Suggest a list of the substances where carbon can exhibit oxidation states from –4 to +4 and nitrogen from –3 to +5.

3

(a)

Write formulas for the following compounds:
(a) Mercury(II) chloride
(b) Nickel(II) sulphate
(c) Tin(IV) oxide
(d) Thallium(I) sulphate
(e) Iron(III) sulphate
(f) Chromium(III) oxide

3

(a)

Whenever a reaction between an oxidising agent and a reducing agent is carried out, a compound of lower oxidation state is formed if the reducing agent is in excess and a compound of higher oxidation state is formed if the oxidising agent is in excess. Justify this statement giving three illustrations.

3

(a)

Refer to the periodic table given in your book and now answer the following question: Select three metals that show disproportionation reaction.

3

(a)

(a) Give two important functions of salt bridge.
(b) Balance the following equation by oxidation number method
Fe²⁺ + Cr₂\({ O }_{ 7 }^{ 2- }\) + H⁺ \(\rightarrow\) Fe³⁺ + Cr³⁺ + H₂O

3

(a)

Identify the oxidant and reductant in the following redox reaction: 
2K₂MnO₄ + Cl₂ \(\rightarrow\) 2kcl + 2KMnO₄

3

(a)

Identify the substance oxidised, reduced, oxidising agent and reducing agent for each of the following reactions
(a) 2AgBr(s) + C₆H₆O₂(aq) \(\rightarrow\) 2Ag(s) + 2HBr(aq) + C₆H₄O₂(aq)
(b) HCHO(l) + 2[Ag(NH₃)₂]⁺ (aq) + 3OH^-(aq) \(\rightarrow\) Ag(s) + HCOO^-(aq) + 4NH₃aq) + 2H₂O(l)
(c) N₂H₄(l) + 2H₂O₂ \(\rightarrow\) N₂(g)) + 4H₂O(l)

3

(a)

Calculate the oxidation number of  (i) C in CH₃COOH (ii) S in \({ S }_{ 2 }{ O }_{ 2 }^{ -2 }\)

3

(a)

Give one example of disproportionation reaction.

3

(a)

Account for the following
(a) HNO₃ acts only as an oxidising agent while HNO₂ can act both as reducing and oxidising agent.
(b) ClO₄ - does not show disproportionation reaction.
(c) Ozone acts as an oxidising agent

3

(a)

Using the standard electrode potentials given in the predict if the reaction between the following is feasible. Fe³⁺(aq)and Cu(s)

3

(a)

Using the standard electrode potentials given in the Table B.l, predict if the reaction between the following is feasible - Ag(s) and Fe³⁺(aq)

3

(a)

Using the standard electrode potentials given in the Table B.l, predict if the reaction between the following is feasible - Br₂ (aq) and Fe²⁺(aq)

3

(a)