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.

← How to perform the classic tablecloth trick successfully Calculating energy of a photon based on wavelength →

More Posts: