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
Decane has 10 carbon atoms and 22 hydrogen atoms.
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.
The questions asks how many moles of carbon atoms.Molar mass is defined as the mass of one mole of a substance or in this case 6.022x1023 atoms of carbon. So the molar mass for carbon is 12.0 g/mol. Therefore the number of moles of carbon atoms is just 36/12.0 = 3.0 moles of carbon.How many atoms are in 36 grams of Carbon?[36 (gC) /12.0 (gC/molC)] * 6.02*10+23 (atoms C/molC) = 1.8*10+24 atoms in 36 g Carbon
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.
12 g of carbon will have 6.023 x 1023 atoms of carbon
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
100 atoms of C-12(12g/6.022x10^23) = 1.993x10^-21g
10% of 1505 = 10% * 1505 = 0.1 * 1505 = 150.5
Let us use carbon in this example. Carbon is 12.01 grams per mole. Let us say we have 2.36 X 10^22 atoms of carbon 2.36 X 10^22 atoms carbon (1mole Carbon/6.022 X 10^23)(12.01 grams Carbon/1mol Carbon ) = 0.47 grams Carbon. 6.022 X 10^23 is Avogadro's number and is a constant that is a mole of anything. Just as a dozen eggs is always 12 eggs.
This is because one mole of atoms (6.02 x 10^23 atoms) weighs 12.011g.
This would be C4H10 and the molecular mass is (12x4) +(1x10) = 48 + 10 = 58g/mole.
We take the atomic mass of carbon to be 12.0Amount of carbon in 0.136g pure sample = 0.136/12.0 = 0.0113 The Avogadro's number is 6.02 x 10^23 Number of carbon atoms = 0.0113 x 6.02 x 10^23 = 6.82 x 10^21
72.0 grams Carbon (1 mole C/12.01 grams)(6.022 X 10^23/1 mole C) = 3.61 X 10^24 atoms of carbon
Not that much!! 4350000 atoms Carbon (1 mole C/6.022 X 10^23)(12.01 grams/1 mole C) = 8.675 X 10^-17 grams
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".)
Decane has 10 carbon atoms and 22 hydrogen atoms.
First, get the molar mass of CCl4, which is carbon tetrachloride. According to the periodic table, carbon has an atomic mass of 12 and chlorine is 35.5, but there's 4 of them, so multiply that by 4. 35.5(4)+12=154grams/mole. If you have 2.5 moles, then it's 154x2.5=305 grams.