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madam [21]
3 years ago
12

10 points) Given the following two half-reactions, write the overall reaction in the direction in which it is product-favored, a

nd calculate the standard cell potential.Pb2+ (aq) + 2 e–à Pb (s) Eº= –0.126 VFe3+ (aq) + e–à Fe2+ (s) Eº = +0.771 V
Chemistry
1 answer:
IceJOKER [234]3 years ago
7 0

Answer:

The over all reaction :

2Fe^{3+}(aq)+Pb(s)\rightarrow 2Fe^{2+}(s)+Pb^{2+}(aq)  

The standard cell potential of the reaction is 0,.897 Volts.

Explanation:

Reduction at cathode :

Fe^{3+}(aq)+e^-\rightarrow Fe^{2+}(s)..[1]  

E^o_{Fe^{3+}/Fe^{2+}}=0.771 V

Reduction potential of Fe^{3+} to Fe^{2+}=0.771 V

Oxidation at anode:

Pb(s)\rightarrow Pb^{2+}(aq)+2e^-.[2]

E^o_{Pb^{2+}/Pb}=-0.126 V

Reduction potential of Pb^{3+} to Pb=-0.126 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}=E^o_{Fe^{3+}/Fe^{2+}}-E^o_{Pb^{2+}/Pb}

=0.771 V-(-0.126 )=0.897 V

The over all reaction : 2 × [1] + [2]

2Fe^{3+}(aq)+Pb(s)\rightarrow 2Fe^{2+}(s)+Pb^{2+}(aq)  

The standard cell potential of the reaction is 0,.897 Volts.

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