Problem: Consider the decomposition of barium carbonate: BaCO3 (s) ⇄ BaO(s) + CO2 (g)Using data from Appendix C in the textbook, calculate the equilibrium pressure of CO2 at 298 K.

FREE Expert Solution

We are considering the decomposition of barium carbonate to calculate the equilibrium pressure of CO2 at 298K.

The equation for the decomposition of BaCO3 is the following:

BaCO3 (s) → BaO (s) + CO2(g)


The equilibrium expression for the reaction is: 

Kp = PCO2Solids are not included in the equilibrium expression


The Standard Gibbs Free Energy of formation of a compound is a change of Gibbs Free energy that accompanies the formation of 1 mole of that substance from its component elements, at their standard states (the most stable form of the element at 25C and 100 kpa). 

(Data from books and the internet)

∆Gof (BaO) = -525.1 kJ/mol

∆Gof (CO2) = -394.4 kJ/mol

∆Goi(BaCO3) = -1134.4 kJ/mol


The formula for the Gibbs Standard Free energy is given as:

Go= nGof -  nGoi

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Problem Details

Consider the decomposition of barium carbonate: BaCO3 (s) ⇄ BaO(s) + CO2 (g)

Using data from Appendix C in the textbook, calculate the equilibrium pressure of CO2 at 298 K.

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