# 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:

Solids 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:

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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.