(d) Identify the element which exhibits neither the negative nor does the positive oxidation state. . Chlorine is used to purify drinking water. Excess of chlorine is harmful.
The excess of chlorine is removed by treating with sulphur dioxide. Present a balanced equation for this redox change taking place in water. . Refer to the periodic table given in your book and now answer the following questions: (a) Select the possible non metals that can show disproportionation reaction.
(b) Select three metals that can show disproportionation reaction. . In Ostwald’s process for the manufacture of nitric acid, the first step involves the oxidation of ammonia gas by oxygen gas to give nitric oxide gas and steam. What is the maximum weight of nitric oxide that can be obtained starting only with .
g. of ammonia and . g of oxygen ? .
Using the standard electrode potentials given in the Table . , predict if the reaction between the following is feasible: (a) Fe + (aq) and I – (aq) (b) Ag + (aq) and Cu(s) (c) Fe + (aq) and Cu(s) (d) Ag(s) and Fe + (aq) (e) Br (aq) and Fe + (aq). . Predict the products of electrolysis in each of the following: (i) An aqueous solution of AgNO with silver electrodes (ii) An aqueous solution AgNO with platinum electrodes (iii) A dilute solution of H SO with platinum electrodes (iv) An aqueous solution of CuCl with platinum electrodes.
. Arrange the following metals in the order in which they displace each other from the solution of their salts. Al, Cu, Fe, Mg and Zn. .
Given the standard electrode potentials, K + /K = – .93V, Ag + /Ag = .80V, Hg + /Hg = .79V Mg + /Mg = – .37V. Cr + /Cr = – .74V arrange these metals in their increasing order of reducing power. . Depict the galvanic cell in which the reaction Zn(s) + 2Ag + (aq) → Zn + (aq) +2Ag(s) takes place, Further show: (i) which of the electrode is negatively charged, (ii) the carriers of