Gibbs Free energy

  1. 1. The problem statement, all variables and given/known data
    CaCO3 <-> CaO + CO2
    At 900K, equilibrium pressure of CO2 is 0.0423 atm. Calculate Gibbs Free energy of Reaction and K.


    2. Relevant equations
    delta G = -RTlnK


    3. The attempt at a solution

    delta G = 5656.3 cal/mol
    K = 0.0423

    I have a feeling that this is incorrect
    Could someone confirm/clarify for me

    Thanks
     
  2. jcsd
  3. I'm not sure what the pressure has to do with it..
     
  4. Mapes

    Mapes 2,532
    Science Advisor
    Homework Helper
    Gold Member

    The equilibrium pressure of CO2 is directly connected to the [itex]\Delta G[/itex] of the reaction. If the forward reaction is strongly favored, the pressure is higher, and vice versa.
     
  5. ok, but does the pressure have anything to do with the calculations?

    delta G = [sum(delta G formation, products) - sum(delta G formation, reactants)]

    which can all be calculated from table values.

    Then the equation:

    delta G = -RTlnK can be used to find K

    is this correct?
     
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