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The chemical reaction takes place only in one direction and Oxidation–reduction reactions, commonly known as redox reactions, are reactions that involve the transfer of electrons from one species to another in other words In a redox reaction, both oxidation and reduction occur simultaneously, for redox reaction the reactant is converted into product and vice versa.

The magnitude of the chemical rate constant, kc, will determine the extent to which Red reacts to form Z. If kc is large, the redox couple Ox/Red will be chemically irreversible on the time scale of the experiment. If kc is small (or zero), the observed couple will be chemically reversible

Commonly, the irreversible reaction means that the equilibrium is considerably shifted to one side and the reversed reaction is too slow. Thus, truly irreversible reactions do not exist. In electrochemistry, the electron moves between an molecule and electrode, S + e = S- . So, if you change a potential, at certain point the amplitude of current will increase until all S is converted to S- . The current returns to the initial value. If now you scan potential in opposite direction, you will observe S- . If both S and S- are stable, then on reversed potential scan the oxidation of S- results in formation of S. This is one-electron electrochemically reversible process. If S- is unstable and form product P, then on reversed scan you will not see S- . This is the electrochemically irreversible process. If you are able to convert P back to S- and remove one electron from S- , you will have chemically reversible reaction.

Thus, chemically all reactions are reversible in principal. The irreversible reaction means that the reversed reaction is too slow.

In other words, reversibility is the thermodynamic term, but the reaction kinetics may affect the rate of achieving the equilibrium.