Entropy Worksheet

 

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  1. What is entropy?

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  2. Why do things tend toward disorder?

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  3. What state of matter has the highest entropy?

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  4. Determine the sign of ΔS:

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    • CaCO3(s)→CaO(s) + CO2(g)

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    • N2(g) + 3H2(g)→ 2NH3(g)

     

     

  5. What is an arrangement versus a microstate?

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  6. There are multiple equations for entropy.  The first relates it to the number of microstates a system has:

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    • Why is this not a very useful equation?

     

     

  7. What would the change in entropy be for the following system change?

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  8. What are the 3 additional equations for entropy, and in which case do you use each?

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  9. One mole of an ideal gas with a volume of 1.0L and a pressure of 5.0 atm is allowed to expand isothermally into an evacuated bulb to give a total volume of 2.0L.  Calculate w and q. 

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  10. The molar heat capacities for CO2 at 298.0K are

    Cv=28.95 J/molK
    Cp=37.27 J/molK

    The molar entropy of CO2 gas at 298.0 K and 1.000 atm is 213.64 J/mol K

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    • Calculate the energy required to change the temperature of 1.000 mol of CO2 from 298.0K to 350.0K, both at constant volume and at constant pressure.

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    • Calculate the molar entropy of CO2 gas at 350.0K and 1.000 atm.

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    • Calculate the molar entropy of CO2 gas at 350.K and 1.174 atm.

     

     

  11. Calculate the entropy change for a process in which 3.00 mol of liquid water at 0°C is combined with 1.00 mol of water at 100.0°C in a perfectly insulated container.  (Assume the molar heat capacity of water is constant at 75.3J/Kmol)

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  12. When changes in state happen under isobaric conditions.  What relationship is established?

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  13. What are the changes of state for each of the following?

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    • Fusion is when

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    • Vaporization is when

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    • Sublimation is when

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    • Condensation is when

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    • Freezing is when

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    • Deposition is when

     

     

  14. The equation to find the change in entropy during a state change are:

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  15. A sample of ice weighing 1.00 mol, initially at a temperature of -30.0°C, is heated to 140.0°C at a constant pressure of 1.00 atm.  Calculate q, w, ΔH, ΔE, and ΔS. For the process.  The molar heat capacities (Cp) for solid, liquid, and gaseous water are 37.5 J/mol K, 75.3 J/mol K, and  36.4 J/mol K respectively.  The enthalpies of fusion and vaporization are 6.01 kJ/mol and 40.7 kJ/mol, respectively.  Assume ideal gas behavior.

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  16. For mercury, the enthalpy of vaporization is 58.51 kJ/mol and the entropy of vaporization is 92.92J/molK.  What is the normal boiling point?

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  17. What do the following signs/values of ΔSuniv indicate?

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    • + : 
    • – :
    • 0 :  

     

     

  18. What sign of ΔSsurroundings would be assigned for

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    • Exothermic: 

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    • Endothermic:

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