(a) Standard reduction potentials of zinc and copper electrodes are -0.76 V and 0.34 V respectively.Which electrode will undergo oxidation and which lelctrode reduction?
`(b) Can we store copper suphate in zinc vessel? Give expalnation support of your answer.

The standard reduction potential of Pb and Zn electrodes are -0.126 and -0.763 V respectively. The cell equation will be

The standard electrode potentials of Zn, Ag and Cu are -0.76, 0.80 and 0.34 volt respectively, then:

Standard reduction potential of Au^(3+)//Au and Sn^(4+)//Sn^(2+) electrodes are 1.5 V and 0.15 V respectively. The net reaction is __________.

A cell is prepared by dipping a copper rod in 1 MCuSO_(4) solution and a nickel rod in 1M NiSO_(4) . The standard reduction potentials of copper and nickel electrodes are +0.34 V and -0.25 V respectively. (i) Which electrode will work as anode and which as cathode? (ii) What will be the cell reaction? (iii) How is the cell represented ? (iv) Calculate the EMF of the cell.

A cell is prepared by dipping a copper rod in 1M CuSO_(4) solution and a nickel rod in 1M NiSO_(4) solution. The standard reduction potentials of copper and nickel electrodes are +0.34 V and -0.25 V respectively. (i) Which electrode will work as anode and which as cathode ? (ii) What will be the cell reaction ? (iii) How is the cell represented ? (iv) Calculate the emf of the cell.

Standard reduction electrode potential of Zn^(2+)//Zn is -0.76V . This means: