What should be change of electrode potential if the `Zn^(2+)` dilution Is increased 100 times of the cell `Zn^(2+)//Zn`?

What will be the change in the half-cell potential, if the concen-tration of Zn^(2+) is diluted 100 times of a Zn^(2+)|Zn half-cell?

Write Nernst equation for electrode potential for the following electrodes : (a) Zn^(2+)+2e rarr Zn

Write the Nernst equation for the half cell Zn_((aq))^(2+)//Zn_((s)).

See whether the cell representation given below is in accordance with the conventation or not. If it is not, then write the correct representation and reaction of the cell. Calculate the standard EMF of the cell: Cu|Cu^(2+)||Zn|Zn^(2+) . ["Given : "E_(Cu^(2+)|Cu)^(@)=+0.34V, E_(Zn^(2+)|Zn)^(@)=-0.76V]

Why standard reduction potential (E^(0)) of Zn^(2+)|Zn system is more negative than expected ?

If Zn^(2+) // Zn electrode is diluted 100 times then what will be the change in e.m.f.

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

A cell is prepared by dipping a zinc rod in 1(M) ZnSo_4 solution. The standard electrode potential for Pb^(2+)/ Pb and Zn^(2+) /Zn electrodes are -0.126V and -0.763 V respectively. Write the half cell reactions and overall cell reaction.

A cell is prepared by dipping a zinc rod in 1(M) ZnSo_4 solution. The standard electrode potential for Pb^(2+)/ Pb and Zn^(2+) /Zn electrodes are -0.126V and -0.763 V respectively. How will you represent the cell?