Avogadro's number is equal to 6.022 x 1023.
Avogadro's hypothesis states that equal volumes of gases at the same temperature and pressure contain the same number of molecules. This principle helped establish the concept of the mole as a unit for measuring the amount of substance.
PV/NrT, pressure(volume)/amount(constant)(temperature). When your temperature, volume, and pressure are all the same, you get the same number of particles. This is avogadros hypothesis. Let's say that you have to balloons. They have the same temperature, volume, and pressure. If you weigh the gases in the balloon, you will find that there is the same amount of particles. In fact Dalton did this was able to find out the amount of particles (atoms) by the mass of objects.
The atomic number in an element is equal to the number of protons in an element. For example, Hydrogen has an atomic number of 1 and 1 proton.
To have Avogadro's number of particles of CoCl2 6H2O, you would need to measure out 1 mole of the compound. This is equivalent to the molar mass of CoCl2 6H2O in grams, which is approximately 237.93 grams.
A neutral atom has equal numbers of elecrons and protons.
Its avogadros number which is 6.02 X 10^23 g/mol
A mole.
Its avogadros number
No.
I asked this question wrong. It should be Avogadros Number. Sorry!
atoms in 12 g of c-12
It is 6.02 (times) 10 to the power of 23
The unit is "per mole", or mol^-1.
It is the number of fundamental particles - atoms or molecules - of a substance in 1 mole of that substance.
Equal amounts of all gases have the same volume at the same conditions.
Avogadro's Theory states that equal volumes of gases at the same temperature and pressure contain the same number of molecules. This theory led to Avogadro's Law, which states that the volume of a gas is directly proportional to the number of moles of gas present.
Avogadro's principle can be applied to ideal gases at constant temperature and pressure. It states that equal volumes of gases at the same temperature and pressure contain the same number of molecules, allowing for calculations involving quantities of gases.