Gibbs Free Energy Homework: CaCO3 <-> CaO + CO2

AI Thread Summary
The discussion focuses on calculating the Gibbs Free Energy (ΔG) for the reaction CaCO3 <-> CaO + CO2 at 900K, where the equilibrium pressure of CO2 is 0.0423 atm. The initial calculation provided for ΔG is 5656.3 cal/mol, but there is uncertainty about its accuracy. Participants clarify that the equilibrium pressure of CO2 is indeed relevant to the ΔG calculation, as it relates to the reaction's favorability. The correct approach involves using the equation ΔG = -RTlnK, where K can be derived from the equilibrium pressure. Understanding the relationship between ΔG, K, and the equilibrium pressure is essential for accurate calculations.
jin.cao
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Homework Statement


CaCO3 <-> CaO + CO2
At 900K, equilibrium pressure of CO2 is 0.0423 atm. Calculate Gibbs Free energy of Reaction and K.

Homework Equations


delta G = -RTlnK

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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I'm not sure what the pressure has to do with it..
 
The equilibrium pressure of CO2 is directly connected to the \Delta G of the reaction. If the forward reaction is strongly favored, the pressure is higher, and vice versa.
 
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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