What is the overall cell potential for this redox reaction? cd + hg22+ → cd2+ + 2hg given: cd2+ + 2e− → cd(s) = –0.40 and hg22+ + 2e− → 2hg(l) = 0.79 –0.19 v 0.19 v 0.91 v 1.19 v

 1.19 V

Explanation:

Standard potential for an electrochemical cell is given by:

= standard electrode potential =

The values have to be reduction potentials.  

Given:

Cadmium is losing electrons , undergo oxidation and thus act as anode. mercury is gaining electrons, undergo reduction and thus acts as cathode.

= standard electrode potential =

Thus the standard potential for an electrochemical cell with the cell reaction is 1.19 V.

The overall cell potential for this redox reaction : 1.19V

Cd + Hg₂²⁺ → Cd²⁺ + 2Hg

Cell potential (E °) is the potential difference between the two electrodes in an electrochemical cell.

Electric current moves from a high potential pole to a low potential, so the cell potential is the difference between an electrode that has a high electrode potential (cathode) and an electrode that has a low electrode potential (anode)

or:

E ° cell = E ° reduction-E ° oxidation

(At the cathode the reduction reaction occurs, the anode oxidation reaction occurs)

The value of E⁰ cells uses a reference electrode which is used as a comparison called the Standard Electrode which is the hydrogen-platinum electrode

In reaction:

Cd + Hg₂²⁺ → Cd²⁺ + 2Hg

Given:

Cd²⁺+ 2e⁻ → Cd (s) = –0.40V and

Hg²⁺ + 2e⁻ → 2Hg (l) = 0.79V

From the value of E ° cells, it can be seen that the higher E ° cells will act as positive poles or cathodes namely Hg₂²⁺

So the reaction happens

at the anode (oxidation reaction) Cd ------> Cd²⁺ + 2e⁻ E ° = +0.40 V

at the cathode (reduction reaction) Hg₂²⁺ + 2e− → 2Hg (l) = 0.79 V

E ° cell = E ° cathode -E ° anode = 0.79 V - (-0.40V) = 1.19V

The standard cell potential

link

link

link

Keywords: cell potential, cathode, anode, reduction, oxidation

h