Problem: Consider this reaction occurring at 298 K: BaCO3(s) ↔ BaO(s) + CO2(g)a. Show that the reaction is not spontaneous under standard conditions by calculating ΔGrxn b. If BaCO3 is placed in an evacuated flask, what is the partial pressure of CO2 when the reaction reaches equilibrium? 

FREE Expert Solution

A)  Show that the reaction is not spontaneous under standard conditions by calculating ΔGrxn 

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


ΔG°rxn=ΔG°f, prod-ΔG°f, react


90% (415 ratings)
View Complete Written Solution
Problem Details

Consider this reaction occurring at 298 K: 

BaCO3(s) ↔ BaO(s) + CO2(g)

a. Show that the reaction is not spontaneous under standard conditions by calculating ΔGrxn 

b. If BaCO3 is placed in an evacuated flask, what is the partial pressure of CO2 when the reaction reaches equilibrium? 

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Gibbs Free Energy concept. You can view video lessons to learn Gibbs Free Energy. Or if you need more Gibbs Free Energy practice, you can also practice Gibbs Free Energy practice problems.