How does a metal oxide becomes unstable and decomposes when gibbs free energy becomes positive?
How does a metal oxide becomes unstable and decomposes when gibbs free energy becomes positive?
Actually every compound or molecule want to achieve its lowest energy state, this is general law of nature.
When we say G of a reaction is negative, it means at any supplied temperature molecules have final energy less than initial energy and in other words we say that molecules are reacting and form more stable compounds.
Now coming on to question, whenever G of metal oxides becomes positive, it means in formation of metal oxide from metal and oxygen, molecules goes towards less stability than they had. And no molecules want to go in reaction in which it become less stable thus metal oxide dissociate and becomes stable as G of dissociation will be negative if G of formation of metal oxide was positive.
Actually every compound or molecule want to achieve its lowest energy state, this is general law of nature.
When we say G of a reaction is negative, it means at any supplied temperature molecules have final energy less than initial energy and in other words we say that molecules are reacting and form more stable compounds.
Now coming on to question, whenever G of metal oxides becomes positive, it means in formation of metal oxide from metal and oxygen, molecules goes towards less stability than they had. And no molecules want to go in reaction in which it become less stable thus metal oxide dissociate and becomes stable as G of dissociation will be negative if G of formation of metal oxide was positive.
