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(a) The cell in which the following reac...

(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)`)

Text Solution

Verified by Experts

(a) `2Fe^(3+)+2I^(-)to2Fe^(2+)+I_(2)(s)`
`E^(@)cell=0.236V,1F=96500C//mol`
`e^(-)+Fe^(3+)toFe^(2+)Jxx2`
`2I^(-)toI_(2)+2e^(-)`
`underlineoverline(" "2Fe^(3+)+2I^(-)+2e^(-)to2Fe^(2+)+I_(2)+2e^(-)" ")`
`thereforen=2`
`DeltaG^(@)=-nFE^(@)cell`
`=-2xx96500xx0.236`
`DeltaG^(@)=45548J`
(b) Quantity of electricity flowing through the wire
`=0.5xx2xx60xx60=3600C`
1F (96500C) is equivalent to flow of 1 mole o `e^(-)` i.e., `6.022xx10^(23)e^(-)s`
`therefore3600C` will be equivalent to `=(6.022xx10^(23))/(96500)xx3600=2.25xx10^(22)e^(-)`s
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(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) ]

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) )

Knowledge Check

  • 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)`

  • For the cell reaction: 2Fe^(3+)(aq)+2l^(-)(aq)to2Fe^(2+)(aq)+l_(2)(aq) E_(cell)^(ɵ)=0.24V at 298K . The rstandard gibbs energy (triangle,G^(ɵ)) of the cell reaction is [Given that faraday constnat F=96400Cmol^(-1)]

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    B
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    C
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    D
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