How many moles of Na contain 1.45x10 21 atoms of Na? (to find moles, divide atoms by Avogadro's number). The atomic mass of any substance is always equal to 1 mole of that substance The atomic mass added up with itself by 6.02 x 10 23 equals the amount of atoms The atomic mass is the amount of protons plus number of atoms. Learn the basics about Avogadro's Number, as a part of chemical calculations.Avogadro’s Number or the Avogadro Constant is 6.02 X 1023 Mol-1. The Avogadro constant or (the Avogadro number earlier) is the number of elementary units in one mole of any substance. The Avogadro constant is denoted as NA. It has the dimension of the reciprocal amount of substance (mol −1). The approximate value of NA is 6.022 × 10 23 mol −1.

Avogadro's number, also known as Avogadro's constant, is defined as the quantity of atoms in precisely 12 grams of 12C. The designation is a recognition of Amedeo Avogadro, who was the first to state that a gas' volume is proportional to how many atoms it has. This number is given as 6.02214179 x 1023 mol-1.

Amadeo Avogadro lived in the early 19th century and was an Italian savant known for his role in many different scientific disciplines. His most famous statement is known as Avogadro's Law, and is a hypothesis that states, 'Equal volumes of ideal or perfect gasses, at the same temperature and pressure, contain the same number of particles, or molecules.'

This is an intriguing hypothesis, because it says that quite different elements, such as nitrogen and hydrogen, still have the same number of molecules in the same volume of an ideal gas. While in real world settings this is not strictly true, it is statistically quite close, and so the ideal model still has a great deal of value.

## 1 Divided By Avogadro Number

The constant can be expressed as (p1)(V1)/(T1)(n1) = (p2)(V2)/(T2)(n2) = constant; where p is the pressure the gas is at, T is the temperature it is at, V is the volume of gas, and n is the number of molar units.

Part of Avogadro's genius, and while this number was named after him, is that he was able to see this fundamental relationship long before the experimental evidence was available to validate it. His innate understanding of the nature of ideal gasses was astounding, and it wasn't until decades later that experimental evidence finally supported his hypothesis.

In the 1860s, more than 50 years after Avogadro first made his hypothesis, the Austrian high school teacher Josef Loschmidt calculated how many molecules were in a single cubic centimeter of a gas under typical pressure and temperature. He determined this to be approximately 2.6X1019 molecules, a number now known as Loschmidt's Constant, and which has since been expanded to 2.68677725X1025 m-3.

Throughout the early years of the 20th century, a search was undertaken to discover the precise value of Avogadro's number. Molecules were still largely theoretical entities to many scientists until the early part of the 20th century, and so actually determining the value through experiment was not feasible. Once it became feasible, however, it was immediately apparent that the value was important, as it reflected on the fundamental nature of ideal gasses.