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
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.
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?