For a general redox reaction

Anode: $$\text{Red}_1 \to \text{Ox}_1^{n_1+} + n_1 e^-$$

Cathode: $$\text{Ox}_2 + n_2 e^- \to \text{Red}_2^{n_2-}$$

Which of the following statement is **incorrect** ?

The overall reaction can be written as $$n_2\text{Red}_1 + n_1\text{Ox}_2 = n_2\text{Ox}_1^{n_1+} + n_1\text{Red}_2^{n_2-}$$

The electrons do not appear in the overall reaction because electrons produced at the anode are consumed at the cathode.

Here n is the number of electrons transferred in redox reaction.

If the reaction is carried out reversibly, the electrical work done is equal to the ratio of charge and potential difference through which charge is moved.