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Boyle’s Law

Boyle’s Law. Pressure and Volume. Background. The first careful experiments on gasses were performed by Robert Boyle (1600s) Boyle studied the relationship between the pressure of a trapped gas and its volume Boyle’s Observations:

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Boyle’s Law

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  1. Boyle’s Law Pressure and Volume

  2. Background • The first careful experiments on gasses were performed by Robert Boyle (1600s) • Boyle studied the relationship between the pressure of a trapped gas and its volume • Boyle’s Observations: • As the pressure increases, the volume of trapped gas decreases P = Pressure V = Volume k = a constant at a specific temperature for a given amount of gas PV = k

  3. Boyle’s Law • Boyle observed that as pressure increases, volume decreases, and vice versa • The relationship is proportional • If we know the volume of a gas at a given pressure, we can predict the change in volume if the pressure is changed P1V1 = k and P2V2 = k we can say: P1V1 = k = P2V2 Or just: P1V1 = P2V2

  4. Calculating Volume A 1.5-L sample of gaseous CCl2F2 is contained at a pressure of 56 torr. If the pressure is changed to 150 torr at a constant temperature, • Will the volume of the gas increase or decrease? • What will be the new volume of the gas? Step 1: write down the information given: P1 = 56 torr P2 = 150 torr V1 = 1.5 L V2 = ? Step 2: use Boyle’s law to solve: (56)(1.5)= (150)(V2) V2 = 0.56 L V2 = (56)(1.5) 150

  5. Calculating Pressure In a car engine the gaseous fuel-air mixture enters the cylinder and is compressed by a moving piston before it is ignited. In a certain engine the initial cylinder volume is 0.725-L. After the piston moves up, the volume is 0.075-L. The mixture initially has a pressure of 1.00 atm. Calculate the pressure of the compressed mixture. Step 1: write down the information given: P1 = 1.00 atm P2 = ? V1 = 0.725 L V2 = 0.075 L P2 = (1.00)(0.725) 0.075 P2 = 9.7 atm Step 2: use Boyle’s law to solve: (1.00)(0.725)= (P2)(0.075)

  6. Boyle’s Law Practice Problems: Calculate the missing quantity: • V = 249mL at 764 mm Hg; V = ? At 654 mm Hg • V = 1.04 L at 1.21 atm; V = ? At 0.671 atm • V = 525 mL at 1.09 atm; V = 122 mL at ? Atm • V = 2.79 mL at 20.2 atm; V = 209 mL at ? Atm • V = 52.1 L at 755 mm Hg; V = ? At 761 mm Hg • What pressure would be needed to compress 25.1 mL of Hydrogen at 1.01 atm to 25% of its original volume? • If the pressure on a 1.04-L sample of gas is doubled, what will be the new volume of the gas? • A 1.04-L sample of gas at 759 mm Hg pressure is expanded until its volume is 2.24 L, what will the pressure be in the expanded gas sample be?

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