Explanation As it is evident from the given data of Gibbs free energy, this reaction is not only feasible thermodynamically, it is also a spontaneous reaction. But, despite being a spontaneous reaction, it requires some amount of activation energy as the initial requirement. Once this activation energy is supplied and the reaction starts occurring, it produces enough amount of energy (as given in the question) to sustain the proceeding of the reaction. Hence, after we provide the initial amount of energy required, this reaction proceeds on its own. But at room temperature, it is not possible to provide the required activation energy. Hence, some initial heating is necessary. Final answer The above reaction does not take place at room temperature because at room temperature, this reaction does not get the energy required as the activation energy for this reaction.
