Problem: Consider the following reaction: PbCO3 (s) ⇌ PbO(s) + CO2 (g)Using data in Appendix C in the textbook, calculate the equilibrium pressure of CO2 in the system at 410 oC.

FREE Expert Solution

We’re asked to calculate the equilibrium pressure of CO2 at 410°C using standard thermodynamic data for the given balanced reaction: 


PbCO3 (s) ⇌ PbO(s) + CO2 (g)


Recall that the equilibrium constant is the ratio of the products and reactants. We use Kp when dealing with pressure 


Kp=PproductsPreactants     


Note that solid and liquid compounds are ignored in the equilibrium expression.


Also, recall that ΔG˚rxn and K are related to each other:


ΔG°rxn=-RTlnK


The thermodynamic data ( ΔH˚f and ΔS˚) of each reactant and product can be found in textbooks/online: 


Substance

ΔH˚f (kJ/mol)

S˚ (J/mol • K)

PbCO3 (s) 

699.1 

131.0

PbO(s)

217.3 

68.7

CO2 (g)

393.5 

213.8


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


ΔG°rxn=ΔH°rxn-TΔS°rxn


For this problem we need to do these steps:


Step 1: Calculate ΔH˚rxn.

Step 2: Calculate ΔS˚rxn.

Step 3: Use ΔH˚rxn and ΔS˚rxn to calculate for ΔG˚rxn.

Step 4: Calculate for K (Kp).

Step 5: From Kp, solve for equilibrium partial pressure of CO2


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Problem Details
Consider the following reaction: PbCO3 (s) ⇌ PbO(s) + CO2 (g)


Using data in Appendix C in the textbook, calculate the equilibrium pressure of CO2 in the system at 410 oC.

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