The Gas Laws Boyle’s Law Charles’ Law Gay-Lussac’s Law Combined Gas Law

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Units used to describe gas samples: Volume Liter (L) Milliliter (mL) 1000 mL = 1L Temperature Kelvin ONLY Pressure Atmosphere (atm) Kilopascale (kPa) 1 atm = 101.3 kPa 1 atm = 760 mm Hg 1 atm = 760 torr

Boyle’s Law Boyle’s Law – at constant temperature, the volume of the gas increases as the pressure decreases. The volume of the gas decreases and the pressure increases. V↑ P↓ Volume L P1V1 = P2V2 If you squeeze a gas sample, you make its volume smaller. Pressure (kPa)

↕ Same temperature Moveable piston Now . . . a container where the volume can change (syringe) Moveable piston ↕ Same temperature Volume is 100 mL at 25°C Volume is 50 mL at 25°C In which system is the pressure higher? (Which has the greater number of collisions with the walls and each other?)

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Charles’ Law Charles’ Law – at a constant pressure, the volume of a gas increases as the temperature of the gas increases and the volume decreases when the temperature decreases. V1 V2 T1 T2 = increase AKE increase the speed of the particles the walls of a flexible container expand – think of hot air balloons! Volume L Temperature (K)

A B Steel cylinder (2L) contains 500 molecules of O2 at 400 K In which system do the O2 molecules have the highest average kinetic energy? In which system will the particles collide with the container walls with the greatest force? In which system is the pressure higher? B B B

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Gay-Lussac’s Law Gay-Lussac’s Law – the pressure of a gas is directly proportional to its absolute temperature at a constant volume. P1 P2 T1 T2 Pressure (atm) = Temperature (K)

To remember how these work. . . P T V Think “Public Tele Vision”

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To remember which constants go with which law . . . Boyle’s Law – Temperature is constant Charles’ Law – Pressure is constant Gay-Lussac’s Law – Volume is constant BLT Cheese Pizza Green Veggies

Combined Gas Law P1V1 P2V2 = T1 T2 The equation is found on Table T. Note that all temperatures must be in Kelvin!

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