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The standard emf of the cell, Cd((s))|...

The standard emf of the cell,
`Cd_((s))|CdCI_(2(aq))(0.1 M)||AgCI_((aq))|Ag_((s))`
in which the cell reaction
`Cd_((s))+2AgCI_((s))to2Ag_((s))+Cd_((aq))^(2+)+2CI_((aq))^(-)` is 0.6915 V at 0 `"^@C` and 0.6573 V at 25 `"^@C` . The enthalpy change of the reaction at 25 `"^@C` is

A

+48.179 KJ

B

-205.5 KJ

C

+123.5 KJ

D

-167.26 KJ

Text Solution

Verified by Experts

The correct Answer is:
B
Given `E_1=0.6915 V, T_1=273 K`
`E_2=0.6573 V, T_2=298` K
Now, `DeltaG=-nFE_(cell)=-2xx96500xx0.6573=-126858.9`
`DeltaS=nF((eE)/(eE))_p`
where `((eE)/(eE))` = Temperature coefficient of emf
`((eE)/(eE))_p` = `(E_2-E_1)/(T_2-T_1)=(0.6573-0.6915)/(298-273)=-0.001368`
`therefore` `DeltaS=2xx96500xx(-0.001368)=-264.024 J K^(-1) mol^(-1)`
Now, `DeltaG=DeltaH-TDeltaS`
`-126858.9=DeltaH-298xx(-264.024)`
`DeltaH=-205538.052 J=-205.5` KJ
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Knowledge Check

  • The standard emf of the cell, Cd(s) |CdCI_(2) (aq) (0.1M)||AgCI(s)|Ag(s) in which the cell reaction is Cd(s) +2AgCI(s) rarr 2Ag(s) +Cd^(2+) (aq) is 0.6915 V at 0^(@)C and 0.6753V at 25^(@)C . The DeltaH of the reaction at 25^(@)C is,-

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    B
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    D
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