Since 12 g C is 1.0 mole C there are 6.02*10+23 atoms in (each) mole; that's the definition of a mole
85.9 (g C) = 85.9 (g C) / 12.00 (g/mol C) = 7.158 (mol C)7.158 (mol C)*[6.022*1023 (atoms/mol C)] = 4.31*1024 C-atoms
There are approximately 1.34 x 10^22 carbon atoms in 1.6 g of carbon. This calculation is based on the molar mass of carbon (12 g/mol) and Avogadro's number (6.022 x 10^23 atoms/mol). To find the number of atoms, divide the mass of the sample by the molar mass of carbon, and then multiply by Avogadro's number.
There are 2.92 x 10^22 atoms of 12Carbon in a 3.50 g sample, which is calculated by first determining the molar mass of 12Carbon (12.00 g/mol), then using Avogadro's number to convert from grams to atoms.
the elements are C(carbon), H(Hydrogen), and O(Oxygen). You said G but I can tell you meant C, because G is non existent! The number of atoms is 24(6+12+6=24).
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.
85.9 (g C) = 85.9 (g C) / 12.00 (g/mol C) = 7.158 (mol C)7.158 (mol C)*[6.022*1023 (atoms/mol C)] = 4.31*1024 C-atoms
atoms in 12 g of c-12
atoms in 12 g of c-12
169 g C x 1 mole C/12.011 g x 6.02x10^23 atoms/mole = 8.47x10^24 atoms
There are approximately 1.34 x 10^22 carbon atoms in 1.6 g of carbon. This calculation is based on the molar mass of carbon (12 g/mol) and Avogadro's number (6.022 x 10^23 atoms/mol). To find the number of atoms, divide the mass of the sample by the molar mass of carbon, and then multiply by Avogadro's number.
12 / 24.3 x 6.022x1023 = 2.97x1023 atoms
The number of atoms is 28,099.10e23.
There are 2.92 x 10^22 atoms of 12Carbon in a 3.50 g sample, which is calculated by first determining the molar mass of 12Carbon (12.00 g/mol), then using Avogadro's number to convert from grams to atoms.
the elements are C(carbon), H(Hydrogen), and O(Oxygen). You said G but I can tell you meant C, because G is non existent! The number of atoms is 24(6+12+6=24).
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.
The molar mass of carbon is approximately 12 g/mol. This means that in 5.85 g of graphite, there are 5.85/12 moles of carbon atoms. Therefore, there are 5.85/12 * 6.022 x 10^23 carbon atoms in a 5.85 g piece of graphite.
To find the number of carbon atoms in 0.08 g of carbon, you need to calculate using Avogadro's number and the molar mass of carbon. The molar mass of carbon is approximately 12 g/mol. First, convert grams to moles by dividing 0.08 g by the molar mass of carbon to get approximately 0.0067 moles of carbon. Then, multiply the number of moles by Avogadro's number (6.022 x 10^23) to find that there are approximately 4 x 10^21 atoms of carbon in 0.08 g.