13.2 THE GAS LAWS pp. 302-306

Boyle’s law Robert Boyle Seventeenth-century Irish Chemist

Boyles Law States that for a fixed amount of gas at a constant temperature, the volume of a gas increases as its pressure decreases. Likewise the volume of a gas decreases as its pressure increases. Use PTV ruler

13.2 Boyle’s Law When you squeeze a fixed quantity of gas into a smaller volume the pressure goes up. This rule is known as Boyle’s law.

13.2 Boyle’s Law

Solving Problems A kit used to fix flat tires consists of an aerosol can containing compressed air and a patch to seal the hole in the tire. Suppose 5 liters of air at atmospheric pressure (1 atm) is compressed into a 0.5 liter aerosol can. What is the pressure of the compressed air in the can? Assume no change in temperature or mass.

Solving Problems Looking for: Given Relationships: Solution …final pressure in atmospheres (P2) Given …V1 = 5 L , P1= 1 atm, V2 = .5 L Relationships: Boyle’s Law: P1V1 = P2V2 Solution Rearrange equation so P2 = P1V1 / V2 P2 = 1atm x 5.0 L/ 0.5 L = 10 atm.

13.2 Pressure and Temperature The pressure of a gas is affected by temperature changes. If the mass and volume are kept constant, the pressure goes up when the temperature goes up, and down when the temperature goes down.

13.2 Gay-Lussac’s Law

Charles’s Law Charles was a French physicist who studied gases and made the first ascent in a hydrogen filled balloon in 1783.

Charles’s Law States that for a fixed amount of gas at a constant pressure, the volume of the gas increases as its temperature increases. Likewise, the volume of the gas decreases as its temperature decreases. Use PTV ruler

13.2 Charles’ Law A hot-air balloon floats because the air inside is less dense than the air outside.

13.2 Pressure and Temperature Any time we apply gas laws, the temperature must be in Kelvins. Only the Kelvin scale starts from absolute zero, when energy of particles is theoretically zero.

13.2 Charles’ Law According to Charles’ law, the volume of a gas increases with increasing temperature. Volume decreases with decreasing temperature.

Solving Problems A balloon filled with helium has a volume of 0.50m³ at 21 C. Assuming the pressure and mass remain constant, what volume will the balloon occupy at 0 C.?.

Solving Problems Looking for: Given Relationships: Solution …final volume in cubic meters (V2) Given …T1= 21 C , T2 = 0 C, V = 0.50 m³ Relationships: Convert temps using K = C + 273 Charles’ Law: V1/T1 = V2/T2 Solution Rearrange equation so P2 = P1xT2 / T1 V2 = 0.50 m³ . x 273K / 294K = 0.46 m³.