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Boyle’s Law: P and V

- as one increases,
- the other decreases
- inversely proportional
P1 = P2

V2 V1

Example: Boyle’s Law

Consider a 1.53-L sample of gaseous SO2 at a pressure of 5.6 x 103 Pa. If the pressure is changed to 1.5 x 104 Pa at constant temperature, what will be the new volume of the gas?

Charles’ Law: V and T

- if P is constant, gases expand when heated
- when T increases, gas molecules move faster and collide with the walls more often and with greater force
- to keep the P constant, the V must increase

Charles’ Law: V and T

- Charles’ Law: the V of fixed mass of gas at constant P varies directly with Kelvin T.
- V = kT
- k is a constant for a certain sample of gas that depends on the mass of gas and P
- What kind of graph is V vs. T?

Charles’ Law: V and T

- discovered by French physicist, Jacques Charles in 1787
- first person to fill balloon with hydrogen gas and make solo balloon flight

Example: Charles’ Law & Temp.

A sample of gas at 15°C and 1 atm has a volume of 2.58 L. What volume will this gas occupy at 38°C and 1 atm?

Gay-Lussac’s Law: P and T

- Gay-Lussac’s Law: the P of fixed mass of gas at constant V varies directly with Kelvin T.
- What kind of graph is P vs. T?

Example: Gay-Lussac’s Law

The gas in an aerosol can is at a pressure of 3.00 atm at 25°C. Directions on the can warn the user not to keep the can in a place where temperature exceeds 52°C. What would the gas pressure be in the can at 52°C?

Combined Gas Law

- P1V1 = P2V2
T1 T2

- A cylinder of a gas is kept at a constant volume, as the temperature increases from 24.1 C to 326.4 C. If the initial pressure was 1.10 atm, what is the final pressure in mm Hg?

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