Short Answer TypeConsider the reactions:
(a) H3PO2(aq) + 4 AgNO3(aq) + 2 H2O(l) → H3PO4(aq) + 4Ag(s) + 4HNO3(aq)
(b) H3PO2(aq) + 2CuSO4(aq) + 2H2O(l) → H3PO4(aq) + 2Cu(s) + H2SO4(aq)
(c) C6H5CHO(l) + 2[Ag (NH3)2]+(aq) + 3OH–(aq) → C6H5COO–(aq)+ 2Ag(s) +4NH3 (aq) + 2H2O(l)
(d) C6H5CHO(l) + 2Cu2+(aq) + 5OH–(aq) → No change observed.
What inference do you draw about the behaviour of Ag+ and Cu2+ from these reactions ?
Long Answer TypeDiscuss briefly the types of redox reactions. Give examples.
or
Discuss the following redox reactions.
(a) Combination reactions
(b) Decomposition reactions
(c) Displacement reactions
(d) Disproportionation reactions.
Give one example in each case.
Suggest a scheme of classification of the following redox reactions:
(a) N2(g) + O2(g) → 2 NO (g)
(b) 2Pb(NO3)2(s) → 2PbO(s) + 2 NO2 (g) + ½ O2 (g)
(c) NaH(s) + H2O(l) → NaOH(aq) + H2 (g)
(d)2NO2(g) + 2OH–(aq) → NO2-(aq) +NO3–(aq)+H2O(l)
Short Answer TypeRefer to the periodic table given in your book and now answer the following questions:
(a) Select the possible non-metals that can show disproportionation reaction.
(b) Select three metals that can show disproportionation reaction.
Long Answer TypeShort Answer TypeWhat sorts of informations can you draw from the following reaction?
(CN)2(g) + 2OH– (aq) → CN–(aq) + CNO–(aq) + H2O(l)
Suggest a scheme of classification of the given redox reactions,
N2 (g) + O2 (g) 
2NO (g)
The oxidation number of carbon in (CN)2, CN- and CNO- are +3, +2 and +4 respectively. These are obtained as shown below:
(CN)2: Let the oxidation number of C =x
2(x-3) =0
X= 3
CN-
x-3= -1
x=2
CNO-
X-3-2 =-1
X= 4
(i) The reaction involves the decomposition of cyanogen (CN)2 in alkaline medium.
(ii) Both (CN)2 (i.e. cyanogen) and CN- (i.e., cyanide ions) are pseudo halogens in nature i.e. both behave like halogens in characteristics.
(iii) Cyanogen undergoes disproportionation in the reaction.
(iv) It is an example of a redox reaction.
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