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II. Standard Molar Volume<br />
II. Standard Molar Volume(don’t copy)<br />Objectives:<br />know that the standard molar volume of a gas = 22.4 L at STP.<...
II. Standard Molar Volume(don’t copy)<br />The mole is the SI unit for amount of substance.<br />The mole is used to measu...
II. Standard Molar Volume(don’t copy)<br />1 mole of any substance contains an Avogadro’s number of either atoms, ions, or...
II. Standard Molar Volume<br />Equal amounts of gases, in moles, occupy the same volume under the same temperature and pre...
II. Standard Molar Volume<br />Standard Molar Volume<br />1 mole of any gas will occupy 22.4 L of volume at STP.<br />STP ...
II. Standard Molar Volume(don’t copy)<br />1 mole of any gas will occupy the same volume at STP:<br />	1 mole He = 22.4 L ...
II. Standard Molar Volume<br />The standard molar volume equality, 1 mole (any gas) = 22.4 L (any gas), is used as a conve...
III. The Ideal Gas Law<br />
III. The Ideal Gas Law(don’t copy)<br />Objectives:<br />know the units for each quantity of the ideal gas law equation.<b...
III. The Ideal Gas Law<br />The following must be specified to fully describe the state or condition of any sample of gas:...
III. The Ideal Gas Law<br />The Ideal Gas Law equation: PV = nRT<br />	P = pressure in units of atmospheres (atm)<br />	V ...
III. The Ideal Gas Law<br />Given: 	PV= nRT<br />Derive an equation solving for volume.<br />
III. The Ideal Gas Law<br />Given: 	PV= nRT<br />Derive an equation solving for pressure.<br />
III. The Ideal Gas Law<br />Given: 	PV= nRT<br />Derive an equation solving for temperature.<br />
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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

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

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

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