In one cubic centimeter (cc) of a gas at standard conditions (0°C and 1 atm), there are approximately 2.46 x 10^19 argon atoms. This calculation is based on Avogadro's number and the molar volume of gases under standard conditions.
The volume of one atom of argon cannot be calculated because atoms do not have a definite volume due to their small size and quantum nature. Atoms are typically measured in picometers, which is a unit of length rather than volume.
The number is Avogadro's number, 6.0221409 *10^23
One mole of any substance contains Avogadro's number of particles, which is approximately 6.022 x 10^23. Therefore, one million argon atoms would be equivalent to roughly 1.66 x 10^-17 moles of argon atoms.
To find the number of argon atoms in a 40.0-g sample, you first need to calculate the number of moles of argon in the sample using the molar mass of argon (39.95 g/mol). Then, you can use Avogadro's number (6.022x10^23 atoms/mol) to determine the number of atoms in that many moles of argon.
There are approximately 4.61 x 10^26 argon atoms in 7.66 x 10^5 mol of argon. This calculation is based on Avogadro's number, which represents the number of atoms or molecules in one mole of a substance.
The volume of one atom of argon cannot be calculated because atoms do not have a definite volume due to their small size and quantum nature. Atoms are typically measured in picometers, which is a unit of length rather than volume.
The number is Avogadro's number, 6.0221409 *10^23
One mole of any substance contains Avogadro's number of particles, which is approximately 6.022 x 10^23. Therefore, one million argon atoms would be equivalent to roughly 1.66 x 10^-17 moles of argon atoms.
To find the number of argon atoms in a 40.0-g sample, you first need to calculate the number of moles of argon in the sample using the molar mass of argon (39.95 g/mol). Then, you can use Avogadro's number (6.022x10^23 atoms/mol) to determine the number of atoms in that many moles of argon.
There are approximately 4.61 x 10^26 argon atoms in 7.66 x 10^5 mol of argon. This calculation is based on Avogadro's number, which represents the number of atoms or molecules in one mole of a substance.
To find the volume occupied by 1.5 x 10²³ atoms of argon gas at standard temperature and pressure (STP), we first need to calculate the number of moles. Using Avogadro's number (6.022 x 10²³ atoms/mole), we find that 1.5 x 10²³ atoms corresponds to approximately 0.25 moles of argon. At STP, one mole of an ideal gas occupies about 22.4 liters, so 0.25 moles of argon would occupy about 5.6 liters.
There is one atom in argon. Argon is a "noble gas", which means that it occurs independently. This is true for all of the atoms on the final column of the periodic table. http://en.wikipedia.org/wiki/Noble_gas
One mole of argon has a lower atomic mass compared to one mole of neon, as argon has a higher atomic number and thus heavier atoms. This means that there are more argon atoms in one mole compared to neon, but since each argon atom is heavier, the overall mass is less.
Formula: ArF3 But this compound does not exist
Argon (Ar) is an atom not a molecule. An atom is singular whereas a molecule is a group of two or more atoms.
the covalent radius of argon is 97 pico meter
It depends on the identity of the atom. For example, Hydrogen has one proton, but Helium has two.