Why blue colour of `CuSO_(4)` solution gets discharged when zinc rod is dipped in it ? Given, `E_(Cu^(+2)//Cu)^(@)=0.34 V and E_(Zn^(+2)//Zn)^(@)=-0.76V`

Blue colour of CuSO_(4) solution is discharge slowly when an iron rod is dipped into it. Why?

For the given cell arrangement identify incorrect statement given E^@_(Cu^(2+)//Cu) = 0.34V & E^@_(Zn^(2+)//Zn) = -0.76V

Can a solution of 1 M ZnSO_(4) be stored in a vessel made of copper ? Given that E_(Zn^(+2)//Zn)^(@) =-0.76V and E_(Cu^(+2)//Cu)^(@)=0.34 V

E_(Cu^(2+)//Cu)^(@)=0.34V E_(Cu^(+)//Cu)^(@)=0.522V E_(Cu^(2+)//Cu^(+))^(@)=

E_(Cu^(2+)//Cu)^(@)=0.34V E_(Cu^(+)//Cu)^(@)=0.522V E_(Cu^(2+)//Cu^(+))^(@)=

E_(Cu^(2+)//Cu)^(@) =0.43V E_(Cu^(+)//Cu)^(@)=0.55V E_(Cu^(2+)//Cu^(+))^(@) =

A cell is constructed by dipping a zinc rod in 0.1 M zinc nitrate solution and a lead rod in 0.2 M lead nitrate solution. E_(Pb^(2+)//Pb)^(Theta) = -0.13 V and E_(Zn^(2+)//Zn)^(Theta) = -0.76V (i) Write the spontaneous cell reaction. (ii) Calculate standard emf and emf of the cell.

Which of the following statements is correct? If E_(Cu^(2+)|Cu)^(@)=0.34V, E_(Sn^(2+)|Sn)^(@)=-0.136V,E_(H^+|H_2)^(@)=-0.0V

What does the negative sign in the expression E_(Zn^(2+)//Zn)^(@)=-0.76V mean?

If a small Cu rod is placed in an aqueous solution of ferrous salt, then which of the following will be observed? ( E_((Cu^(2+)) /(Cu))^0 = -0.34 V , E_((Fe^(2+)) /(Fe))^0 = -0.44 V )