How can  you increase the reduction potential of an electrode.

Using the standard electrode potentials given in the Table 8.1, predict if the
reaction between the following is feasible:
(a) Fe³⁺ (aq) and  I^- (aq)
(b) Ag⁺(aq) and Cu(s)
(c) Fe³⁺(aq) and Cu(s)
(d) Ag(s) and Fe³⁺(aq)
(e) Br₂(aq) and Fe²⁺(aq)

Predict the products of electrolysis in each of the following:

(i) An aqueous solution of AgNO₃ with silver electrodes. 

ii)An aqueous solution AgNO₃ with platinum electrodes. 

iii) A dilute solution of H₂SO₄ with platinum electrodes.

iv) An aqueous solution of CuCl₂ with platinum electrodes. 

Depict the galvanic cell in which the reaction Zn(s) + 2Ag⁺ (aq) → Zn²⁺(aq) +2Ag(s)
takes place, Further show:
(i) which of the electrode is negatively charged,
(ii) the carriers of the current in the cell, and
(iii) individual reaction at each electrode.

Consider the following reaction,


The values of x,y and z in the reaction are respectively

• 5,2 and 16

• 2,5 and 8

• 2,5 and 16

• 2,5 and 16

180.

Which of the following chemical reactions depicts the oxidizing behaviour of H₂SO₄?

• 2HI+ H₂SO₄ →I₂ +SO₂+2HO

• Ca(OH)₂ +H₂SO₄ → CaSO₄ +2H₂O

• NaCl +H₂SO₄ → NaHSO₄ + HCl

• NaCl +H₂SO₄ → NaHSO₄ + HCl