1. Pressure and Temperature William Thomson “Lord Kelvin”

2. Measuring Pressure The first device for measuring atmospheric pressure was developed by Evangelista Torricelli during the 17 th century. The device was called a “barometer” Baro = weight Meter = measure

3. An Early Barometer The normal pressure due to the atmosphere at sea level can support a column of mercury that is 760 mm high.

4. Pressure  Is caused by the collisions of molecules with the walls of a container  is equal to force/unit area

5. Standard Pressure 1 standard atmosphere (atm)  1 standard atmosphere (atm)  101.3 kPa (kilopascals)  14.7 lbs/in2  760 mm Hg (millimeters of mercury)  760 torr

6. Pressure UnitSymbolDefinition/Relationship PascalPaSI pressure unit 1 Pa = 1 newton/meter 2 Millimeter of mercury mm HgPressure that supports a 1 mm column of mercury in a barometer AtmosphereatmAverage atmospheric pressure at sea level and 0  C Torrtorr1 torr = 1 mm Hg Pressure is the force created by the collisions of molecules with the walls of a container

7. The Kelvin Scale

8. Standard Temperature Standard Temperature equals:  273 Kelvin (273 K)  0  C

9. Converting Celsius to Kelvin Gas law problems involving temperature require that the temperature be in KELVINS! Kelvins =  C + 273 °C = Kelvins - 273

10. Standard Temperature and Pressure “STP” Either of these:  273 Kelvin (273 K)  0  C Either of these:  273 Kelvin (273 K)  0  C And any one of these: 1 atm  1 atm  101.3 kPa  14.7 lbs/in 2 (psi)  760 mm Hg  760 torr And any one of these: 1 atm  1 atm  101.3 kPa  14.7 lbs/in 2 (psi)  760 mm Hg  760 torr

11. Standard Molar Volume One mole of a gas at STP has a volume of 22.4 Liters

12. Mole Relationships Mole Atoms or molecules Atoms or molecules Liters Grams 6.02 x 10 23 AtomicMassAtomicMass 22. 4 L 22.4 L