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IceJOKER [234]
3 years ago
7

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
Chemistry
1 answer:
sukhopar [10]3 years ago
8 0

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.

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