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C:\Fakepath\Notes   Ii Standard Molar Volume And Iii The Ideal Gas Law
C:\Fakepath\Notes   Ii Standard Molar Volume And Iii The Ideal Gas Law
C:\Fakepath\Notes   Ii Standard Molar Volume And Iii The Ideal Gas Law
C:\Fakepath\Notes   Ii Standard Molar Volume And Iii The Ideal Gas Law
C:\Fakepath\Notes   Ii Standard Molar Volume And Iii The Ideal Gas Law
C:\Fakepath\Notes   Ii Standard Molar Volume And Iii The Ideal Gas Law
C:\Fakepath\Notes   Ii Standard Molar Volume And Iii The Ideal Gas Law
C:\Fakepath\Notes   Ii Standard Molar Volume And Iii The Ideal Gas Law
C:\Fakepath\Notes   Ii Standard Molar Volume And Iii The Ideal Gas Law
C:\Fakepath\Notes   Ii Standard Molar Volume And Iii The Ideal Gas Law
C:\Fakepath\Notes   Ii Standard Molar Volume And Iii The Ideal Gas Law
C:\Fakepath\Notes   Ii Standard Molar Volume And Iii The Ideal Gas Law
C:\Fakepath\Notes   Ii Standard Molar Volume And Iii The Ideal Gas Law
C:\Fakepath\Notes   Ii Standard Molar Volume And Iii The Ideal Gas Law
C:\Fakepath\Notes   Ii Standard Molar Volume And Iii The Ideal Gas Law
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C:\Fakepath\Notes Ii Standard Molar Volume And Iii The Ideal Gas Law

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chapter 13 notes sections II and III

chapter 13 notes sections II and III

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  • 1. II. Standard Molar Volume
  • 2. II. Standard Molar Volume(don’t copy)
    Objectives:
    know that the standard molar volume of a gas = 22.4 L at STP.
    know standard temperature = 0 ˚C.
    know that standard pressure = 1 atm.
    calculate the volumes of samples of gases at STP.
  • 3. II. Standard Molar Volume(don’t copy)
    The mole is the SI unit for amount of substance.
    The mole is used to measure amounts of solids.
    The mole is used to measure amounts of substance dissolved in liquids.
    The mole is used to measure amounts of gases.
  • 4. II. Standard Molar Volume(don’t copy)
    1 mole of any substance contains an Avogadro’s number of either atoms, ions, or molecules.
    Example 1: 1 mole He = 6.02 x 1023 He atoms
    Example 2: 1 mole N2 = 6.02 x 1023 N2 molecules
  • 5. II. Standard Molar Volume
    Equal amounts of gases, in moles, occupy the same volume under the same temperature and pressure conditions.
  • 6. II. Standard Molar Volume
    Standard Molar Volume
    1 mole of any gas will occupy 22.4 L of volume at STP.
    STP = standard temperature and pressure conditions.
    T = 0 ˚C
    P = 1 atm
  • 7. II. Standard Molar Volume(don’t copy)
    1 mole of any gas will occupy the same volume at STP:
    1 mole He = 22.4 L He
    1 mole O2 = 22.4 L O2
    1 mole N2 = 22.4 L N2
    1 mole Ar = 22.4 L Ar
    1 mole CO2 = 22.4 L CO2
  • 8. II. Standard Molar Volume
    The standard molar volume equality, 1 mole (any gas) = 22.4 L (any gas), is used as a conversion when calculating quantities of gases in chemical changes.
  • 9. III. The Ideal Gas Law
  • 10. III. The Ideal Gas Law(don’t copy)
    Objectives:
    know the units for each quantity of the ideal gas law equation.
    calculate the pressures, volumes, temperatures, and amounts of gases by the ideal gas law equation.
  • 11. III. The Ideal Gas Law
    The following must be specified to fully describe the state or condition of any sample of gas:
    moles of gas
    temperature of the gas
    pressure of the gas
    volume of the gas
  • 12. III. The Ideal Gas Law
    The Ideal Gas Law equation: PV = nRT
    P = pressure in units of atmospheres (atm)
    V = volume in units of liters (L)
    n = amount of gas in moles (mol)
    R = molar gas constant; R = 0.0281 L atm / mol K
    T = temperature in Kelvin (K)
  • 13. III. The Ideal Gas Law
    Given: PV= nRT
    Derive an equation solving for volume.
  • 14. III. The Ideal Gas Law
    Given: PV= nRT
    Derive an equation solving for pressure.
  • 15. III. The Ideal Gas Law
    Given: PV= nRT
    Derive an equation solving for temperature.

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