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

Answer:

The standard cell potential of the reaction is 1.24 Volts.

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.