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

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.

Why is the value of E_(Cu^(2+)|Cu)^(0)(+0.34V) positive ?

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

Using the data find out the strongest reducing agent - E_(Cr_(2)O_(7)^(2-)|Cr^(+))^(@)=+1.33V, E_(Cl_(2)|Cl^(-))^(@)=+1.36V E_(MnO_(4)^(-)|Mn^(2+))^(@)=+1.51V, E_(Cr^(2+)|Cr)^(@)=-0.74V

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

Arrange K^(+), Zn^(2+), H^(+), Cu^(2+) ions in order of their tendency to be liberated at cathode. [E_(cu^(2+)|Cu)^(@)=+0.34V, E_(2H^(+)|H_(2))^(@)=0.00V , E_(Zn^(2+)|Zn)^(@)=-0.76V E_(K^(+)|K)^(@)=-2.93V]

Consider the galvanic cell Cu|Cu^(2+)(0.13M)||Ag^(+)(0.01M)|Ag (i) Calculate the reduction potential of each electrode and EMF of the cell (ii) Is is reaction representing the cell spontaneous ? ["Given : "E_(Cu^(2+)|Cu)^(@)=+0.34V and E_(Ag^(+)|Ag)^(@)=+0.80V]

An aqueous solution containing Cu^(2+), Hg_(2)^(2+) and Ag^(+) ions, each with a concentration of 1M, is being electrolysed by using Pt - electrodes. If the voltage between the electrodes is increased gradually, which one of these ions will be deposited first and which one will be deposited last at the cathode? E_(Ag^(+)|Ag)^(@)=0.8V, E_(Cu^(+)|Cu)^(@)=0.34V & E_(Hg^(+)|2Hg)^(@)=0.79

Which among the following vessels is used to store CuSO_(4) solution ? a Ag vessel [ Given E_(Zn^(2+)|Zn)^(0)=-0.76V, E_(Cu^(2+)|Cu)^(0)=+0.34V and E_(Ag^(+)|Ag)^(0)=0.80V ]