Gibbs Free Energy Homework: CaCO3 <-> CaO + CO2

In summary, at a temperature of 900K, the equilibrium pressure of CO2 is 0.0423 atm for the reaction CaCO3 <-> CaO + CO2. To calculate the Gibbs Free energy of the reaction, the equation delta G = -RTlnK can be used, where delta G can be found by subtracting the sum of the formation energies of the products from the sum of the formation energies of the reactants. Once delta G is calculated, K can be found by using the equation delta G = -RTlnK. However, the pressure does not directly affect the calculations.
  • #1
jin.cao
13
0

Homework Statement


CaCO3 <-> CaO + CO2
At 900K, equilibrium pressure of CO2 is 0.0423 atm. Calculate Gibbs Free energy of Reaction and K.

Homework Equations


delta G = -RTlnK

The Attempt at a Solution



delta G = 5656.3 cal/mol
K = 0.0423

I have a feeling that this is incorrect
Could someone confirm/clarify for me

Thanks
 
Physics news on Phys.org
  • #2
I'm not sure what the pressure has to do with it..
 
  • #3
The equilibrium pressure of CO2 is directly connected to the [itex]\Delta G[/itex] of the reaction. If the forward reaction is strongly favored, the pressure is higher, and vice versa.
 
  • #4
ok, but does the pressure have anything to do with the calculations?

delta G = [sum(delta G formation, products) - sum(delta G formation, reactants)]

which can all be calculated from table values.

Then the equation:

delta G = -RTlnK can be used to find K

is this correct?
 

1. What is Gibbs Free Energy?

Gibbs Free Energy is a thermodynamic quantity that measures the energy available for useful work in a system at constant temperature and pressure. It takes into account changes in enthalpy and entropy to predict whether a reaction will occur spontaneously.

2. How is Gibbs Free Energy related to the reaction CaCO3 <-> CaO + CO2?

In this reaction, the Gibbs Free Energy is used to determine whether the reaction will occur spontaneously. If the Gibbs Free Energy is negative, the reaction will proceed in the forward direction, producing CaO and CO2. If the Gibbs Free Energy is positive, the reaction will not occur spontaneously and an external energy source will be needed to drive the reaction in the forward direction.

3. What factors affect the Gibbs Free Energy of a reaction?

The Gibbs Free Energy is affected by the enthalpy and entropy changes of the reaction, as well as the temperature and pressure. An increase in temperature or pressure can decrease the Gibbs Free Energy of a reaction, making it more likely to occur spontaneously.

4. How is the Gibbs Free Energy calculated?

The Gibbs Free Energy is calculated using the equation ΔG = ΔH - TΔS, where ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy. This equation takes into account the changes in energy and disorder of the system.

5. Can the Gibbs Free Energy be used to predict the direction of a reaction?

Yes, the Gibbs Free Energy can be used to predict the direction of a reaction. If the value of ΔG is negative, the reaction will occur spontaneously in the forward direction. If the value of ΔG is positive, the reaction will not occur spontaneously in the forward direction and an external energy source will be needed to drive the reaction.

Similar threads

  • Biology and Chemistry Homework Help
Replies
1
Views
2K
  • Biology and Chemistry Homework Help
Replies
1
Views
2K
  • Biology and Chemistry Homework Help
Replies
7
Views
2K
  • Biology and Chemistry Homework Help
Replies
1
Views
1K
  • Biology and Chemistry Homework Help
Replies
4
Views
1K
Replies
12
Views
737
  • Biology and Chemistry Homework Help
Replies
1
Views
2K
  • Biology and Chemistry Homework Help
Replies
1
Views
2K
  • Biology and Chemistry Homework Help
Replies
9
Views
2K
  • Biology and Chemistry Homework Help
Replies
7
Views
1K
Back
Top