## Chemical formula &

## Mole calculations

###### Chemical formulae & Balancing Equations

###### Introduction to the Mole (& Empirical formula calculations)

###### Stoichiometry - Reacting masses

### Introduction to the Mole

A **mole** is a unit that refers to a specific amount of a chemical substance. One mole (1 mol) is the amount of a substance that contain particles (either atoms, molecules or formulae) of the substance. e.g. in 1 mol of water there are** **water molecules, in 1 mol of helium there are atoms of helium (= **Avogadro’s number**).

**RAM - Relative Atomic Mass (A r)** = the average mass of an atom compared to 1/12th the mass of an atom of carbon-12.

e.g. Chlorine mainly contains 2 isotopes: Cl-35 (75%) & Cl-37 (25%)

The A*r* is an average of the two taking into account relative abundances:(35 x 0.) + 37 x 0.25) = 35.5

**RFM - Relative Formula Mass (M r) **= sum of RAMs of all atoms present in a formula

e.g. M*r* of H2SO4: (1 x 2) + (32 x 1) + (16 x 4) = 98

A*r* & M*r* are the symbols of RAM and RFM respectfully.

The mass of one mole of atoms/molecules is the RAM/RFM expressed in grams.

#### Empirical formula calculations

To work out the empirical formula of a compound, you need to compare the number of moles of each element present in the compound. Therefore, to do this you first take the percentage or (mass in g) of each element present to work out the number of moles of each. Divide the number of moles of each element by the smallest value (number of moles) as this will will result in the simplest whole number ratio.

e.g.:

#### Concentration & Gas volumes

Not as clearly identified in the video is the method to quickly determine the volume of a gas when the number of moles is known. At r.t.p (room temperature & pressure, ~25C and 1 atm): **volume (dm3) = mol x 24**, and at s.t.p (standard temperature and pressure, = 0C and 1 atm):

**volume**

*(*dm*3)*= mol x 22.4© Copyright rmcstudy