Gas Laws and Pressure Relationship Explained
Explore the relationship between volume, temperature, and pressure in gases through Gay-Lussac's Law, Charles's Law, Boyle's Law, and the Combined Gas Law. Understand how changes in these variables affect gas pressure and volume, with practical examples provided.
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Presentation Transcript
If volume is constant, and temperature increases, what happens to pressure? It increases!
P= P 1 2 Volume is constant T T 1 2 * Remember, Temperature MUST be in Kelvin
P V P V = 1 T 1 2 T 2 1 2
Charless Law Pressure is constant Boyle s Law Temperature is constant V= V = P V P V 1 2 1 1 2 2 T T 1 2 Gay-Lussac s Law Volume is constant Combined Law Contains all variables P V P V P= P = 1 T 1 2 T 2 1 2 T T 1 2 1 2
An aerosol can has a pressure of 103 kPa at 25oC. It is thrown into a fire and its temperature increases to 928oC. What will its pressure be?
P= P 1 2 T T 1 2 P1 = 103 kPa P2 = ? T1 = 25 oC + 273 = 298 K T2 = 928 oC + 273 = 1201 K 103 kPa P P2 = 415 kPa = 2 298 1201 K K
The volume of a gas-filled balloon is 30.0 L at 313 K and 153 kPa. What would the volume be at STP?
P V P V = 1 T 1 2 T 2 1 2 V1 = 30.0L T1 = 313 K P1 = 153 kPa V2 = ? T2 = 273 K P2 = 101.3 kPa ( )( ) ( )( ) V 153 30 0 . 101 3 . kPa 313 L kPa 273 = 2 K K = 14 7 . . 0 371 V 2 V2 = 39.6 L
