These NiCad batteries each have a potential of 1.75 V.The two half reactions occurring are:2Ni(OH)3(s) + 2e- 2Ni(OH)2(s) + 2OH-(aq)Cd(s) + 2OH-(aq) Cd(OH)2(s) + 2e-Which statement is incorrect:Select one:a.Cadmium forms the anode.b.Nickel metal is not involved in the reaction.c.The cadmium becomes eroded as the battery is used.d.The nett battery reaction involves only solid substances.e.The cadmium electrode has the more positive potential.

One common type of rechargeable cell is the nickel–cadmium (NiCad) battery. For each terminal of this battery state the initial and final oxidation number of the element when the cell is delivering a current. Hence deduce which electrode is acting as the anode and which the cathode.

Which of the following batteries is an example of a primary cell?Group of answer choicesNickel-cadmium (NiCd) also known as "nicad"Nickel-metal hydride (NiMH)AlkalineLead acid

At 298 K, the standard electrode potentials of Mg2+/Mg, Ni2+/Ni, Cu2+/Cu and Au3+/Au are –2.36 V, –0.25 V, 0.34 V and 1.40 V respectivelyOn the basis of standard electrode potential, predict which of the following reactions can occur?

The half-reaction at the cathode in an electrochemical cell is given below. What other half-reaction would most likely occur at the anode to produce a spontaneous reaction?Zn2+(aq) + 2e- Zn(s)Click for a reduction potential chartA.H2(g) 2H+(aq) + 2e-B.K+(aq) + e- K(s)C.Al(s) Al3+(aq) + 3e-D.Zn(s) Zn2+(aq) + 2e-

The anode half-reaction occurring during the discharge of a lead storage battery is