Home
Class 12
CHEMISTRY
Consider the following E^@ values . E(F...

Consider the following ` E^@` values . `E_(Fe^(3+)//Fe^(2+)^@ = + 0.77 V`,
`E_(Sn^(2+)//Sn)^@=- 15. V` The `E_(cell)^@` for the reaction ,
`Sn (s) + 2Fe_(aq)^(3+) rarr 2 Fe_(aq.)^(2+) + Sn_(aq.)^(2+) is :

A

`-0.58 V`

B

`-0.30 V`

C

`+0.30V`

D

`+0.58 V`

Text Solution

Verified by Experts

The correct Answer is:
c
At anode `: Fe(s) rarr Fe^(2+)(aq)+2e^(-)`
`(` hald oxidation `)`
At cathode `: Sn^(2+)(aq)+2e^(-) rarr Sn(s)`
`(` half reduction `)`
`ulbar(Cell reaction : Fe(s)+Sn^(2+)(aq)rarr Fe^(2+)(aq)+Sn(s))`
`E^(c-)._(cell)=(E^(c-)._(red))_(c)-(E^(c-)._(red))_(a)`
`=(-0.14)-(0.44)=0.30V.`
Promotional Banner

Similar Questions

Explore conceptually related problems

Consider the following E^(@) values E^(@)(Fe^(3+)|Fe^(2+))=+0.77V,E^(@)(Sn^(2+)|Sn)=-0.14V under standard conditions , the potemtial for the reaction : Sn(s)+2Fe^(3+)(aq)to2Fe^(2+)(aq)+Sn^(2+)(aq) is

Given E_(Fe^(3+)//Fe)^(@) = -0.36 V, E_(Fe^(2+)//Fe)^(@)= - 0.439V . The value of standard electrode potential for the change , Fe^(3+)+e^(-) rarr Fe^(2+) will be

Determine the feasibility of the reaction 2Al_((s))+3Sn_((aq))^(4+)rarr 2Al^(3+)+3Sn_((aq))^(2+)

The equilibrium constant of the reaction : A_((s))+2B_((aq))^(+)hArr A_((aq))^(2+)+2B_((s)): E_(cell)^(@)=0.0295V is :

Calculate Delta_rG^@ for the following reactions: Fe^(+2) (aq)+Ag^(+) (aq) to Fe^(+3) (aq)+Ag (s)

Given electrode potentials are , Fe^(3+) + e to Fe^(2+), E^@ = 0.771V " " I_2 + 2e to 2I^(-), E^@ = 0.536 V , E^@ cell for the cell reaction, 2Fe^(3+) + 2I^(-) to 2Fe^(2+) + I_2 is