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For the reduction of silver ions with co...

For the reduction of silver ions with copper metal, the standard cell potential was found to be + 0.46 V at 25 `"^@C` . The value of standard Gibb's energy, `Delta"^@C` will be (F = 96500 C `mol^(-1)` )

A

-89.0 KJ

B

-89.0 J

C

-44.5 KJ

D

-98.0 KJ

Text Solution

Verified by Experts

The correct Answer is:
A
The cell reaction can be written as
`Cu+2Ag^(+)toCu^(2+)+2Ag`
We know, `DeltaG^@=-nFE_(cell)^@`
= `-2xx96500xx0.46=-88780` J
`=-88.780 KJ~~-89` KJ
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For the reduction of silver ions with copper metal, the standard cell potential was found to be +0.46 V at 25^(@) C. The value of standard Gibbs energy. DeltaG^(@) will be (F= 96500 C "mol"^(-1) )

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Knowledge Check

  • For the reduction of silver ions with copper metal, the standard cell potential was found to be +0.46V at 25 ^ (@)C the value of the standard Gibb's energy , DeltaG^(@) will be

    A
    `-98.0kJ`
    B
    `89.0 kJ`
    C
    `-89.0J`
    D
    `44.5kJ`.

  • For the reduction of silver ions with copper metal, the standard cell potential was foound to be +0.46 V at 25^(@) C . The value of standard Gibbs energy, DeltaG^(@) will be (F = 96,500C mol^(-1)) :

    A
    `-98.00 kJ`
    B
    `-89.0 kJ`
    C
    `-89.0 J`
    D
    `-44.5 kJ`

  • For the reduction of silver ions with copper metal, the standard cell potential was found to be +0.46 V at 25^(@) C. The value of standard Gibbs energy. DeltaG^(@) will be (F= 96500 C "mol"^(-1) )

    A
    `-98.0 kJ`
    B
    `-89.0 kJ`
    C
    `-89.0 J`
    D
    `-44.5 kJ`

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