbon which has atomic mass = 12, you have one mole. ( Avogadro's number is one mole: 6.02×10²³ )
One mole of 12C has a mass of 12.00000 grams (exactly, by definition).One mole of 13C has a mass of 13.00335 grams.One mole of 14C has a mass of 14.00324 grams.One mole of natural carbon - i.e. a sample with the ration of isotopes equal to that in nature - has a mass of 12.0107 grams.
Because the sum of protons, neutrons and electrons masses in sulfur atom is higher than in a carbon atom.
We use the equation: Mass = Number of moles * Molecular or atomic mass Since the number of moles is 1 ("one mole of carbon-12 atoms") and the atomic mass of carbon-12 atoms is 12, hence the mass would be 12 grams. Note that the unit grams (g) is used here, as it is the SI unit for mass measurement. I hope this is useful! :)
For the same reason that one dozen pencils has a smaller mass than one dozen bricks. Each atom of carbon weighs less than each atom of sulfur, and a mole of each has the same number of atoms, so a mole S will weigh more than a mole C.
no The mole contain a number of atoms equal to number of atoms in 12 g of carbon-12. The atomic mass unit is equal to one-twelfth the mass of a carbon-12 atom or 1,660538921(73)×10−27 kg.
One mole of carbon and one mole of sodium have exactly the same number of atoms. That is what defines the mole, Avogadro's number, 6,022 X 1023 atoms per mole is the definition of mole.
One mole of anything is Avagadro's constant, 6.02 × 1023. One mole of paperclips is 6.02 × 1023 paperclips, one mole of books is 6.02 × 1023 books, and one mole of carbon is 6.02 × 1023 atoms.
This is because one mole of atoms (6.02 x 10^23 atoms) weighs 12.011g.
The atomic mass, in grams, is the mass of one mole of atoms.
Since each mole of carbon dioxide molecules contains two moles of oxygen atoms, as indicated by the formula CO2 for carbon dioxide, half a mole of carbon dioxide will have one mole of oxygen atoms.
If the Atomic Mass of an atom is x, then the mass of 1 mole of the atoms is x gram.
Atomic mass of carbon: 12.0 grams12.01 grams C × (6.02 × 1023 atoms) / (12.0 grams) = 6.03 × 1023 atoms of CarbonNote that one mole of any substance is Avogadro's constant (6.02 × 1023) and that one mole of Carbon is 12.0 grams. So if you have 12.01 grams of carbon (roughly one mole) you should get about Avogadro's constant.
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.