The reaction of copper and silver nitrate is spontaneous. Cu(s) + 2AgNO_3(aq) ri

Question

The reaction of copper and silver nitrate is spontaneous. Cu(s) + 2AgNO_3(aq) rightarrow Cu(NO_3)_2 (aq) + 2Ag(s) The reverse reaction, in which silver metal is placed in the copper nitrate solution, is not spontaneous. Which statement best describes the oxidizing and reducing abilities of the reactants? Select one: a. Silver is a better oxidizing agent than copper. b. Copper is a better reducing agent than silver. c. Silver ion (Ag*) is a stronger oxidizing agent than copper ion (Cu*) and copper metal is a stronger reducing agent than silver. d. Copper is a better oxidizing agent than silver and silver is a better reducing agent than copper.

Explanation / Answer

In the forward reaction, Cu(0) is oxidized to Cu(+2) in Cu(NO3)2 and Ag(+1) in AgNO3 is reduced to Ag(0). Hence, Cu metal i.e Cu(0) acts as the reducing agent in the forward reaction which is spontaneous alongside Ag(+1) acts as the oxidizing agent. In the reverse, non-spontaneous reaction, Cu(+2) is reduced to Cu(0) by Ag metal i.e. Ag(0), hence Ag should act as the reducing agent in the reverse reaction and Cu(+2) acts as the oxidizing agent to oxidize Ag(0) to Ag(+1). But the reverse reaction being non-spontanenous, Ag metal as the reducing agent and Cu(+2) as the oxidizing agent must be weak enough not to promote the backward reaction. Hence, the third option i.e. option C. saying Silver ion (Ag+) is stronger oxidizing agent than Cu2+ and Cu metal i.e. Cu(0) is a stronger reducing agent than Ag metal i.e. Ag(0).

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