Using the standard electrode potentials given in the Table 8.1, predict if the reaction between the following is feasible: (b) $Ag^+(aq)$ and $Cu(s)$

Predict the products of electrolysis in each of the following: (iii) A dilute solution of $H_2SO_4$ with platinum electrodes

Justify that the following reactions are redox reactions: (c) $4BCl_3(g) + 3LiAlH_4(s) \rightarrow 2B_2H_6(g) + 3LiCl(s) + 3AlCl_3(s)$

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

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 $I^-(aq)$

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

Consider the elements : $Cs$, $Ne$, $I$ and $F$. (d) Identify the element which exhibits neither the negative nor does the positive oxidation state.

Arrange the following metals in the order in which they displace each other from the solution of their salts. $Al$, $Cu$, $Fe$, $Mg$ and $Zn$.

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 ?

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) $Cl_2O_7(g) + H_2O_2(aq) \rightarrow ClO_2^-(aq) + O_2(g) + H^+$

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 ?

What are the oxidation number of the underlined elements in each of the following and how do you rationalise your results ? (a) $KI_3$

Consider the elements : $Cs$, $Ne$, $I$ and $F$. (c) Identify the element that exhibits both positive and negative oxidation states.

Assign oxidation number to the underlined elements in each of the following species: (b) $NaHSO_4$

Justify that the following reactions are redox reactions: (a) $CuO(s) + H_2(g) \rightarrow Cu(s) + H_2O(g)$

Write formulas for the following compounds: (f) Chromium(III) oxide

Predict the products of electrolysis in each of the following: (iv) An aqueous solution of $CuCl_2$ with platinum electrodes.

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

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.