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The standard reduction potential of zinc...

The standard reduction potential of zinc and silver at 298 K are `E_((Zn^(2+)) /(Zn))^0 = -0.76 V`, `E_((Ag^(+))/(Ag))^0= 0.80V` Which of the following reactions actually takes place in a cell reaction?

A

` Zn^(2+)(aq)+Ag^(+)(aq)rarrZn(s)+Ag(s)`

B

`Zn(s)+Ag(s)rarrZ^(2+)(aq)+Ag^(+)(aq)`

C

`Zn^(2+)(aq)+2Ag(s)rarr2Ag^(+)(aq)+Zn(s)`

D

`Zn(s)+2Ag^(+)(aq)rarrZn^(2+)(aq)+2Ag(s)`

Text Solution

Verified by Experts

The correct Answer is:
D
More the R.P. easier to reduce. Thus `Ag^(+)` will be reduced and Zn will be oxidised.
`Zn(s)+2Ag^(+)(aq)rarrZn^(2+)(aq)+2Ag(s)`
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Standard reduction electrode potential of Zn^(2+)//Zn is -0.76V . This means:

Consider the cell : Zn|Zn^(2+)(aq)(1.0M)||Cu^(2+)(aq)(1.0M)||Cu Thee standard reduction potentials are 0.350V for Cu^(2+)(aq)+2e^(-)rarrCu and -0.763V for Zn^(2+)(aq)+2e^(-) rarr Zn a. Write the cell reaction. b. Calculate the EMF of the cell. c. Is the reaction spontaneous or not ?

For Zn^(2+) //Zn, E^(@) =- 0.76 , for Ag^(+)//Ag, E^(@) = -0.799V . The correct statement is

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The standard oxidation potentials, , for the half reactions are as follows : Zn rightarrow Zn^(2+) + 2e^(-) , E^(@) = +0.76V Fe rightarrow Fe^(2+)+ 2e^(-), E^(@) = + 0.41 V The EMF for the cell reaction, Fe^(2+) + Zn rightarrow Zn^(2+) + Fe