Question

Atoms A and X are fictional atoms. Suppose that the standard potential for the reduction of X^2+ is +0.51 V, and the standard potential for the reduction of A^2+ is -0.33. Find the standard potential for an electrochemical cell with the cell reaction that follows.

Answer 1

If you are given the standard potential for the reduction of X^2+ is +0.51 V, and the standard potential for the reduction of A^2+ is -0.33, just add the two. The standard potential for an electrochemical cell with the cell is 0.18V

Answer 2

Answer: Thus the standard potential for an electrochemical cell with the cell reaction that follows is 0.84 V.

Step-by-step explanation:

Standard potential for an electrochemical cell is given by:

`E^0{cell}` = standard electrode potential =
`E^0{cathode}-E^0{anode}`

The
`E^0` values have to be reduction potentials.

Given: Reduction potential for atom X:

`E^o_(X^(2+)/X)=+0.51V`

`E^o_(A^(2+)/A)=-0.33V`

The element A with negative reduction potential will lose electrons undergo oxidation and thus act as anode.The element X with positive reduction potential will gain electrons undergo reduction and thus acts as cathode.

`X^(2+)+A\rightarrow X+A^(2+)`

`E^0{cell}` = standard electrode potential =
`E^0{cathode}-E^0{anode}=+0.51-(-0.33)=0.84V`

Thus the standard potential for an electrochemical cell with the cell reaction that follows is 0.84 V.