A cell is prepared by dipping a copper rod in 1 M `CusO_4` and nickel rod in 1 M `NiSO_4` solution.
`(E^0)_((Cu^(+2))/Cu=0.34V` , `(E^0)_((Cl^-)/(Cl))=0.36V`
Give cell construction.

Explain Can Cl_2 be stored in copper cylinder ? (E^0)_((Cu^(2+))/(Cu)=0.34V , (E^0)_(Cl^-)/(Cl)=0.36V

A galvanic cell is made by dipping a Zn - rod in 0.1 (M) Zn(NO_(3))_(2) and a Pb - rod in 0.25 (M) Pb(NO_(3))_(2) solution. Calculate EMF of the cell, write the cell reaction and represent the cell. Given : E_(Pb^(2+)|Pb)^(@)=-0.13V, E_(Zn^(2+)|Zn)^(@)=-0.77V.

Will Cu dissolve as Cu^(2+) in 1 (M) HCl solution? Will it do so in 1 (M) HNO_(3) solution? ["Given : "E_(Cu^(2+)|Cu)^(@)=+0.34 and E_(NO_(3)^(-)|NO)^(@)=+0.96]

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?

What is the potential of a half-cell consisting of zinc electrode in "0.01 M ZnSO_(4) solution 25^(@)C. E^(@) = 0.763 V.

Explain why the stability of Cu^(+) io in aqueous solution is lower Cu^(2+) ion . E_(Cu^(2+)|Cu)^(@)= +0.34 "V & "E_(Cu^(+)|Cu)^(@)= +0.52 V

A solution of AgNO_3 was stirred with iron rod. Will it cause any change in the concentration of silver and nitrate ions? ( (E^0)_((Fe^(2+))/(Fe)=-0.44V) , ((E^0)_((Ag^+)/(Ag))=0.80V)

Consider the following cell reaction Znabs(Zn^(2+)(1M)) abs(Cd^(+2)(1M))Cd.Give the cell reaction and calculate the standard cell potential. (E^0)_((Zn^(2+))/(Zn)=-0.76V , (E^0)_((Cd^(2+))/(Cd)=0.40V

Calculate the value of the equilibrium constant of the following reaction at 298 K: Given: E_(Cu^(2+)|Cu)^(@)=+0.34V and E_(Cl_(2)|2Cl^(-))^(@)=+1.36V