Redox Reactions

How many of these compounds will undergo disproportionation on hydrolysis? CO?, NO?, Cl?, F?, ClO?, Cl?O?, N?O?, SO?, P?O?

At $20.0\mathrm{m}\mathrm{L}$ solution containing $0.2\mathrm{g}$ impure ${\mathrm{H}}_2{\mathrm{O}}_2$ reacts completely with $0.316\mathrm{g}$ of ${\mathrm{K}\mathrm{M}\mathrm{n}\mathrm{O}}_4$ in acid solution. The purity of ${\mathrm{H}}_2{\mathrm{O}}_2$ (in %) is (mol. wt. of ${\mathrm{H}}_2{\mathrm{O}}_2=34$ ; mol. wt. of ${\mathrm{K}\mathrm{M}\mathrm{n}\mathrm{O}}_4=158$ ) 

On heating, lead (II) nitrate gives a brown gas (A). The gas (A) on cooling changes to a colourless solid/liquid (B). (B) on heating with NO changes to a blue solid (C). The oxidation number of nitrogen in solid $\left(C\right)$ is:

Consider the following equations :

$2{\mathrm{F}\mathrm{e}}^{2+}+{\mathrm{H}}_2{\mathrm{O}}_2\to \mathrm{x}\mathrm{A}+\mathrm{y}\mathrm{B}$ (in basic medium)

(in acidic medium)

$2{\mathrm{M}\mathrm{n}\mathrm{O}}_4^{-}+6{\mathrm{H}}^{+}+5{\mathrm{H}}_2{\mathrm{O}}_2\to {\mathrm{x}}^{\mathrm{\text{'}}}\mathrm{C}+{\mathrm{y}}^{\mathrm{\text{'}}}\mathrm{D}+{\mathrm{z}}^{\mathrm{\text{'}}}\mathrm{E}$

(in acidic medium)

The sum of the stoichiometric coefficients $x,y,x^{\mathrm{\text{'}}},y^{\mathrm{\text{'}}}$ and $z^{\mathrm{\text{'}}}$ for products $A,B,C,D$ and $E$ , respectively, is

40. Best reducing agent is:
(a) He              (b) Be           (c) Li            (d) Al

37. Which element is considered to have oxidation number of +3 in all its compounds?

(a) Be              (b) Li             (c) Al         (d) Sc

36. Oxidation number ofS in S₂O₈^-2 is

(a) -2           (b) -6           (c) +2          (d) +6

36. Oxidation number ofS in S₂O₈^-2 is

32. Assertion: Na⁺ ion has an oxidation number of +1, Mg²⁺ ion, +2, Fe³⁺ ion, +3, Cl^– ion, –1, O^2– ion, –2; and so on.

Reason: For ions composed of only one atom, the oxidation number is equal to the charge on the ion.

Dinitrogen and dioxygen are main constituents of air, but these do not react with each other to form oxides of nitrogen because _________. 
(i) The reaction is endothermic and requires very high temperatures. 
(ii) The reaction can be initiated only in presence of a catalyst. 
(iii) Oxides of nitrogen are unstable. 
(iv) N₂ and O₂ are unreactive.