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Five gas laws are commonly used in the General Chemistry courses at Eastfield College. They are Boyle’s Law, Charles’ Law, Gay-Lussac’s Law, The Combined Gas Law, and the Ideal Gas Law. This handout is a guide to help you understand how they are defined and also how they work. Each Law will be defined and you will be given an example for each.
Combined Gas Law: For a given amount of gas the product of the Pressure and Volume is divided by its Kelvin Temperature.
| P 1V 1 | = | P2V2 |
T1 |
T2 |
Layman: This is a combination of Boyle, Charles, and Gay-Lussac’s gas laws
| P1V1 = P2V2 | V1 | = | V1 | P1 | = | P2 | P1V1 | = | P2V2 | ||||
| T1 | T1 | V1 | V2 | T1 |
T2 |
A certain amount of gas has a temperature of 273 K, a pressure of 2 atm and a volume of 500 ml. How many liters of gas would you have if the pressure is 4 atm and the temperature 200 K?
P1 = 2 atm P2 = 4 atm
T1 = 273 K T2 = 200 K
V1 = 500 ml V2 = ?
| P1V1 | = | P2V2 |
T1 |
T2 |
| P1V1T2 | = | V2 |
T1P2 |
V2 = (2 atm)(500ml)(200K) = 183ml = .183L
(4atm)(273K)