The number of Avogadro is the number of molecules in a mole of substance.The value is 6,022 140 857(74).1o.e23.
You can work this out by dividing the molecular mass of calcium, 40, by Avogadros number, 6.02214129(27)×1023 mol−1 This will give you the answer as the molecular mass of an element is the combined weight of the number of atoms that make up one mole, which is the same as Avogadros number.
One Mole, or Avogadro's Number, is 6.022 X 1023
Two times Avogadro's number (6.022×10 to the 23)
The number of elementary entities in a mole of the substance. The elementary entities depends on the particles making up the substance. For example, argon is made of single atoms, so a mole of argon simply contains Avogadro's number of atoms. Water, on the other hand, is made of molecules, so a mole of water contains Avogadro's number of molecules. Now each water molecule, H2O, contains 3 atoms so a mole of water contains 3xAvogadro's number of atoms. Sodium chloride, NaCl, is made of sodium and chloride ions, in a ratio of 1:1. So a mole of sodium chloride contains Avogadro's number of sodium ions, and Avogadro's number of chloride ions. A mole of sodium chloride therefore contains 2xAvogadro's number of ions in total. The number comes from the number of carbon atoms in 12g of carbon-12.
A cubic meter of gas at standard temperature and pressure will have approximately 2.6 x 1025 molecules. This is based on the Avogadro's Number of molecules, (approximately 6.022 x 1023) taking up a volume of around 23 liters. Alternatively, 32 grams of oxygen has Avogadro's number of molecules.
Who ever came up with the number 3 is cool, but i know you did not come up with number 3.
Amedeo Avogadro did not discover Avogadro's constant. In chemistry, the quantity of a substance that equals one mole was named in honor of Avogadro, but not because he discovered it. Avogadro's number, NA (or Avogadro's constant) is approximately 6.0221415 × 1023.Johann Josef Loschmidt is given credit for the first calculation of the value of Avogadro's number in the year 1865. Of course, the first calculation was fairly crude and many people have improved on this calculation since. Notably, Jean Baptiste Perrin received the Nobel Prize in Physics in 1926 for extensive work establishing the atomic nature of matter and that work involved experimental results that gave a reliable value for Avogadro's number.Avogadro is given credit for Avogadro's Law which asserts that if two gases have the same temperature, volume and pressure, then the elementary entities (molecules) that make up the gasses have masses in the same proportion as the masses of the two quantities of gas. In 1811, Avogadro hypothesized this law. His work and plus the work of many others eventually led to knowing Avagadro's number which allows one to actually know the mass of the molecules in the gas, not just the ratios of masses.The research of Avogadro, Loschmidt, Perrin, Einstein and many others was taking place in the 19th century when the idea that there were such things as atoms and molecules was still developing and these researchers are famous because they made important advancements that eventually led to the modern understanding of atoms and molecules.
it originated from the number google
Silver has 107.87 grams per mole. You have 34.12 grams, so set up a direct proportion where 107.87/1=34.12/x. Solve for x to get 0.316 moles of silver. Now, multiple this by Avogadro's number, which is the number of representative particles of any substance in a mole of that substance. Avogadro's number is 6.02x1023, so that number times 0.316=approx. 1.90x1023 atoms of silver.
(Apex) The relationship between volume and moles (Explanation) Avogadro's law describes the above relationship when pressure and temperature are held constant. When this happens, the volume increases as the moles increase, because they take up more space because there are simply more molecules.
Avogadro came up with what we know as Avodgadro's number. The idea is that at a specific temperature and pressure, equal volumes of two gases will contain the same number of atoms or molecules. This idea was the basis for relative molecular masses, i.e. ways to compare samples that have different atomic masses using the number of atoms or molecules in the sample.