Avagadro's number says there are 6.02x1023 particles of a pure substance in one mole of that pure substance. (A particle is an atom, molecule, or ion.)
(2.1 mol CO2) (6.02x1023 molecules CO2/1 mol CO2)
= (2.1)( 6.02x1023 molecules CO2) = 1.26 x 1024 molecules CO2
44.0095(14) g/mol x 2.1mols = 92.41995g is wrong I know that
92.4- Nova Net
The answer is 12,64.10e+23
1.26X10^24
The formula is CO2, so there is one atom of carbon and two atoms of oxygen in each molecule.So there are 2.5x10^21 atoms of carbon in that many molecules of CO2.
molar mass NH3 = 17 g/molmolar mass SF6 = 146 g/molmolecules in 0.55g SF6 = 0.55g x 1mol/146g x 6.02x10^23 molecules/mole = 2.27x10^21 moleculesgrams NH3 needed = 2.27x10^21 molecules x 1mol/6.02x10^23 molecules x 17g/mol = 0.064 grams
6.022*10**23 atoms / mol = avagadro's constant 63.546 g / mol = atomic weight of copper 1 atom / 6.022*10**23 atoms/mol * 63.546 g/mol = 1.05523082*10**-22g 1 g / 63.546 g/mol * 6.022*10**23 atoms/mol = 9.476599629*10**21 atoms
to get the answer just take number of moles you have and multiply it by the molecular mass of the compound which is 22g/mol in lithium oxide's case. 23mol x 22g/mol = 506 g of Li2O
moles = mass (g) divided by the molecular weight (g/mol) moles = 100g/12.01
6.022 * 10^21
The mass of the Earth's atmosphere is 5.25x10^21 grams. If we assume the molar mass of air is approximately 29 grams per mole we get:(5.25x10^21) multiplied by Avogadro's constant (6.02x10^23) and then divided by (29 grams/ mol) = 1.09x10^44 molecules of air in the atmosphere.
We know for every 6.022 x 10^23 molecules, we have a mole of a substance, right? So if we have 3920molecules, we can use the above conversion factor to get: 3920 molecules CO2 x (1mol CO2/(6.022x10^23molecules CO2)) = 6.51 x 10^-21 moles CO2. There are three significant figures in this problem, from the 3929 molecules.
(6.022*10^23) * [1.000 (g) / (8 * 32.00 (g/mol)] = 2.352*10^21 molecules
The formula is CO2, so there is one atom of carbon and two atoms of oxygen in each molecule.So there are 2.5x10^21 atoms of carbon in that many molecules of CO2.
0.2550 g AlC3 (1 mol/132 g) =0.001932 mol AlCl3 0.001932 mol AlCl3 (6.022 x 10^23 molecules AlCl3/1 mol AlCl3) = 1.163 x 10^21 1.163x10^21 molecules AlCl3 (3 mol Cl/1 mol AlCl3) =3.490x10^21 Cl ions 3.490x10^21 Cl ions (1 mol/6.022 x 10^23) =5.795x10^-3 moles Cl The formula to solve this problem appears above.
In one (1) molecule CO2 there are 3 atoms ( 1 C-atom and 2 O-atoms), so in 5 molecules CO2 (5CO2) there are 5 x 3 (= 15) atoms. Thus fifteenis the answer to you.
Air is 21% oxygen so 21% of 200 is 42 oxygen molecules.
molar mass NH3 = 17 g/molmolar mass SF6 = 146 g/molmolecules in 0.55g SF6 = 0.55g x 1mol/146g x 6.02x10^23 molecules/mole = 2.27x10^21 moleculesgrams NH3 needed = 2.27x10^21 molecules x 1mol/6.02x10^23 molecules x 17g/mol = 0.064 grams
aproximately 432567000
The gram molecular mass of carbon dioxide is about 44.01 grams. By definition, this value is the number of grams of carbon dioxide that contains Avogadro's Number ("AN") of molecules. Avogadro's Number is about 6.022 X 10^23. Therefore the number of molecules in 1 gram is (1/44.01)(AN) or 2 X 10^21 molecules, to the justified number of significant digits.
0.0156 moles x 6.02x10^23 atoms/mole = 9.39x10^21 atoms