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“ The Behavior of Gases ”

“ The Behavior of Gases ”. Original slides by Stephen L. Cotton. Compressibility. Gases can expand to fill its container, unlike solids or liquids The reverse is also true: They are easily compressed , or squeezed into a smaller volume

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“ The Behavior of Gases ”

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  1. “The Behavior of Gases” Original slides by Stephen L. Cotton

  2. Compressibility • Gases can expand to fill its container, unlike solids or liquids • The reverse is also true: • They are easily compressed, or squeezed into a smaller volume • Compressibility is a measure of how much the volume of matter decreases under pressure

  3. Compressibility • This is the idea behind placing “air bags” in automobiles • In an accident, the air compresses more than the steering wheel or dash when you strike it • The impact forces the gas particles closer together, because there is a lot of empty space between them

  4. Compressibility • At room temperature, the distance between particles is about 10x the diameter of the particle • This empty space makes gases good insulators(example: windows, coats) • How does the volume of the particles in a gas compare to the overall volume of the gas?

  5. Variables that describe a Gas • The four variables and their common units: 1. pressure (P) in kilopascals 2. volume (V) in Liters 3. temperature (T) in Kelvin 4. amount (n) in moles • The amount of gas, volume, andtemperature are factors that affect gas pressure.

  6. Amount of Gas • When we inflate a balloon, we are adding gas molecules. • Increasing the number of gas particles increases the number of collisions • thus, the pressure increases • If temperature is constant, then doubling the number of particles doubles the pressure

  7. Pressure and the number of molecules are directly related • More molecules means more collisions, and… • Fewer molecules means fewer collisions. • Gases naturally move from areas of high pressure to low pressure, because there is empty space to move into – a spray can is example.

  8. Common use? • A practical application is Aerosol (spray) cans • gas moves from higher pressure to lower pressure • a propellant forces the product out • whipped cream, hair spray, paint • Is the can really ever “empty”?

  9. Volume of Gas • In a smaller container, the molecules have less room to move. • The particles hit the sides of the container more often. • As volume decreases, pressure increases. (think of a syringe) • Thus, volume and pressure are inversely related to each other

  10. Temperature of Gas • Raising the temperature of a gas increases the pressure, if the volume is held constant. (Temp. and Pres. are directly related) • The molecules hit the walls harder, and more frequently! • Should you throw an aerosol can into a fire? What could happen? • When should your automobile tire pressure be checked?

  11. The Gas Laws are mathematical • The gas laws will describe HOW gases behave. • Gas behavior can be predicted by the theory. • The amount of change can be calculated with mathematical equations. • You need to know both of these: the theory, and the math

  12. Boyle’s Law Gas pressure is inversely proportional to the volume, when temperature is held constant. • Pressure x Volume = a constant • Equation: P1V1 = P2V2 (T = constant)

  13. Charles’s Law • The volume of a fixed mass of gas is directly proportional to the Kelvin temperature, when pressure is held constant. • This extrapolates to zero volume at a temperature of zero Kelvin.

  14. Converting Celsius to Kelvin • Gas law problems involving temperature will always require that the temperature be in Kelvin. (Remember that no degree sign is shown with the kelvin scale.) • Reason? There will never be a zero volume, since we have never reached absolute zero. Kelvin = C + 273 °C = Kelvin - 273 and

  15. Gay-Lussac’s Law • The pressure and Kelvin temperature of a gas are directly proportional, provided that the volume remains constant. • How does a pressure cooker affect the time needed to cook food?

  16. The Combined Gas Law The combined gas law expresses the relationship between pressure, volume and temperature of a fixed amount of gas.

  17. The combined gas law contains all the other gas laws! • If the temperature remains constant... P1 V1 P2 x V2 x = T1 T2 Boyle’s Law

  18. The combined gas law contains all the other gas laws! • If the pressure remains constant... P1 V1 P2 x V2 x = T1 T2 Charles’s Law

  19. The combined gas law contains all the other gas laws! • If the volume remains constant... P1 V1 P2 x V2 x = T1 T2 Gay-Lussac’s Law

  20. The Ideal Gas Law • Equation: PV = nRT • R = 0.0821 (Latm) / (moleK) • The other units must match the value of the constant, in order to cancel out.

  21. The Ideal Gas Law • We now have a new way to count moles (the amount of matter), by measuring T, P, and V. We aren’t restricted to only STP conditions: P V R T n =

  22. Dalton’s Law of Partial Pressures For a mixture of gases in a container, PTotal = P1 + P2 + P3 + . . . • P1 represents the “partial pressure”, or the contribution by that gas. • Dalton’s Law is particularly useful in calculating the pressure of gases collected over water.

  23. If the first three containers are all put into the fourth, we can find the pressure in that container by adding up the pressure in the first 3: 2 atm + 1 atm = 6 atm + 3 atm 4 3 2 1

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