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Pressure
• Pressure is force per unit area– In the English system,
pounds per square inch or psi
– Atmospheric pressure is about 14.7 psi
• Pressure = Force
Area
• 1 atm = 14.7 psi• 1 atm = 760 mmHg
– The mmHg is also called the Torr after Torricelli, inventor of the barometer
• SI unit of measurement, the pascal (Pa)– 1 Pa is the pressure exerted by
a 0.1 mm high film of water on the surface beneath it
– The bar = 105 Pa– 1.013 bar = 1 atm = 760 mmHg
= 14.7 psi = 100 kPa
Gas Pressure Measurement
• The barometer measures pressure in terms of the height of a column on liquid mercury– The atmosphere exerts a
force on a pool of mercury, causing it to rise
– One standard atmosphere of pressure is a column of mercury 760 mm high
– Mercury is used to keep the column a manageable height
Gas Pressure Measurement cont.
• The manometer measures gas pressure by differential– The height of the column
of liquid is proportional to the pressure
– Gas pressure can be more or less than atmospheric pressure
Dalton’s Law of Partial Pressure
• Dalton’s law of partial pressures states that the sum of the partial pressures of gases sum to the total pressure of the gases when combined.
• Ptot = P1 + P2 + P3 + …
Boyles’s Law
• The product of the pressure and volume for a trapped sample of gas = a constant (k)
• PV = k • P1V1 = P2V2 for analysis
of a system before and after
Sample Boyle’s Law problem
• A quantity of gas under a pressure of 106.6 kPa has a volume of 380 dm3. What is the volume of the gas at 103.3 kPa, if the temperature is held constant?
• P1 x V1 = P2 x V2
• (106.6 kPa) x (380 dm3) = (103.3 kPa) x (V2)
• V2 = 400 dm3
Absolute Zero and the Kelvin Scale
• Absolute Zero is the temperature where all motion stops (-273C)
• For gases, the SI unit uses the Kelvin (K) scale.– Kelvins = (273 + C)
Charles’ Law
• The volume of each gas is directly proportional to temperature
• V = bT– B = a constant– V1/T1 = V2/T2
– Temperature is in Kelvins (273 + C)
Charles’ Law Calculation
• At constant pressure, the volume of a gas is increased from 150 dm3 to 300 dm3 by heating it. If the original temperature of the gas was 20 oC, what will its final temperature be (oC)?
• T1 = 20 oC + 273 = 293 K
• T2 = X K
• V1 = 150 dm3
• V2 = 300 dm3
Avogadro’s Law
• Volume is directly proportional to the number of moles of gas
• V = an– V1/n1 = V2/n2
The Combined Gas Law
1 1 2 2
1 2
PV PV
T T
Sample Problem
• A sample of helium gas has a volume of 0.180 L, a pressure of 0.800 atm and a temperature of 29°C. What is the new temperature(°C) of the gas at a volume of 90.0 mL and a pressure of 3.20 atm?