Gibbs Free Energy Worksheet

 

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  1. What is Gibb’s free energy? What is its symbol?

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  2. What is the equation for Gibbs Free Energy (ΔG)?

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  3. Why is it such a useful state function?

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  4. What sign must ΔG have to indicate a spontaneous process?

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  5. At what temperatures would the following processes be spontaneous?

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    • +ΔS, -ΔH

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    • -ΔS, -ΔH

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    • +ΔS, +ΔH

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    • -ΔS, +ΔH

     

     

  6. For the following constant pressure process

    2NO2(g)     N2O4(g)

    • ΔH° is -58.03 kJ and ΔS° is -176.6J/K.  What is the value of ΔG° at 298K?

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    • At what temperature is ΔG° = 0 (assume ΔH° and ΔS° are not temp. dependent).

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    • Would ΔG° be negative above or below that temp?


     

  7. For

     

    2O(g)    → O2(g)

      8.  

    • Sign of ΔH?

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    • Sign of ΔS?

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    • Would this process be spontaneous at low or high temperatures?

     

     

  8. ΔGo gives us important information about the _________ position of a reaction.

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  9. The value of ΔG depends on the __________and__________ of reactants and products.  Therefore the value of ΔG __________ as a reaction proceeds.

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  10. At equilibrium the value for ΔG is _____.

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  11. Provide an equation for the following relationships:

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    • ΔG (non-standard) to concentrations/pressures of reactants/products.

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      • When would you use this equation?

       

    • Relates ΔG° to K

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      • When would you use this equation?

       

    • Relates K to T

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      • When would you use this equation?

       

    • Van’t Hoff Equation

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      • When would you use this equation?

  12. Consider

    4NH3(g) + 5O2(g) 4NO (g) + 6H2O(g)

     

    Calculate K at 825°C if ΔH° is -908kJ and ΔS° is 181J/K

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  13. What is free energy of formation?

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  14. What is the symbol for the free energy of formation?

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  15. What is the free energy of formation for an element in its standard state?

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  16. What is the equation used to solve for the free energy of reaction using the free energy of formation?

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