Home
Class 12
CHEMISTRY
If the standed electrode potential for a...

If the standed electrode potential for a cell is 2 V at 300 K, the equilibrium constant (K) for the reaction
`Zn(s)+Cu^(2+)(aq) hArrZn^(2+)(aq)+Cu(s)`
at 300 K is approximately
`(R=8JK^(-1)mol^(-1),F=96000Cmol^(-1))`

A

`e^(-80)`

B

`e^(-160)`

C

`e^(320)`

D

`e^(160)`

Text Solution

AI Generated Solution

Promotional Banner

Similar Questions

Explore conceptually related problems

If the standard electrode potential for a cell is at 300 K, the equilibrium constant (K) for the reaction Zn(s) + Cu^(2+) (aq) at 300 k is approximately : (R=8JK^(-1) mol^(-1) , F= 96000 mol^(-1))

The standard electrode potential for Deniell cell is 1.1V . Calculate the standart Gibbs energy for the reaction. Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq)+Cu(s)

The standard electrode potential for Daniell cell is 1.1 V. Calculate the standard Gibbs energy for the reaction. Zn(s)+Cu^(2+)(aq)rarrZn^(2+)(aq)+Cu(s)

The equilibrium constant of the reaction : Zn(s)+2Ag^(+)(aq)toZn(aq)+2Ag(s),E^(@)=1.50V at 298 K is

Calculate the equilibrium costant log (K_(c)) for the reaction Zn(s)+Cu^(2+)(aq)rarrZn^(2+)(aq)+Cu(s) [Given E_(cell)^(2)=1.1 V ]

The equilbrium constant for the reaction : Cu + 2 Ag^(+) (aq) rarr Cu(2+) (aq) +2 Ag, E^@ = 0. 46 V at 299 K is

The equilibrium constant (K) for the reaction Cu(s)+2Ag^(+) (aq) rarr Cu^(2+) (aq)+2Ag(s) , will be [Given, E_(cell)^(@)=0.46 V ]

Calculate the equilibrium constant for the reaction at 298K. Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq) +Cu(s) Given, E_(Zn^(2+)//Zn)^(@) =- 0.76V and E_(Cu^(2+)//Cu)^(@) = +0.34 V