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Gibbs Free energy

by jin.cao
Tags: energy, free, gibbs
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jin.cao
#1
Mar30-08, 07:47 AM
P: 13
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
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ron99
#2
Apr1-08, 10:30 AM
P: 2
I'm not sure what the pressure has to do with it..
Mapes
#3
Apr1-08, 02:01 PM
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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.

ron99
#4
Apr1-08, 04:40 PM
P: 2
Gibbs Free energy

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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