Question

What is the voltage of an electrolytic cell with nickel and copper electrodes?

Answer 1

the voltages cells electromotive force derived from the reduction potentials of each cell, here we have ,

${ni}^{2} {aq} \: + 2e - that \: gives \: ni{s} \: where \: e = - 0.23v \\ {cu}^{2} {aq} \: + 2e \: that \: gives \: cu{s} \: where \: e = 0.34v \\ {cu}^{2} {aq} \: + ni that \: gives \: {ni}^{2} + cu \: \\ where \: e =ered - eox \: \\ e = 0.57v \:$

quantitative play this is a copper coin is introduced and Nickel ions full stop hence the cells reaction would be,

Answer 2

$\huge\sf{\pink{\underline{\underline {♡Answer}}}}$

The voltage is the cell's electromotive force derived from the reduction potentials of each cell, here we have,

Ni2+(aq)+2e−→Ni(s)

where

E=−0.23V

Cu2+(aq)+2e−→Cu(s)

where

E=0.34V

Quantitatively, this is saying copper ions are more easily reduced than nickel ions. Hence, the cell's reaction would be,