A voltaic cell is constructed. One electrode compartment consist of a zinc strip

Question

A voltaic cell is constructed. One electrode compartment consist of a zinc strip placed in a solution of Zn (NO3)2, and the other has a nickel strip placed in a solution of NiCl2. The overall cell reaction is: Zn(s)+Ni^2+ (aq)=Zn^2+(aq)+Ni(s).

(a) Write the half-reactions that occur in the two electrode compartments.

(b) Which electrode is the anode and which is the cathode?
(c) Indicate the signs of the electrodes.

(d) Do the electrons flow from the zinc electrode to the nickel electrode or from the nickel to the zinc?
(e) In which direction do the cations and the anions migrate through the solution?

Explanation / Answer

a) Zn (S) = Zn^(2+) (aq) + 2e- Oxidation (anode)

Ni^(2+) (aq) + 2e- = Ni(s) Reduction (Cathode)

b) The Zn electrode where oxidation occurs is the anode

the Ni electrode where reduction occurs is the Cathode

c) The Zn electrode where oxidation occurs is positive

the Ni electrode where reduction occurs is negative

d) The Electron flow from From Zn electrode to Nickel electrode in the external circuit

e) The cations Zn 2+ move away from Zn anode into the solution while the Ni2+ ions move towards the Ni cathode depositing on it. The anions move towards the anode Zn. In general cations move towards Ni cathode and Anions to Zn anode

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