Justify that the following reactions are redox reactions: (b) $Fe_2O_3(s) + 3CO(g) \rightarrow 2Fe(s) + 3CO_2(g)$

Depict the galvanic cell in which the reaction $Zn(s) + 2Ag^+(aq) \rightarrow Zn^{2+}(aq) + 2Ag(s)$ takes place, Further show: (ii) the carriers of the current in the cell, and

Using the standard electrode potentials given in the Table 8.1, predict if the reaction between the following is feasible: (a) $Fe^{3+}(aq)$ and $I^-(aq)$

Depict the galvanic cell in which the reaction $Zn(s) + 2Ag^+(aq) \rightarrow Zn^{2+}(aq) + 2Ag(s)$ takes place, Further show: (iii) individual reaction at each electrode.

Balance the following equations in basic medium by ion-electron method and oxidation number methods and identify the oxidising agent and the reducing agent. (c) $Cl_2O_7(g) + H_2O_2(aq) \rightarrow ClO_2^-(aq) + O_2(g) + H^+$

How do you count for the following observations ? (b) When concentrated sulphuric acid is added to an inorganic mixture containing chloride, we get colourless pungent smelling gas HCl, but if the mixture contains bromide then we get red vapour of bromine. Why ?

Identify the substance oxidised reduced, oxidising agent and reducing agent for each of the following reactions: (a) $2AgBr(s) + C_6H_6O_2(aq) \rightarrow 2Ag(s) + 2HBr(aq) + C_6H_4O_2(aq)$

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

Using the standard electrode potentials given in the Table 8.1, predict if the reaction between the following is feasible: (c) $Fe^{3+}(aq)$ and $Cu(s)$

What sorts of informations can you draw from the following reaction ? $(CN)_2(g) + 2OH^-(aq) \rightarrow CN^-(aq) + CNO^-(aq) + H_2O(l)$

Assign oxidation number to the underlined elements in each of the following species: (e) $CaO_2$

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

Why does the following reaction occur ? $XeO_6^{4-}(aq) + 2F^-(aq) + 6H^+(aq) \rightarrow XeO_3(g) + F_2(g) + 3H_2O(l)$. What conclusion about the compound $Na_4XeO_6$ (of which $XeO_6^{4-}$ is a part) can be drawn from 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) $P_4(s) + OH^-(aq) \rightarrow PH_3(g) + HPO_2^-(aq)$

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

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

Balance the following equations in basic medium by ion-electron method and oxidation number methods and identify the oxidising agent and the reducing agent. (b) $N_2H_4(l) + ClO_3^-(aq) \rightarrow NO(g) + Cl^-(g)$

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

Consider the reactions: (a) $H_3PO_2(aq) + 4AgNO_3(aq) + 2H_2O(l) \rightarrow H_3PO_4(aq) + 4Ag(s) + 4HNO_3(aq)$ (b) $H_3PO_2(aq) + 2CuSO_4(aq) + 2H_2O(l) \rightarrow H_3PO_4(aq) + 2Cu(s) + H_2SO_4(aq)$ (c) $C_6H_5CHO(l) + 2[Ag(NH_3)_2]^+(aq) + 3OH^-(aq) \rightarrow C_6H_5COO^-(aq) + 2Ag(s) + 4NH_3(aq) + 2H_2O(l)$ (d) $C_6H_5CHO(l) + 2Cu^{2+}(aq) + 5OH^-(aq) \rightarrow$ No change observed. What inference do you draw about the behaviour of $Ag^+$ and $Cu^{2+}$ from these reactions ?

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