Part 1

There are 5 gas laws that we are going to look at: Boyle’s Law (pressure and volume) Charles’ Law (temperature and volume) Gay-Lussac’s Law (pressure and temperature) Combined Gas Law (pressure, temperature, and volume) Ideal Gas Law (pressure, volume, number of moles, and temperature) Numbers 1 – 3 will be on the test this Thursday.

Boyle’s Law (Robert Boyle – 1662) Pressure and volume are inversely proportional As the volume of the container decreases, pressure increases. Formula: P1V1 = P2V2 P: Pressure (Kilopascals, kPa) V: Volume (Litres, L)

Example 1 & 2 A gas has a volume of 15.4 L and a pressure of 232.5 kPa. Find the new volume if the pressure increases to 325 kPa. A gas has an unknown original volume and a pressure of 103 kPa. If the gas undergoes a change to have a volume of 1.3 L and a pressure of 88.5 kPa, what was the original volume of the gas?

You will be given this information on tests Pressure Conversions Use “Cross Multiply and Divide” method 101.325kPa = 1 atm = 760mm Hg You will be given this information on tests Ex 1. Convert 1.23 atm to mmHg Ex 2. Convert 980 mmHg to kPa

Charles’ Law (Jacques Charles - 1780) Temperature and volume are directly proportional. As the temperature of a gas increases, so does the volume of the gas. Formula: V: Volume (Litres - L) T: Temperature (Kelvin – K) To convert Celsius to Kelvin: TK = TC + 273.15 To convert Kelvin to Celsius: TC = TK – 273.15

Examples 1. Neon gas has a volume of 3.0L at 38°C. If the gas is cooled to 29°C, what is the new volume of the Neon gas? 2. You are given 14.0L of argon gas at 101.325 kPa and 39°C. You are going to sell this Argon gas to someone that isn’t very familiar with chemistry, so you offer to sell it to them by the litre. What would you have to do to turn your sample of argon gas into 22.0 L and make more profit?