The most recent topic in Chemistry- THE MOLE. The chemical unit is just as ugly as the animal, in my opinion. Although I am still very confused with the subject, I have retained some information about this important unit of measurement. So far, I have learned that the mole is used to express small amounts of matter, such as elements and compounds. This unit provides us with a consistent way to convert between atoms/molecules and grams, and when performing calculations, the mole is a convenient unit.
The mole is defined as “the quantity of a substance that has the same number of particles as are found in 12.000 grams of carbon-12.” This number is equivalent to 6.022×1023, and is called Avogadro’s number. I was surprised by the flexibility of the mole. By this, I mean the way in which it makes any conversion simple. For example, one mole of a compound contains 6.022×10^23 molecules of a compound. The molecular weight of the compound in atomic mass units is the same as the mass in grams of one mole of a compound, making conversions between atoms/molecules, moles, and grams. The formula for determining the number of moles of a sample is below.
weight of sample (g) / molar weight (g/mol)