Predict the products of electrolysis in each of the following: (i) An aqueous solution of $AgNO_3$ with silver electrodes

Write formulas for the following compounds: (b) Nickel(II) sulphate

Assign oxidation number to the underlined elements in each of the following species: (d) $K_2MnO_4$

How do you count for the following observations ? (a) Though alkaline potassium permanganate and acidic potassium permanganate both are used as oxidants, yet in the manufacture of benzoic acid from toluene we use alcoholic potassium permanganate as an oxidant. Why ? Write a balanced redox equation for the reaction.

Balance the following equations in basic medium by ion-electron method and oxidation number methods and identify the oxidising agent and the reducing agent. (a) $P_4(s) + OH^-(aq) \rightarrow PH_3(g) + HPO_2^-(aq)$

What are the oxidation number of the underlined elements in each of the following and how do you rationalise your results ? (d) $CH_3CH_2OH$

Refer to the periodic table given in your book and now answer the following questions: (b) Select three metals that can show disproportionation reaction.

Balance the following redox reactions by ion – electron method : (d) $Cr_2O_7^{2-} + SO_2(g) \rightarrow Cr^{3+}(aq) + SO_4^{2-}(aq)$ (in acidic solution)

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.

What are the oxidation number of the underlined elements in each of the following and how do you rationalise your results ? (c) $Fe_3O_4$

Write formulas for the following compounds: (c) Tin(IV) oxide

Assign oxidation number to the underlined elements in each of the following species: (f) $NaBH_4$

Consider the elements : $Cs$, $Ne$, $I$ and $F$. (b) Identify the element that exhibits only postive oxidation state.

What are the oxidation number of the underlined elements in each of the following and how do you rationalise your results ? (e) $CH_3COOH$

Using the standard electrode potentials given in the Table 8.1, predict if the reaction between the following is feasible: (e) $Br_2(aq)$ and $Fe^{2+}(aq)$.

Assign oxidation number to the underlined elements in each of the following species: (g) $H_2S_2O_7$

Write formulas for the following compounds: (d) Thallium(I) sulphate

The compound $AgF_2$ is unstable compound. However, if formed, the compound acts as a very strong oxidising agent. Why ?

Assign oxidation number to the underlined elements in each of the following species: (h) $KAl(SO_4)_2.12H_2O$

Identify the substance oxidised reduced, oxidising agent and reducing agent for each of the following reactions: (d) $N_2H_4(l) + 2H_2O_2(l) \rightarrow N_2(g) + 4H_2O(l)$