Kinetic Molecular Theory

 

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  1. What are the postulates of the kinetic molecular theory?

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  2. From this information under what conditions would real gases behave similarly to ideal gases? 

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  3. What is the equation for Average Kinetic Energy?
    1. What does kinetic energy describe?
    2. How does temperature effect kinetic energy?

     

     

  4. What is the equation for the root mean square velocity?
    1. How does mass affect the velocity?
    2. How does temperature affect the velocity?

     

     

  5. Consider:


    1. If the plot represents the velocity distribution of 1.0 L of H2 (g) versus 1.0 L of Ar (g) at STP, which plot corresponds to each gas?

    2. If the plots correspond to the velocity distribution of 1.0 L of O2 (g) at 273K and 1273K, which plot corresponds to each temperature?
    3. Under which temperature condition would the O2 (g) behave most ideally?

     

     

  6. What is diffusion?

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  7. What is effusion?

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  8. What is Graham’s Law?

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  9. It took 5.3 minutes for 1.0 L of helium to effuse through a porous barrier.  How long will it take for 1.0L of chlorine gas to effuse under identical conditions?

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  10. Consider the following equations


    How would the following affect number of collisions and length of mean free path?
    1. Increase in mass?
    2. Increase in diameter of particle?
    3. Increase concentration of gas?

     

     

  11. What is the Van Der Waal’s Equation?
    1. What is it correcting for?
    2. What does the variable “a” have to do with?
    3. What does the variable “b” have to do with?

     

     

  12. Would He(g) or H2O(g) have a greater value of “a”?

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  13. Would He(g) or Xe(g) have a smaller value of “b”?

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