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 1300 K .

FREE Expert Solution

We’re being asked to determine the equilibrium pressure COat 1300 K for the given reaction:

BaCO3 (s)  BaO(s) + CO2 (g)


The K expression for this reaction is: 


Kp=productsreactants=PCO2

*Note: Solids and liquids are not included in the equilibrium constant expression.



Recall that ΔG˚rxn and K are related to each other:


ΔG°rxn=-RTlnK


We can use the following equation to solve for ΔG˚rxn:


ΔG°rxn=ΔH°rxn-TΔS°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 


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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 1300 K .

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