Home
Class 12
CHEMISTRY
The cell in whiCHM the following reactio...

The cell in whiCHM the following reaction occurs `:`
`2Fe^(3+)(aq)+2I^(c-)(aq) rarr 2Fe^(2+)(aq)+I_(2)(s)` has
`E^(c-)``_(cell)=0.2136V` at `298K`. Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.

Text Solution

Verified by Experts

`DeltaG^(0)=-nFE^(@)`
`=-2 xx 96500 xx0.236J`
`=-45548J=-45.548kJ`
`"K=Antilog"[(nE^(@))/(0.059)]"= Antilog"(2xx0.236)/(0.059)=10^(8)`
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • ELECTRO CHEMISTRY

    NARAYNA|Exercise W.E-7|1 Videos

  • ELECTRO CHEMISTRY

    NARAYNA|Exercise W.E-8|1 Videos

  • ELECTRO CHEMISTRY

    NARAYNA|Exercise W.E-5|1 Videos

  • 15TH GROUP ELEMENTS

    NARAYNA|Exercise EXERCISE - 4 (NCERT EXEMPLERS/HOTs)|27 Videos

Similar Questions

Explore conceptually related problems

Thus emf of the cell = 0.91 V. Q.3.6. The cell in which the following reaction occurs : 2Fe^(3+) (aq) + 2I^(-)(aq) to 2Fe^(2+0 (aq) + I_(2)(s) has E_("cell")^(@) = 0.236 V at 298 K Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.

The cell in which the following reaction occurs: 2Fe^(3+)(aq)+2I^(-)(aq)to2Fe^(2+)(aq)+I_(2)(s) has E_(cell)^(@)=0.236V at 298K. Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.

Knowledge Check

  • What is ‘A’ in the following reaction? 2Fe^(3+) (aq) + Sn^(2+) (aq) rarr 2 Fe^(2+) (aq) + A

    A
    `Sn^(3+)(aq)`
    B
    `Sn^(4+) (aq)`
    C
    `Sn^(2+) (aq)`
    D
    `Sn(s)`

  • The cell in which the following reaction occurs : 2Fe_(aq)^(3+) + 2I_(aq)^(-) to 2Fe_(aq)^(2+) + I_(2(s)) "has" E_("cell")^(o) = 0.236 V "at" 298 K The equilibrium constnat of the cell reaction is

    A
    `6.69xx 10^(-7)`
    B
    `9.69 xx 10^(-7)`
    C
    `9.69 xx 10^(7)`
    D
    `6.69 xx 10^(7)`

    • Similar Questions

    Explore conceptually related problems

    The cell in which the following reaction occurs : 2Fe^(3+)(aq)+2I^(-)(aq)rarr2Fe^(2+)(aq)+I_(2)(s)" has "E_("cell")^(@)=0.236V . Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.

    The cell in which the following reaction occurs 2Fe^(3+)(aq)+2I^(-)(aq)to2Fe^(2+)(aq)+I_(2)(aq)+I_(2)(s) has E_(cell)^(0)=0.236V at 298 K. Calculate the standard gibbs energy and the equilibrium constant of the cell reaction.

    The cell in which the following reaction occurs 2Fe^(3+)(aq)+2I^(-)(aq) to 2Fe^(2+)(aq)+2I_(2) " has "E_(cell)^(@)=0.236 V " at "298 K . Calculate standard Gibbs energy and equilibrium constant for the reaction.

    The cell in which the following reaction occurs 2Fe^(3+)(aq)+2I^(-)(aq)to2Fe^(2+)(aq)+I_(2)(s) has E_(cell)^(@)=0.236V at 298K. Calculate the standard gibbs energy of the cell reaction. (Given: 1F=96,500" C "mol^(-1) )

    (a) The cell in which the following reaction occurs: 2Fe^(3+) (aq) + 2I^(-) (aq) to 2Fe^(2+) (aq) + I_(2) (s) has E_("cell")^(@) 0.236 V at 298 K. Calculate the standard Gibbs energy of the cell reaction. [Given: 1F = 96,500 C mol^(-1) ] (b) How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 hours? [Given: 1F =96,500 mol^(-1) ]

    (a) The cell in which the following reactions occurs: 2Fe^(3+)(aq)=2I^(-)(aq)to2Fe^(2+)(aq)+I_(2)(s) has E_(cell)^(@)=0.236V at 298 K. Calculate the standard Gibbs energy of the cell reaction. (Given: 1F=96,500" C "mol^(-1) ) (b) How many electrons flow through a metallic wire if a current of 0.5 A is passed for 2 hours? (Given: 1F=96,500" C "mol^(-1) )

    Home
    Profile