Home
Class 12
CHEMISTRY
The standard e.m.f of a cell, involving ...

The standard e.m.f of a cell, involving one electron change is found to be 0.591 V at `25^(@) C`. The equilibrium constant of the reaction is : `(F=96,500C mol^(-1)`: R=8.314 `Jk^(-1)mol^(-1)`

A

`1.0 xx10^(1)`

B

`1.0xx10^(5)`

C

`1.0xx10^(10)`

D

`1.0xx10^(30)`

Text Solution

Verified by Experts

The correct Answer is:
C
Relation between `K_(eq)` and `E_("cell")^(@)` is
`E_("cell")^(@)=0.0591/n"log" K_(eq)` (at 298 K)
`0591=0.0591/1log K_(eq)`
`:. K_(eq)=1xx10^(10)`
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    BITSAT GUIDE|Exercise BITSAT Archives|13 Videos

  • D AND F BLOCK ELEMENTS

    BITSAT GUIDE|Exercise BITSAT Archives|10 Videos

  • GENERAL ORGANIC CHEMISTRY

    BITSAT GUIDE|Exercise BITSAT|13 Videos

Similar Questions

Explore conceptually related problems

The standard e.m.f. of a cell, invoving one electron change is found to be 0.591 V at 25^0C . The equilibrium constant of the reaction is ( F= 96500 mol^-1, R=8.314 JK^-1mol^-1)

The standard emf of a cell having one electron change is found to be 0.591 V at 25^@ C , The equilibrium constant of the reaction is :

For a cell involving two electron change , E_(cell)^(@) = 0.3 V at 25^(@) C . The equilibrium constant of the reaction is