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The following electrochemical cell has b...

The following electrochemical cell has been set-up,
`Pt(1)|Fe^(3+), Fe^(2+) (a=1)||Ce^(4+), Ce^(3+) (a=1) Pt (2)`
`E^(@) (Fe^(3+) //Fe^(2+))=0.77 V, E^(@) (Ce^(4+)//Ce^(3+))=1.61 V`
If an ammeter is connected between the two platinum electrodes, predict the direction of flow of current. Will the current increase or decrease with time ?

Text Solution

Verified by Experts

For the cell as represented, `E_(cell)^(@)=E_(Ce^(4+),Ce^(3+))^(@)-E_(Fe^(3+),Fe^(2+))^(@)=1.61-0.77=0.84V`
As `E_(cell)^(@) gt 0`, left hand electrode is anode while right hand electrode is cathode. Hence, current will flow from right to left. The current will decrease with time till ultimately the reaction stops.
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