Home
Class 12
CHEMISTRY
If at 25^(@)C the standard emf of the ce...

If at `25^(@)C` the standard emf of the cell `|Zn(s)|Zn^(2+)(1M)||Cu^(2+)(0.1M)|Cu(s)` is 1.3 volt, calculate the emf of the cell.

Text Solution

Verified by Experts

`Zn(s)|Zn^(2+) (1M)|Cu^(2+)(0.1 M)|Cu(s)`
Standard emf of the cell `(E_("cell")^(@)) = 1.3` volt
`E_("cell") = ?`
From Nernst equation, we have
`E_("cell") = E_("cell")^(@) - (0.0591)/(n) log""([Zn^(2+)])/([Cu^(2+)])`
`= 1.3 - (0.0591)/(2) log""(1)/(0.1)`
`= 1.3 - 0.0295 xx log 10`
`= 1.3 - 0.0295 = 1.2705`
Promotional Banner

Similar Questions

Explore conceptually related problems

If at 25^@C , the standard emf of the cell |Zn(s)| Zn^2+ (1M) || Cu^2(0.1 M) | Cu (s) is 1.3 volt, calculate the emf of the cell.

The standard emf for the cell reaction, Zn+Cu^(2+) =Cu+Zn^(2+) is 1.10 volt at 25^@C . The emf for the cell reaction, when 0.1MCu^(2+) and 0.1 MZn^(2+) solutions are used , at 25^@C is:

For the cell Zn|Zn^(2+)||Cu^(2+)|Cu if the concentration of Zn^(2+) and Cu^(2+) ions is doubled, the emf of the cell:

Calculate the standard electrode potential of Ni^(2+) | Ni electrode if emf of the cell, Ni(s) | Ni^(2+) ( 0.01 M ) || Cu^(2+) ( 0.1M) | Cu(s) is 0.059 V. [ Given E_(Cu^(2+) //Cu) ^(@) = + 0.34V

The emf of the cell involving following changes Zn(s)+Ni^(2+)(1M)rarrZn^(2+)(1M)+Ni(s) is 0.5105V. The standard emf of the cell is :

The emf of the cell, Zn|Zn^(2+)(1M)||Cu^(2+)|Cu(1M) is 1.1 volt, if the standard reduction potential of Zn^(2+)|Zn is -0.78 volt,what is the oxidation potential of Cu|Cu^(2+) ?