Respuesta :
Answer : The standard potential for the given cell is 0.9 V
Explanation :
The standard reduction potentials for zinc and copper are:
[tex]E^o_{(Mn^{2+}/Mn)}=-1.18V\\E^o_{(Co^{2+}/Co)}=-0.28V[/tex]
The substance having highest positive [tex]E^o[/tex] potential will always get reduced and will undergo reduction reaction.
Here, cobalt will undergo reduction reaction will get reduced. Manganese will undergo oxidation reaction and will get oxidized.
Oxidation half reaction: [tex]Mn\rightarrow Mn^{2+}+2e^-[/tex]
Reduction half reaction: [tex]Co^{2+}+2e^-\rightarrow Co[/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]
[tex]E^o_{cell}=E^o_{(Co^{2+}/Co)}-E^o_{(Mn^{2+}/Mn)}[/tex]
Putting values in above equation, we get:
[tex]E^o_{cell}=(-0.28V)-(-1.18)=0.9V[/tex]
Hence, the standard potential for the given cell is 0.9 V
The standard potential of the given cell is 0.9 V. The cell potential is the potential difference between anode and cathode.
What is the standard potential of a cell?
It is the potential difference between a cathode and anode at 298 K, 1 atm, and 1 M solution.
[tex]E^0_{cell} = E^0_{cathode} -E^0_{anode} [/tex]
Where,
[tex]E^0 _{cell} [/tex] - the standard potential of a cell
[tex] E^0_{cathode} [/tex] - Reduction potential of cobalt
[tex]E^0_{anode} [/tex] - Reduction potential of Magnease
Put the values in the formula,
[tex]E^0_{cell} = (-28\rm \ V)- (-1.18 \rm \ V)\\\\E^0_{cell} = 0.9 \rm \ V[/tex]
Therefore, the standard potential of the given cell is 0.9 V.
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