Home
Class 12
CHEMISTRY
The standard emf for the cell cell react...

The standard emf for the cell cell reaction ` Zn + Cu^(2+) rarr Zn^(2+) + Cu ` is 1.10 volt at ` 25^@ C`. The emf for the cell reaction when ` 0.1 M Cu^(2+)` and ` 0.1 M ZN^(2+)` solutions are used at `25^@ =C` is .

A

`1.10` volt

B

`0.110` volt

C

`-1.10` volt

D

`-0.110` volt

Text Solution

Verified by Experts

The correct Answer is:
A
`E_("cell")= E_("cell")^(@) -(0.0591)/(n)"log" ([Zn^(2+)])/([cu^(2+)])`
`= 1.10- (0.0591)/(2) log = 1.10 V`
Promotional Banner

Similar Questions

Explore conceptually related problems

The measured e.m.f. at 25^(@)C for the cell reaction, Zn(s) +XCu^(2+)._((eq))(1.0M) rarr Cu(s) ._((aq))(0.1M) is 1.3 volt, calculate E^(@) for the cell reaction.

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

For the redox reaction: Zn(s) +Cu^(2+) (0.1M) rarr Zn^(2+) (1M)+Cu(s) taking place in a cell, E_(cell)^(@) is 1.10 volt. E_(cell) for the cell will be (2.303 (RT)/(F) = 0l.0591)

The emf of a cell corresponding to the reaction Zn +2H^(+)(aq) rarr Zn^(2+) (0.1M) +H_(2)(g) 1 atm is 0.28 volt at 25^(@)C . Calculate the pH of the solution at the hydrogen electrode. E_(Zn^(2+)//Zn)^(@) =- 0.76 volt and E_(H^(+)//H_(2))^(@) = 0

For the net cell reaction of the cell Zn(s) |Xn^(2+) ||Cd^(2+) |Cd(s) DeltaG^(@) in Kilojules at 25^(@)C is (E_(cell)^(@) = 0.360 V) :-

The emf of the cell involving the following reaction, 2Ag^(+) +H_(2) rarr 2Ag +2H^(+) is 0.80 volt. The standard oxidation potential of silver electrode is:-