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Kinetic Molecular Theory and Real Gases

Kinetic Molecular Theory and Real Gases. Root Mean Squared, Effusion, Real Gases. Discussion Questions: Kinetic Molecular Theory. Do all your molecules hit the walls of their container with the same force? Justify your answer based on kinetic molecular theory.

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Kinetic Molecular Theory and Real Gases

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  1. Kinetic Molecular Theory and Real Gases

    Root Mean Squared, Effusion, Real Gases
  2. Discussion Questions: Kinetic Molecular Theory Do all your molecules hit the walls of their container with the same force? Justify your answer based on kinetic molecular theory. Iclicker: A) Yes B) No C) not enough information D) I don’t know
  3. Discussion Questions: Kinetic Molecular Theory How does the frequency and force (respectively) of the collisions of the molecules of a gas with the walls of the container change as the temperature of the gas is decreased at constant temperature? Justify based on kinetic model of gases. Iclicker A) Increase, Increase B) Increase, Decrease C) Decrease, Increase D) Decrease, Decrease E) I don’t know.
  4. Discussion Questions Kinetic Molecular Theory If you increase the molecular mass, the rms____________. Justify your answer A) Increases B) Decreases C) stays the same
  5. Concept: Kinetic molecular Theory Effusion: Without doing any calculations, put the following in order of increasing rate of effusion and time of effusion. Molecular masses are in parenthesis. Ne (20.18 g/mol), C3H8 (44.11), He (4.00) and NO2 (46.01)
  6. Calculations: Kinetic Molecular Theory What is the molar mass of a compound that takes 2.7 times as long to effuse through a porous plug as it did for the same amount of XeF2 at the same temperature and pressure? Iclicker: A) 1.2x103 g/mol B) 0.043 g/mol C)457.11 g/molD) 0.016 g/mol E) I don’t know Hint:
  7. Real Gas example (we may not have time for this one the real gas material, depending on the speed of the class we may finish this up on Friday.) Conditions 1 Calculate the pressure exerted by 1.00 mol of C2H6 behaving as an ideal gas and a Van der Waals gas when it is at 1) 273.15 in 22.414L and also 2) at 1000. K in 0.100L. Think about what these answers tell you. Ideal Gas Law Van Der Waals Gas Rearranged for P
  8. Real Gas example (we may not have time for this one the real gas material, depending on the speed of the class we may finish this up on Friday.) Conditions 2 Calculate the pressure exerted by 1.00 mol of C2H6 behaving as an ideal gas and a Van der Waals gas when it is at 1) 273.15 in 22.414L and also 2) at 1000. K in 0.100L. Think about what these answers tell you. Ideal Gas Law Van Der Waals Gas Rearranged for P
  9. Real Gas example (we may not have time for this one the real gas material, depending on the speed of the class we may finish this up on Friday.) Summary Calculate the pressure exerted by 1.00 mol of C2H6 behaving as an ideal gas and a Van der Waals gas when it is at 1) 273.15 in 22.414L and also 2) at 1000. K in 0.100L. Think about what these answers tell you. Condition 2 High Pressure Condition 1 Atmospheric like Ideal Gas Law Van Der Waals Gas Difference 989atm 0.006atm
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