Question

Question 8.17 Consider the reactions:

(a) H3PO2(aq) + 4 AgNO3(aq) + 2 H2O(l)→H3PO4(aq) + 4Ag(s) + 4HNO3(aq)

(b) H3PO2(aq) + 2CuSO4(aq) + 2 H2O(l)→H3PO4(aq) + 2Cu(s) + H2SO4(aq)

(c) C6H5CHO(l) + 2[Ag (NH3)2]+(aq) + 3OH–(aq)→C6H5COO–(aq) + 2Ag(s) + 4NH3 (aq) + 2 H2O(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?

Class XI Redox Reactions Page 273

Answer 1

Hi

Please see the attached file !

Hope it helps you !

Answer 2

in reaction (a), we see that oxidation number of Ag is decreases from +1 to zero and oxidation number of P increases from +1 to +5. hence, AgNO3 act as oxidising agent.

similarly , in reaction (b), we see that oxidation number of Cu is decreases from +2 to zero and oxidation number of P increases from +1 to +5 . hence, CuSO4 acts as oxidising agent.

in reaction (c), [Ag(NH3)2]^+ oxidises benzaldehyde to Benzoic acid but in reaction (d), Cu2+ do not oxidise benzaldehyde to Benzoic acid .{ because reaction is unchanged}
This indicates that Ag^+ is a stronger oxidizing agent than Cu2+ .