Summary of Avogadro's Number, the Mole and How to Use the Mole
Avogadro's hypothesis states that equal volumes of gases at the same temperature and pressure have equal numbers of molecules.
Amedeo Avogadro proposed this hypothesis in 1811, leading to the development of relative masses, atomic mass units, and the concept of the mole.
relative masses were determined using Avogadro's hypothesis, with one carbon equaling 12 hydrogen, leading to the development of the atomic mass unit.
The mole is defined as Avogadro's number, which is 6.022 x 10^23, and is the SI unit for the amount of a substance.
molar mass is the mass of one mole of a substance in grams, easily calculated by looking at the atomic mass on the periodic table and changing it to grams.
molar mass calculations for compounds involve adding the molar masses of all elements in the compound.
Examples of molar masses include calcium (40.08 g/mol), hydrogen (1.01 g/mol), oxygen (16 g/mol), and nitrogen (14.01 g/mol).
molar mass calculations for compounds, like nitric acid (HNO3), involve adding the molar masses of all elements in the compound.
The molar mass of HNO3 is 63.02 g/mol, meaning one mole of HNO3 equals 63.02 grams.
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Notable Quotes
— 01:17 — « Avogadros hypothesis states equal volumes of gases at the same temperature and pressure have equal numbers of molecules. »
— 03:37 — « Avogadros number is the number of atoms in 12 grams of carbon-12 and the symbol for Avogadros number is 6.022 times 10 to the 23. »
— 04:41 — « A mole of salt has 6.022 times 10 to the 23 formula units. »
— 04:55 — « 1 mole per 6.022 times 10 to the 23 - its kind of like a little magic. »
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