Send the link below via email or IMCopy
Present to your audienceStart remote presentation
- Invited audience members will follow you as you navigate and present
- People invited to a presentation do not need a Prezi account
- This link expires 10 minutes after you close the presentation
- A maximum of 30 users can follow your presentation
- Learn more about this feature in our knowledge base article
Do you really want to delete this prezi?
Neither you, nor the coeditors you shared it with will be able to recover it again.
Make your likes visible on Facebook?
You can change this under Settings & Account at any time.
Gay-Lussac's Gas Law
Transcript of Gay-Lussac's Gas Law
Joseph Louis Gay-Lussac (1778–1850)
A French chemist and physicist,
Known for his studies on the physical
properties of gases.
A balloon enthusiast as well, in 1804 he
made a hot-air balloon ascent to a height of 20,000 feet in
an early investigation of the Earth's atmosphere
In 1805, discovered that the basic composition of the
atmosphere does not change with decreasing pressure
Definition of Gay-Lussac's Law
Explanation of Real World Applications
1. Soda: If a can of pop becomes heated, the can will explode.
Guy-Lussac’s law explains this, because as the temperature rises, the pressure inside the can increases at the same rate. As the pressure inside pushes outwards on the can, it will eventually explode.
2. Firing a gun:
A gun is fired when gun powder is heated. As the temperature rises, the pressure builds up and expands behind the bullet, until it is fired.
Gay-Lussac's law is represented by a mathematical relationship.
A 20 L cylinder contains 6 atm of gas at 27°C. What would the pressure of the gas be if the gas was heated to 77 °C?
-Gay Lussac’s law states that:
The pressure of an ideal gas is directly proportional to its absolute temperature.
-Temperature goes up, pressure goes up. Temperature goes down, pressure goes down.
-Only applies to ideal
gases with a constant volume.
"P" stands for pressure and "T" stands for temperature
P1 = initial pressure
T1 = initial absolute temperature
P2 = final pressure
T2 = final absolute temperature
Temperature is measured in
Kelvins (K)! NOT °C or °F
. Pressure is measured in
defined as a force of one newton per square meter
Or it can be measured in atmospheres (atm) Atmosphere originally was a unit related to the air pressure at sea level.
Since the cylinder's volume remains unchanged while the gas is heated Gay-Lussac's gas law applies!
P1 = 6 atm
T1 = 27°C
P2 = ? atm
T2 = 77°C
Step 1: Convert from Celsius to Kelvin (K)
27°C + 273 = 300 K
77°C + 273 = 350 K
Step 2: Insert variables into equation and solve for Pf
"Charles and Gay-Lussac's Law." Charles and Gay-Lussac's Law. NASA, 7 Mar. 2011. Web. 15 May 2014.
Helmenstine, Todd. "What Is The Formula For Gay-Lussac’s Law?"About.com Chemistry. N.p., n.d. Web. 16 May 2014.
Helmenstine, Todd. "Review Gay-Lussac's Gas Law with This Sample Chemistry Problem." About.com Chemistry. About.com. Web. 17 May 2014.
Helmenstine, Anne M. "How to Convert Celsius to Kelvin." About.com Chemistry. About.com. Web. 17 May 2014.
"Gases." Gases. NJIT. Web. 20 May 2014. <http://njcmr.njit.edu/distils/lab/chemistry/Gases/gas.html>.
Links for Pictures
Links for Videos
By: Sara Abdulrazzak, Zoé Hunter, Adrienne Joe, Aya Salka
The speed of molecules is dependent on the temperature and pressure of the gas. The higher the pressure or the higher the temperature, the more kinetic energy. When the temperature increases the molecules are excited and begin to move at a faster rate. Because the molecules are moving really quickly, more pressure is being applied to the “walls” of the containers as the molecules collide with it.
As the temperature drops, the amount of kinetic energy drops as well, causing the speed of the molecules to decrease as well. Due to the decrease in the speed of the molecules, the particles are not colliding into the walls as frequently as they did in the higher temperature. This is also known as a decrease in pressure.