Calculating Standard Gibbs Free Energy Change at 770 K
Question:
For the reaction CO (g) + 2 H2O (g) → CO2 (g) + H2 (g) at 770 K, Keq = 5.10. Calculate the standard Gibbs free energy change (ΔG°) for the reaction at 770 K.
Answer:
The standard Gibbs free energy change (ΔG°) for the reaction at 770 K is approximately -10,060.50 J/mol.
Calculating Standard Gibbs Free Energy Change:
To calculate the standard Gibbs free energy change (ΔG°) for the reaction at 770 K, we can use the equation:
ΔG° = -RT ln(Keq)
Where:
- ΔG° is the standard Gibbs free energy change
- R is the gas constant (8.314 J/(mol·K))
- T is the temperature in Kelvin (770 K)
- Keq is the equilibrium constant (5.10)
Now, let's substitute the values and calculate ΔG°:
ΔG° = - (8.314 J/(mol·K)) * (770 K) * ln(5.10)
ΔG° = - (8.314 J/(mol·K)) * (770 K) * 1.6292405397
ΔG° ≈ -10,060.50 J/mol
Therefore, the standard Gibbs free energy change (ΔG°) for the reaction at 770 K is approximately -10,060.50 J/mol.