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Given : E(Fe^(3+)//Fe)^@=-0.036 V E(Fe^...

Given : `E_(Fe^(3+)//Fe)^@=-0.036` V `E_(Fe^(2+)//Fe)^@=-0.439` V. The value of standard electrode potential for the change,
`Fe_((aq))^(3+)+e^(-)toFe_((aq))^(2+)` will be

A

-0.072 V

B

0.385 V

C

0.770 V

D

-0.270 V

Text Solution

Verified by Experts

The correct Answer is:
C
Given, `Fe^(3+)+3e^(-)toFe, E_(1)^@=-0.036` V
`Fe^(2+)+2e^(-)toFe, E_(2)^@=-0.439` V
Required equation is
`Fe^(3+)+e^(-)toFe^(2+), E_3^(@)=?`
Applying, `DeltaG^@=-nFE^@` `therefore` `DeltaG_3^@=DeltaG_1^@-DeltaG_2^@`
`(-n_3FE_3^@)=(-n_1FE_1^@)-(-n_2FE_2^@)`
`E_3^@=3E_1^@-2E_2^@=3xx(-0.036)-2xx(-0.439)`
`E_3^@` =-0.108+0.878=0.77 V
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MTG GUIDE-ELECTROCHEMISTRY-NEET Café (Topicwise Practice Questions) (CELLS AND ELECTRODE POTENTIAL)
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