The given reaction is:
CCl4 + 2H2O → CO2 + 4 HCl
The standard Gibbs free energy change for this reaction is, ΔG°= -232 kJ/mole. Since ΔG is negative, this implies that the above reaction must be spontaneous and thermodynamically favored.
However, the activation energy for this reaction is high. This implies that when CCl4 and H2O collide they need to overcome an energy barrier to form the products. In other words, although the reaction is thermodynamically favored it is not kinetically favored. The reaction might proceed at an extremely slow rate as a result of which no obvious change might be observed.
This reaction does not occur easily because the activation energy of the process is high.
The term activation energy refers to the energy that is required that reactants possess before they can cross the energy barrier between reactants and products.
We can see that the change in free energy for this reaction negative hence a sponteanous reaction is expected. However, this reaction does not occur easily because the activation energy of the process is high and the can only be overcome by addition of energy maybe via a spark.
Learn more about activation energy: https://brainly.com/question/14502795?
