Question

Using these metal ion/metal standard reduction potentials Cd2+(aq)|Cd(s) Zn2+(aq)|Zn(s) Ni2+(aq)|Ni(s) Cu2+(aq)/Cu(s) -0.40 V -0.76 V ‑0.25 V +0.34 V Calculate the standard cell potential for the cell whose reaction is Ni2+(aq) + Zn(s) →Zn2+(aq)+ Ni(s)

Answer 1

Answer: The standard cell potential for the cell is +0.51 V

Explanation:

Given : $E^0_{Ni^{2+}/Ni}=-0.25V$

$E^0_{Zn^{2+}/Zn}=-0.76V$

The given reaction is:

$Ni^{2+}(aq)+Zn(s)\rightarrow Zn^{2+}(aq)+Ni(s)$

As nickel is undergoing reduction, it acts as cathode and Zinc is undergoing oxidation, so it acts as anode.

$E^0_{cell}=E^0_{cathode}-E^0_{anode}$

where both $E^0$  are standard reduction potentials.

Thus putting the values we get:

$E^0_{cell}=-0.25-(-0.76)$

$E^0_{cell}=0.51V$

Thus the standard cell potential for the cell is +0.51 V