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 ?
(a) Ag ions are reduced to Ag which is precipitated.
(b)Â Cu2+Â (aq) are reduced to Cu which is precipitated.
(c)Â Ag+Â (aq) present in the complex are reduced to Ag which gets precipitated as shining mirror.
(d)Â Cu2+Â (aq) ions are not reduced by C6H5CHO (benzaldehyde) which is a very weak reducing agent.
Therefore from the above reactions, we conclude that Ag+Â ion is a stronger oxidising agent than Cu2+Â ions.
Long Answer TypeDiscuss briefly the types of redox reactions. Give examples.Â
or
Discuss the following redox reactions.
(a)Â Combination reactions
(b)Â Decomposition reactions
(c)Â Displacement reactions
(d)Â 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)Â Select the possible non-metals that can show disproportionation reaction.
(b)Â 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)
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