Chem Lect 2

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RDURU1
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264118
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Chem Lect 2
Updated:
2014-03-02 22:17:16
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MCAT chemistry
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MCAT Chem Lec 2
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  1. 0o C and 1 atm are a part of ___________
    standard temperature and pressure (STP)
  2. This is the distance traveled by a gas molecule between collisions. Usually very very small distances.
    the mean free path
  3. Name the four characteristics of ideal gas that is not shared by real gas
    • 1. Gas molecules have zero volume
    • 2. Gas molecules exert no force other than repulsive force due to collisions
    • 3. Gas molecules make completely elastic collisions.
    • 4. the average kinetic energy of gas molecules is directly proportional to the temperature of the gas
  4. Formula and units for the ideal gas law
    • PV=nRT
    • P= pressure (atm)
    • V= volume (L)
    • n= moles (mol)
    • R=universal gas constant (0.08206 L*atm*K-1*mol-1) or (8.314 J K-1 mol-1)
    • T=temperture (K)
  5. At STP, one mole of any gas will occupy the standard molar volume of ________ liters
    22.4 L
  6. The amount of pressure contributed by any gas in a gaseous mixture is called this type of pressure of that gas.
    To find it U must take the total pressure and multiply it by the mole fraction of the particular gas
    Partial Pressure
  7. Equation for Partial Pressure
    Pa= XaPtotal
  8. Dalton's Law formula of partial pressure
    Ptotal=P1+P2+P3......
  9. How to find the average translational kinetic energy
    KEavg=(3/2)RT
  10. Graham's law shows a relationship that gives the ratio of the rms velocity of tow gases in a homogeneous mixture. what is the formula?
    V1/V2 = rootm2/rootm1
  11. The spreading of gas from high pressure to very low pressure through a "pinhole"
    Effusion
  12. This law gives information about the rates of two types of gaseous spreading : effusion and diffusion.
    Graham's law
  13. formula for effusion and mass of the gases
    (effusion rate1)/(effusion rate2) = (root M2)/(root M1)
  14. This is the spreading of one gas into another gas or into empty space
    diffusion
  15. The higher the temperature the more collision can occur. More collisions equal higher chance of the reaction occurring. This leads us to believe:
    The rate of a reaction increases with temperature
  16. This provides an enlightening method for visualizing chemical reactions. In order for a chemical reaction to occur, the reacting molecules must collide. There are a high frequency of collisions but they do not always result in a reaction.
    The collision model of reactions
  17. The threshold energy that must be reached by the relative kinetic energies of the colliding molecules in order to a reaction to occur
    activation energy
  18. These are species that are products of one reaction and reactants of a later reaction in a reaction chain. Their concentration is often very low because they are often unstable and react as quickly as they are formed
    intermediates

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