Question

A voltaic cell uses the following reaction: 2Ag+ (aq, 1 M) + Fe (s) ↔ 2Ag (s) + Fe2+ (aq, 1 M) Given that the standard reduction potential of Ag+ to Ag (s) is +0.80 V and the standard reduction potential of Fe2+ to Fe (s) is −0.44 V, calculate the standard cell potential, E°cell.−1.24 V1.24 V2.04 V0.36 V

Answer 1

The standard cell potential of the reaction is 1.24 Volts.

Step-by-step explanation:

`2Ag^+(aq)+Fe(s)\rightarrow 2Ag (s)+Fe^(2+)(aq)`

Reduction at cathode :

`Ag^+(aq)+e^-\rightarrow Ag (s)`

Reduction potential of
`Ag^(+)` to Ag=
`E^o_(1)=0.80 V`

Oxidation at anode:

`Fe(s)\rightarrow Fe^(2+)(aq)+2e^-`

Reduction potential of
`Fe^(2+)` to Fe=
`E^o_(2)=-0.44 V`

To calculate the
`E^o_(cell)` of the reaction, we use the equation:

`E^o_(cell)=E^o_(red,cathode)-E^o_(red,anode)`

Putting values in above equation, we get:

`E^o_(cell)=0.80 V -(-0.44 V)=1.24 V`

The standard cell potential of the reaction is 1.24 Volts.