
#1
Mar3008, 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 



#2
Apr108, 10:30 AM

P: 2

I'm not sure what the pressure has to do with it..




#3
Apr108, 02:01 PM

Sci Advisor
HW Helper
PF Gold
P: 2,532

The equilibrium pressure of CO_{2} 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.




#4
Apr108, 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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