Gas Laws
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This document discusses the properties of gases and the gas laws. It explains that gases have higher energy, lower density, and flow to fill their container compared to liquids and solids. The document also describes how temperature and pressure are measured, noting that pressure is measured using a barometer that reads the height of mercury. It then explains the gas laws of Boyle's Law and Charles' Law, which describe how the volume of a gas changes with pressure and temperature respectively when other variables are held constant.
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- Charles' Law explains that the volume of a gas is proportional to the Kelvin temperature if pressure remains constant.
- The Combined Gas Law combines Boyle's, Charles', and Gay-Lussac's Laws to relate the pressure, volume, temperature, and amount of gas.
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Oxygen: 1.429 g/L or 1.429 g/m3
Chlorine: 3.214 g/L or 3.214 g/m3
Radon: 9.73 g/L or 9.73 g/m3
Principal of gases, gas law flow of
This document discusses gas laws and the behavior of gases. It covers topics like gas pressure, temperature, Boyle's law, Charles' law, the three states of matter, diffusion and effusion of gases, Dalton's law of partial pressures, Henry's law, the ideal gas law, laminar and turbulent gas flow, and the clinical implications of gas behavior. Key points include that gas pressure is caused by molecular collisions, Boyle's law states that pressure and volume are inversely proportional at constant temperature, and Charles' law relates volume and temperature changes at constant pressure.
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Gas Laws
- 2. GASES & THEIR PROPERTIES THE GAS LAWS 2
- 3. WHAT MAKES A GAS DIFFERENT FROM SOLIDS AND LIQUIDS ? • (1) ENERGY STATE - GASES HAVE A HIGHER ENERGY CONTENT • (2) DENSITY - GASES HAVE LOW DENSITY • (3) GASES ARE FLUIDS - THEY FLOW AND TAKE THE SHAPE OF THEIR CONTAINER (SO DO LIQUIDS) • (4) THEY RESPOND NOTABLY TO CHANGES IN TEMPERATURE AND PRESSURE 3
- 4. HOW ARE TEMPERATURE AND PRESSURE MEASURED ? • TEMPERATURE IS MEASURED WITH A THERMOMETER (OF COURSE !) • PRESSURE IS MEASURED WITH A BAROMETER. IT ALLOWS MERCURY TO BE PUSHED UP A VERTICAL GLASS TUBE BY GAS PRESSURE AND THEN THE HEIGHT OF THE MERCURY IN THE TUBE IS READ. PRESSURE IS THEREFORE OFTEN MEASURED IN LENGTH UNITS SUCH AS MILLIMETERS, CENTIMETERS OR INCHES. • YOU HAVE CERTAINLY HEARD TEMPERATURE AND BAROMETER READING DURING WEATHER REPORTS ! 4
- 5. TORRICELLI’S BAROMETER • Hg LEVEL • NORMAL AIR PRESSURE: • 1 ATM • 760 MM OF Hg • 29.92 INCHES • 14.7 PSI • 101.3 KPa 5
- 6. HOW DO GASES RESPOND TO TEMPERATURE & PRESSURE ? • AS THE TEMPERATURE OF A GAS INCREASES, ITS VOLUME INCREASES (DIRECT) • AS THE PRESSURE ON A GAS INCREASES, ITS VOLUME DECREASES (INVERSE) 6
- 7. VARIABLES WHICH EFFECT GAS BEHAVIOR • (1) VOLUME (LITERS) • (2) PRESSURE (ATM OR MM OF Hg) • (3) TEMPERATURE (DEGREES KELVIN) • (4) QUANTITY OF GAS (MOLES) 7
- 8. HOW DO CONFINED GASES AT A CONSTANT TEMPERATURE RESPOND TO PRESSURE CHANGES ? • AS PRESSURE GOES UP, VOLUME GOES DOWN (INVERSE) • BOYLE’S LAW SAYS: • P1 x V1 = P2 x V2 • PRESSURE 1 AND 2 MUST BE IN THE SAME UNITS • VOLUME 1 AND 2 MUST BE IN THE SAME UNITS INVERSE!! 8
- 9. HOW DO CONFINED GASES AT A CONSTANT TEMPERATURE RESPOND TO PRESSURE CHANGES ? (CONT’D) AN INVERSE RELATIONSHIP 9
- 10. HOW DOES TEMPERATURE EFFECT THE VOLUME OF A FIXED QUANTITY OF GAS AT A CONSTANT PRESSURE ? • AS TEMPERATURE GOES UP, VOLUME GOES UP (DIRECT) • CHARLES LAW SAYS: • V1 / T1 = V2 / T2 • VOLUMES 1 AND 2 MUST BE THE SAME UNITS • TEMPERATURES 1 AND 2 MUST BE IN KELVIN KELVIN RULES •CHARLES 10
- 11. Volume T E M P E R A T U R E - 273 0C Absolute Zero No Gas is Ideal real gases liquefy before absolute zero An ideal gas would shrink to zero volume at absolute zero 11
- 12. WHAT IS KELVIN TEMPERATURE ? • KELVIN TEMPERATURE STARTS AT ABSOLUTE ZERO (- 273 DEGREES CELSIUS) • AT ABSOLUTE ZERO, NO HEAT IS PRESENT IN THE SYSTEM (A CONDITION WHICH CAN NEVER BE ACHIEVIED!) • ALMOST ALL SCIENTIFIC CALCULATIONS INVOLVING TEMPERATURE USE THE KELVIN SCALE WHICH IS SOMETIMES CALLED THE ABSOLUTE TEMPERATURE SCALE. • KELVIN = 273 + DEGREES CELSIUS 12
- 13. •13 Click Here