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.
For this you don't need the Atomic Mass. Take the number of moles and multiply it by Avogadro's constant, 6.02 × 1023. Divide by one mole for units to cancel.
4.00 moles C × (6.02 × 1023 atoms) = 2.41 × 1024 atoms C
the atomic mass of carbon: 12.01 # of moles of carbon: 4 # of grams in 4 moles of carbon: ? 12.01 * 4 = ? = 48.04
Two moles of carbon contain 12,044 283 58.1023 atoms.
1 mole = 6.02 × 1023 atoms
4.31 moles × (6.02 × 1023) = 2.6 × 1024 atoms carbon
Amount of carbon
= mass of sample / atomic mass
= 4.50 / 12.0
= 0.375mol
There are 0.375 moles of carbon in a 4.50g pure sample.
1 mole carbon equal 12,01 g.
Moles of carbon dioxide = grams/amu of carbon dioxide. Moles = 19g/44amu Moles of carbon dioxide = .432
0.1 moles There is one carbon and two oxygens 1 x 0.1 = 0.1
3.5 moles CaCO3 (1 mole carbon/1 mole CaCO3) = 3.5 moles
The number of moles of carbon in 11,5 g of ibuprofen is 0,725.
1.2 Moles
Moles of carbon dioxide = grams/amu of carbon dioxide. Moles = 19g/44amu Moles of carbon dioxide = .432
0.1 moles There is one carbon and two oxygens 1 x 0.1 = 0.1
211g of carbon dioxide are equal to 4,794 moles.
19
About one half mole. 6 grams carbon (1 mole C/12.01 grams) = 0.4996 moles of carbon --------------------------------- that is, 0.5 moles carbon ---------------------------------
3.5 moles CaCO3 (1 mole carbon/1 mole CaCO3) = 3.5 moles
10 g of carbon is equivalent to 0,8326 moles.
0,515 g of carbon is equal to 0,043 moles.
The number of moles of carbon in 11,5 g of ibuprofen is 0,725.
6,1x10-3 moles of carbon 36,7350592277.1020 atoms.
There are 24 moles of Carbon (C) in 2 moles of table sugar (sucrose)
30.0 grams carbon (1 mole C/12.01 grams) = 2.50 moles carbon ===============