`E^@` (standard electrode potential) values generally become less negative as we move across a transition series. But `E^@`values of `Ni^2//Ni` and `Zn^(2+)//Zn` are exceptions. Justify.

Using the standard electrode potentials given in the text (Table 8.1), predict if the reaction between the following is feasible? a) 'F e^(3+)(a q)' and 'I^-(a q)' b) 'Ag^+(aq)' and 'Cu(s)' c) 'Fe^(3+)(aq)' and 'Cu(s)' d) 'A g(s)' and 'F e^(3+)(a q)' e) 'Br_2(aq)' and 'Fe^(2+)(aq)'

The Standard electrode potentials of some electrodes are given below: E^@_(Zn^(2+)Zn) = -0.76 V, E^@(Cu^(2+)Cu) =+0.34, E^@_(Ag, Ag) = + 0.80V, E^@_(H, H_2)=0V What is the reaction taking place at SHE when it is connected to Ag/Ag^+. Electrode to form a galvanic cell?

The cell reaction in Daniell cell is Zn(s) + Cu^(2+) (aq) to Zn^(2+)(aq) + Cu(s) and Nernst equation for single electrode potential for general electrode reaction M^+ (aq) + n e^(-) to M(s) is E_(M^(n+)//M)=E_(M^(n+)//M)^@- (2.303 RT)/(nF) log [[M]]/[[M^(n+)]] Derive Nernst equation for Daniell cell

A solution of Ni(NO_3)_2 is electrolysed between platinam electrodes using a current of 5 am^- peres for 20 minutes. What mass of N i is d e posited at the cathode?