Gay-Lussac's Law In Use
We know in Gay-Lussac's law
Volume remains constant
Also you know that if you put a sealed container in a fire it will make the pressure inside the canister increase.
This is Gay-Lussac's law
`P_1` and `T_1` refer to the pressure and temperature before you throw the container in the fire and `P_2` and `T_2` refer to the pressure and temperature after you throw the container in the fire.
Increasing the temperature of the gas increases the pressure in the container.
Increasing the temperature of a gas speeds up the molecules and they have more energy (kinetic energy) to hit and push the side of the container. The molecules will exert more pressure.
The SI unit used to measure pressure is `Pa` (Pascals)
The SI unit used to measure temperature is `K` (Kelvin)
You can use other units for pressure such as pounds per square inch or `mm` of mercury or atm (atmospheres) as long as you use the same units either side of the equation but you must use Kelvin for temperature.
Never forget to convert temperature to Kelvin
Temperature in Kelvin `=` Temperature in degrees Celsius `(\ ^(circ)C)+273`
You must always use temperature measured in Kelvin in any gas law equation.
1. A `30\ \L` sample of nitrogen inside a rigid, metal container at `20^circC` is placed inside an oven whose temperature is `50^circC`. The pressure inside the container at `20^circC` was at 3.00 atm. What is the pressure of the nitrogen after its temperature is increased to `50^circC` ?
`P_2=3.31atm` (to three significant figures)
2. If a gas in a closed container is pressurized from `15` atmospheres to `16` atmospheres and its original temperature was `25^circC`, what would the final temperature of the gas be in degrees Celsius?
But don't forget to convert back from Kelvin to degrees Celsius
3. The temperature of a sample of gas in a steel container at `30\ \kPa` is increased from `-100^circC` to `1.00xx10^3\ \^circC`. What is the final pressure inside the tank.
`P_2=221\ \kPa` to three significant figures