1. DO NOW: 1)What are the four variables used to describe a gas
DO NOW: 1)What are the four variables used to describe a gas? 2) If the volume of a gas decreased, the pressure of the would (increase/decrease)

2. After today you will be able to…
Explain the effect on gas properties using Boyle’s
Calculate an unknown pressure, temperature, or volume by solving algebraically

3. Boyle’s Law: Pressure and Volume
Robert Boyle was the first person to study the pressure-volume relationship of gases.
In 1662 Boyle proposed a law to describe this relationship.

4. “For a given mass of a gas at constant temperature, the volume of a gas varies inversely with pressure.”

5. Boyle’s Law: Pressure and Volume
We can simplify this relationship by the formula: Where, P1, P2 = pressure in any unit (atm, kPa, mmHg), BUT they must match! V1, V2 = volume in any unit (usually, L or mL), BUT they must match!
P1 V1 = P2 V2

6. Boyle’s Law: Example P1 V1=P2 V2 V2 180L =
A gas has a volume of 30.0L at 150 kPa. What is the volume of the gas at atm? P1= V1= P2= V2=
1 atm
150 kPa x
P1 V1=P2 V2 =
1.5 atm
101.3 kPa
30.0L
0.252 atm ?
(1.5 atm)
(30.0L) =
(0.252 atm)
(V2) V2 =
180L

7. Questions? Practice Time!!
Reaction on

8. DOL-Choose at least 2!
Synthetic diamonds can be manufactured at pressures of 6.00 x 104 atm. If we took 2.00 liters of gas at 1.00 atm and compressed it to a pressure of 6.00 x 104 atm, what would the volume of that gas be?
 The highest pressure ever produced in a laboratory setting was about 2.0 x 106 atm. If we have a 1.0 x 10-5 liter sample of a gas at that pressure, then release the pressure until it is equal to atm, what would the new volume of that gas be?
1.00 L of a gas at standard temperature and pressure is compressed to 473 mL. What is the new pressure of the gas?