# Kinetic Theory, Reaction Rates and Energy Effects

## 8 terms · quantitive relationships between gases, colligative properties, vapour pressure and boiling pressure, and energy effects.

### Boyle's Law (P+V):

Pressure and volume are INVERSELY proportional.
i.e. -as pressure increase, volume decreases.
-as pressure decreases, volume increases.

P1V1 = P2V2

### Charle's Law (V+T):

Volume and temp. are DIRECTLY proportional
i.e if temp increases, volume increases & if temp decreases, volume decreases.

V1/T1 = V2/T2
*Use KELVIN (K) rather than celsius.
^0C + 273 = K
K - 273 = ^0C

### Combined Gas Law (P,V and T):

P1V1/ T1 = P2V2/T2

### Colligative Properties:

Vapour pressure, melting temperature and boiling temperature.
*Applies to liquids and solutions.

### Boiling Pressure:

As a liquid boils, bubbles of gas form inside the liquid, and if there's enough pressure inside the bubble, it will rise to the surface, burst and release vapour.
=> When MAX vapour pressure = Atmosphere Pressure

### Define: Vapour Pressure

Collisions of the vapour from the liquid.

### Adding a Solute (Effects on Boiling Point and Melting Point):

B.Point and M.Point are changed by adding another chemical;
B.point increases, but freezing point decreases.

The more moles of solute (i.e. greater number of particles attracting H2O), the higher the boiling point (due to increased number of ions).

### Energy Effects:

-Energy is measured in kJ, and in an equations, kJ/mol.
-Reactants have a given amount of chemical energy/ enthalpy (Hr).
- Products have a given amount of enthalpy (Hp).

=> The amount of energy GIVEN OUT OR ABSORBED is called the HEAT OF THE REACTION.