#300
There are 0.75 moles of carbon in 0.09 g. Since there is 1 mole of carbon contains 6.022 x 10^23 atoms, there are 4.52 x 10^22 atoms of carbon in 0.09 g.
A single atom of carbon contains 6 protons and 6 neutrons in its nucleus, surrounded by 6 electrons. Therefore, there are 6 atoms in a carbon molecule.
One mole of any element contains 6.02 x 1023 atoms. So 1mole of carbon = 6.02x1023 atoms. 0.8mole of carbon = 0.8 x 6.02x1023 0.8 mole of carbon = 4.816 x 1023
There are 4 chlorine atoms in a molecule of carbon tetrachloride. Calculate the number of moles of carbon tetrachloride in 55 ml using the density provided. Then use Avogadro's number (6.022 x 10^23) to determine the number of chlorine atoms present.
There are 1.9 grams of Carbon. The molar mass of carbon is approximately 12 grams per mole. This means there are ~0.158 moles of carbon. Since 1 mole of carbon contains Avogadro's number of atoms (~6.022 x 10^23 atoms), then 0.158 moles would contain ~9.53 x 10^22 atoms.
0,515 g of carbon is equal to 0,043 moles.
There are 7.16 moles of carbon in 85.9 g of carbon (85.9 g / 12 g/mol). Since there are 6.022 x 10^23 atoms in 1 mole of carbon, the number of carbon atoms in 85.9 g is 4.31 x 10^24 atoms.
1 mole of carbon (or 12 g) has 6 x 1023 atoms. So, 3 moles of carbon (or 36 g) has 18 x 1023 atoms
There are 1 mole of carbon atoms in 12g of carbon. This is because the molar mass of carbon is 12 g/mol, so 12g of carbon is equivalent to 1 mole of carbon atoms.
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.
There are 1.9 grams of Carbon. The molar mass of carbon is approximately 12 grams per mole. This means there are ~0.158 moles of carbon. Since 1 mole of carbon contains Avogadro's number of atoms (~6.022 x 10^23 atoms), then 0.158 moles would contain ~9.53 x 10^22 atoms.
There are 0.75 moles of carbon in 0.09 g. Since there is 1 mole of carbon contains 6.022 x 10^23 atoms, there are 4.52 x 10^22 atoms of carbon in 0.09 g.
There are approximately 2.42 x 10^22 atoms in 1 cm^3 of carbon, assuming a density of 2.26 g/cm^3 and an atomic weight of 12.011 g/mol for carbon.
To find the number of carbon atoms in 12 g of carbon (C), you first need to calculate the number of moles of carbon (C) in 12 g using its molar mass. Then, you can use Avogadro's number (6.022 x 10^23) to determine the number of atoms in that many moles of carbon (C).
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.
To calculate the number of atoms in 63.5 g of carbon monoxide, first determine the number of moles of carbon monoxide using its molar mass (28.01 g/mol). Then, use Avogadro's number (6.022 x 10^23) to convert moles to atoms. A single molecule of carbon monoxide consists of 1 carbon atom and 1 oxygen atom.
There are 4 chlorine atoms in a molecule of carbon tetrachloride. Calculate the number of moles of carbon tetrachloride in 55 ml using the density provided. Then use Avogadro's number (6.022 x 10^23) to determine the number of chlorine atoms present.