**Boyle's Law**

Boyle's Law states the volume of a definite quantity of dry gas is inversely proportional to the pressure, provided the temperature remains constant.

Mathematically Boyle's law can be expressed as P_{1}V_{1} = P_{2}V_{2}

- V
_{1}is the original volume - V
_{2}is the new volume - P
_{1}is original pressure - P
_{2}is the new pressure

Suppose you have a gas with 45.0 ml of volume and has a pressure of 760.mm. If the pressure is increased to 800mm and the temperature remains constant then according to Boyle's Law the new volume is 42.8 ml.

(760mm)(45.0ml) = (800mm)(V_{2})

V_{2}=42.8ml

**Charle's Law**

Charle's Law can be stated as the volume occupied by any sample of gas at a constant pressure is directly proportional to the absolute temperature.

V / T =constant

- V is the volume
- T is the absolute temperature (measured in Kelvin)

Charles's Law can be rearranged into two other useful equations.

V_{1} / T_{1} = V_{2} / T_{2}

- V
_{1}is the initial volume - T
_{1}is the initial temperature - V
_{2}is the final volume - T
_{2}is the final temperature

V_{2} = V_{1} (T_{2} / T_{1})

- V
_{2}is the final volume - T
_{2}is the final temperature - V
_{1}is the initial volume - T
_{1}is the initial temperature

*Important*: Charles's Law only works when the pressure is constant.

*Note*: Charles's Law is fairly accurate but gases tend to deviate from it at very high and low pressures.

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