BOYLE’S LAW CHARLE’S LAW GAY-LUSSAC’S LAW AVOGADRO’S LAW COMBINED GAS LAW BEHAVIOR OF GASES GAS LAWS

DIRECTIONS FOR THESE NOTES USING THE “FACTORS AFFECTING GASES INVESTIGATION” AND “BEHAVIOR OF GASES” HANDOUT TO FOLLOW ALONG HAVE YOUR NOTEBOOK/PAPER IN HAND FOR PARTS NOT FOUND IN THE HANDOUT

BEHAVIOR OF GASES We’ve discussed some characteristic of assumptions and characteristics of gases according to the Kinetic Molecular Theory: i. Gases move randomly and rapidly in straight line paths. ii. Collisions between particles and the walls of a container are elastic (they don’t stick) because there are no significant forces of attraction or repulsion. iii. Gases have no significant volume and can take up the shape and volume of a container

BEHAVIOR OF GASES Kinetic Molecular Theory can also explain other properties and variables of gases and their relationship to each other. These variables are: 1. AMOUNT OF A GAS (MOLES) 2. PRESSURE 3. VOLUME 4. TEMPERATURE

BOYLE’S LAWBOYLE’S LAW: PRESSURE & VOLUME As the pressure of a gas increases, the volume decreases (constant temperature) P 1 V 1 = P 2 V 2

BOYLE’S LAW: PRESSURE & VOLUME As the pressure of a gas increases, the volume decreases (constant temperature) A balloon at an initial volume of 25 mL and 1 atm is expanded to 100 mL, what is the final pressure? P 1 = 1 atm V 1 = 25 mL (1 atm) x (25 mL) = ( ??? atm) x (100 mL) V 2 = 100 mL (1atm)x(25mL) / (100mL) = 0.25 atm P 2 = ???? P 1 V 1 = P 2 V 2

BOYLE’S LAW: PRESSURE & VOLUME As the pressure of a gas increases, the volume decreases (constant temperature) A balloon at an initial volume of 25 mL and 1 atm is expanded to 100 mL, what is the final pressure? P 1 = 1 atm V 1 = 25 mL (1 atm) x (25 mL) = ( ??? atm) x (100 mL) V 2 = 100 mL (1atm)x(25mL) / (100mL) = 0.25 atm P 2 = ???? P 1 V 1 = P 2 V 2

BOYLE’S LAW: PRESSURE & VOLUME As the pressure of a gas increases, the volume decreases (constant temperature) A balloon at an initial volume of 25 mL and 1 atm is expanded to 100 mL, what is the final pressure? P 1 = 1 atm V 1 = 25 mL (1 atm) x (25 mL) = ( ??? atm) x (100 mL) V 2 = 100 mL (1atm)x(25mL) / (100mL) = 0.25 atm P 2 = ???? P 1 V 1 = P 2 V 2

BOYLE’S LAW: PRESSURE & VOLUME As the pressure of a gas increases, the volume decreases (constant temperature) A balloon at an initial volume of 25 mL and 1 atm is expanded to 100 mL, what is the final pressure? P 1 = 1 atm V 1 = 25 mL (1 atm) x (25 mL) = ( ??? atm) x (100 mL) V 2 = 100 mL (1atm)x(25mL) / (100mL) = 0.25 atm P 2 = ???? P 1 V 1 = P 2 V 2

CHARLE’S LAWCHARLE’S LAW: TEMPERATURE & VOLUME As the temperature of an enclosed gas increases, the volume increases (Constant pressure) NOTE: Absolute Zero is 0 K (  273°C) where the motion of particles ceases (stops)

CHARLE’S LAW: TEMPERATURE & VOLUME A balloon at 300 K and 100 mL is heated to 400 K. What is the final volume? SET-UP?

GAY-LUSSAC’S LAWGAY-LUSSAC’S LAW: PRESSURE & TEMPERATURE As the temperature of an enclosed gas increases, the pressure increases (Constant Volume)

GAY-LUSSAC’S LAW: PRESSURE & TEMPERATURE A balloon at 1 atm and 298 K is compressed to 2 atm. What is the final temperature? Set-up?

AVOGADRO’S LAW: VOLUME & MOLES Equal volumes of gases at the same temperature and pressure have equal number of moles (n).

COMBINED GAS LAW The combined gas law describes the relationship among the pressure, temperature and volume of an enclosed gas. It allows you to do calculations for situations in which the number of moles of gas is constant.

COMBINED GAS LAW A balloon is at initial conditions of 373 K, 1 atm and 100 L is expanded to 200 L and 0.5 atm. What is the final temperature of the balloon?