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⊙Give me a brief description about moles???
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The mole is theunit of measurement in the International System of Units (SI) for amount of substance. It isdefined as the amount of a chemical substance thatcontains as many elementary entities, e.g., atoms, molecules, ions, electrons,or photons, as there are atoms in 12 grams of carbon-12 (12C), the isotope of carbon with relative atomic mass12 by definition. Thisnumber is expressed by the Avogadro constant, which has a value of 6.022140857(74)×1023 mol−1.The mole is one of the base units of the SI, and has the unit symbol mol.
Think of moles as a "chemist'sdozen". Just as12 eggs is a dozen eggs, 6.02 × 1023 eggs is a mole of eggs. 6.02 × 1023 molecules of oxygen is a mole of oxygen.
The number of grams in a mole is different from substance to substance. If you're like most students,it's this that's confusing you.Picture it this way: a dozen elephants havea different weight than a dozen rabbits- but in each case, you have a dozen animals. Similarly, a mole of oxygengas has a different weight than a mole of water- but in each case, you have 6.02×1023 molecules.
Why use moles? You often want to know how many molecules you have in a sample of a substance. Counting the molecules individually would be completely impractical. Even if you hada way to see the individual molecules, there are just too many, evenin a tiny sample. Moles were defined to solve the problem of counting large numbers of molecules. With moles, you count the number of molecules in the sample by weighing it.big
Think of moles as a "chemist'sdozen". Just as12 eggs is a dozen eggs, 6.02 × 1023 eggs is a mole of eggs. 6.02 × 1023 molecules of oxygen is a mole of oxygen.
The number of grams in a mole is different from substance to substance. If you're like most students,it's this that's confusing you.Picture it this way: a dozen elephants havea different weight than a dozen rabbits- but in each case, you have a dozen animals. Similarly, a mole of oxygengas has a different weight than a mole of water- but in each case, you have 6.02×1023 molecules.
Why use moles? You often want to know how many molecules you have in a sample of a substance. Counting the molecules individually would be completely impractical. Even if you hada way to see the individual molecules, there are just too many, evenin a tiny sample. Moles were defined to solve the problem of counting large numbers of molecules. With moles, you count the number of molecules in the sample by weighing it.big
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