Answer: The standard potential for the given cell is 0.89 V
Explanation:
The standard reduction potentials for zinc and copper are:
[tex]E^o_{(Cu^{2+}/Cu)}=+0.13V\\E^o_{(Zn^{2+}/Zn)}=-0.76V[/tex]
The substance having highest positive [tex]E^o[/tex] potential will always get reduced and will undergo reduction reaction. Here, copper will undergo reduction reaction will get reduced.
Zinc will undergo oxidation reaction and will get oxidized.
Oxidation half reaction: [tex]Zn\rightarrow Zn^{2+}+2e^-[/tex]
Reduction half reaction: [tex]Cu^{2+}+2e^-\rightarrow Cu[/tex]
Oxidation reaction occurs at anode and reduction reaction occurs at cathode.
To calculate the [tex]E^o_{cell}[/tex] of the reaction, we use the equation:
[tex]E^o_{cell}=E^o_{cathode}-E^o_{anode}[/tex]
Putting values in above equation, we get:
[tex]E^o_{cell}=0.13-(-0.76)=0.89V[/tex]
Hence, the standard potential for the given cell is 0.89 V
The cell potential of the galvalnic or voltaic cell is 1.1 V.
The Nernst equation is used to calculate the cell potential of an electrochemical cell under non standard conditions.
Now we know that;
E= E° - 0.0592/nlog Q
E° = 1.1 - 0.0592/2 log(1/1)
E° = 1.1 V
Hence, the cell potential of the galvalnic or voltaic cell is 1.1 V.
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