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Using the standart electrode potential f...

Using the standart electrode potential find out the pair between which redox reaction is not feasible
`E^(-)` values `Fe^(3+)//Fe^(2+)=+0.77 I_(2) / I =+0.54 V`
`Cu^(2+)//Cu=+0.34 Ag^(+)//Ag=+80 v`

A

`Fe^(3+)` and `I^(-)`

B

`Ag^(+)` and Cu

C

`Fe^(3+)` and Cu

D

`Ag^(+)` and `Fe^(3+)`

Text Solution

Verified by Experts

The correct Answer is:
A
`Ag^(+)` and `Fe^(3+)` reaction is not feasible because they have almost same standard electrode potential
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Using the standard electrode potential, find out the pair between which redox reaction is not feasible. E^(@) values : Fe^(3+)//Fe^(2+)=+0.77, I_(2)//I^(-)=+0.54 V Cu^(2+)//Cu= + 0.34 V, Ag^(+)//Ag= +0.80 V

Using the standard electrode potential, find out the pair between which redox reaction is not feasible. E^(θ) values: Fe^(3+)//Fe^(2+)=0.77, I_(2)//I^(-)=+0.54 , Cu^(2+)//Cu=+0.34, Ag^(+)//Ag=+0.80V

The more positive the value of E^(θ) , the greater is the trendency of the species to get reduced. Using the standard electrode potential of redox coples given below find out which of the following is the strongest oxidising agent. E^(θ) values: Fe^(3+)//Fe^(2+) = +0.77 I_(2)(s)//I^(-) = +0.54 , Cu^(2+)//Cu = +0.34, Ag^(+)//A = 0.80V

On the bassis of standard electrode potential of redox couples given below, find out which of the following is the strongest oxdising afent . (E^@ value : Fe^(3+)) = + 0. 77 C, I_(2(g)) | I = + 0/ 54 V , Cu^(2+) | Cu = + 34 V, Ag^(+) |Ag = + 0. 80 V) .

MHTCET PREVIOUS YEAR PAPERS AND PRACTICE PAPERS-ELECTROCHEMISTRY-Exercise 2
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