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Chemistry » H. Kinetic Molecular Theory

  • H.1. Kinetic Energy

    1. H.1.M. Play Multiplayer 0 wins, 0 losses

    2. H.1.Q. Unit Challenge

    3. H.1.1. Average Kinetic Energy

      1. H.1.1.1. Calculating average kinetic energy
      2. H.1.1.2. Determining changes in average kinetic energy with changes in temperature

    4. H.1.2. Root-mean-square (rms) speed (urms)

      1. H.1.2.1. Calculating urms
      2. H.1.2.2. Determining relative difference in urms based on changes

    5. H.1.3. Graham’s law of diffusion and effusion

      1. H.1.3.1. Calculating molar mass from rates of diffusion
      2. H.1.3.2. Calculating relative speed of diffusion
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  • H.2. Pressure (P = F/A)

    1. H.2.M. Play Multiplayer 0 wins, 0 losses

    2. H.2.Q. Unit Challenge

    3. H.2.1. Relevant Pressure Units (mmHg (torr), pascal, atm)

      1. H.2.1.1. Converting mmHg (torr) to Standard atmospheric pressure (atm)
      2. H.2.1.2. Converting atm to mmHg (torr)
      3. H.2.1.3. Converting atm to pascal (Pa)
      4. H.2.1.4. Converting Pa to atm

    4. H.2.2. Pressure Equation (P = F/A)

      1. H.2.2.1. Calculating pressure given force and area
      2. H.2.2.2. Calculating force given pressure and area
      3. H.2.2.3. Calculating area given pressure and force

    5. H.2.3. Dalton’s Law of Partial Pressures

      1. H.2.3.1. Calculating mole fraction
      2. H.2.3.2. Calculating pressure exerted by an element
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  • H.3. Charles’ Law, Boyle’s Law, Avogadro’s Law, Gay-Lussac’s Law

    1. H.3.M. Play Multiplayer 0 wins, 0 losses

    2. H.3.Q. Unit Challenge

    3. H.3.1. Boyle’s Law (P1V1 = P2V2)

      1. H.3.1.1. Calculating the Pressure using Boyle’s Law
      2. H.3.1.2. Calculating the Volume using Boyle’s Law

    4. H.3.2. Charles’ Law (V1T2 = V2 T1)

      1. H.3.2.1. Calculating the volume using Charles’ Law
      2. H.3.2.2. Calculating the temperature using Charles’ Law

    5. H.3.3. Gay-Lussac’s Law (P1T2 = P2T1)

      1. H.3.3.1. Calculating the pressure using Gay-Lussac’s Law
      2. H.3.3.2. Calculating the temperature using Gay-Lussac’s Law

    6. H.3.4. Avogadro’s Law and Law of Combining Volumes

      1. H.3.4.1. Determining volume of gas given the number of moles of gas
      2. H.3.4.2. Determining number of moles of gas given the volume
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  • H.4. Ideal Gas Law (PV=nRT)

    1. H.4.M. Play Multiplayer 0 wins, 0 losses

    2. H.4.Q. Unit Challenge

    3. H.4.1. Ideal Gas Law

      1. H.4.1.1. Describing relationship between variables in gas laws
      2. H.4.1.2. Deriving the gas constant
      3. H.4.1.3. Deriving the molar volume of a gas at STP
      4. H.4.1.4. Solving problems involving the Ideal Gas Law equation

    4. H.4.2. Combined Gas Laws (P1V1/T1 = P2V2/T2 and P1V1/n1T1 = P2V2/n2T2)

      1. H.4.2.1. Solving problems involving the Combined Gas Law when moles are constant
      2. H.4.2.2. Solving problems involving the combined Gas Law when moles are not constant

    5. H.4.3. Density and Molar Mass

      1. H.4.3.1. Calculating molar mass of a gas given density, temperature, and pressure
      2. H.4.3.2. Calculating density of a gas given molar mass, temperature, and pressure

    6. H.4.4. Gas Stoichiometry

      1. H.4.4.1. Converting from volume at STP to moles
      2. H.4.4.2. Converting from volume, temperature, and pressure to moles
      3. H.4.4.3. Calculating amount of one gas given amount of another gas in a reaction
      4. H.4.4.4. Solving stoichiometry problems with mixed units (volume/pressure of gas and mass)
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