We’re being asked to determine the equilibrium pressure CO2 at 1300 K for the given reaction:
BaCO3 (s) ⇄ BaO(s) + CO2 (g)
The K expression for this reaction is:
*Note: Solids and liquids are not included in the equilibrium constant expression.
Recall that ΔG˚rxn and K are related to each other:
We can use the following equation to solve for ΔG˚rxn:
We’re given the ΔH˚rxn and ΔS˚rxn of the reaction from the appendix:
ΔH˚rxn = -1213.0 kJ/mol
ΔS˚rxn = 112.1 J/mol•K
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 1300 K .
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