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Chemistry Study Guide #6

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Chemistry Study Guide #6

1/5/04

- Avogrado- 1776-1856. Italian. Laws of Definite and Multiple Proportions.

- Avogrado’s Principle- equal volumes of all gases at the same temperature and pressure contain same number of molecules

- Avogrado didn’t discover the mole, but his principles were used

A mole is simply a number

ç (pi) = 3.14159

Dozen = 12

Gross = 144

Ream = 500

Mole = 6.0221367 x 10²³

- “1 mole is the amount of substance which contains as many particles as there are atoms in exactly 12 g of carbon-12.”

- Atomic weight is measured in grams per mole (g/mol)

o Ex. Carbon weighs 12.0107, so 12.0107 g. carbon have 1 mol of particles

- For compounds, add elements together

o Ex. CuSO4—4 x 16.00 + 1 x 32.07 + 1 x 63.55 = 159.62 g/mol. There will be 1 mol of particles in 159.62 grams of CuSO4

The molar (or gram- formula) mass for any substance is equal to the number of grams of the substance in one mole.

8-1

Relative atomic mass- accounts for isotopes- not exact

Molar mass- numerically equal to atomic mass. Unit is g/mol

Single- atom mass (in grams)- molar mass/ mol