The reaction of copper and silver nitrate is spontaneous. Cu( s ) + 2AgNO 3 ( aq

Question

The reaction of copper and silver nitrate is spontaneous.

Cu(s) + 2AgNO3(aq) ?
Cu(NO3?)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?

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 (Cu2+?) 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

The oxidation number of Cu changes from 0 to +2 thus getting oxidised, while the oxidation number of Ag changes from +2 to zero, thus getting reduced in the above given reaction.

The substance which is oxidised is known as the reducing agent while the one getting reduced is known as the oxidising agent.

In our first case, Ag is the oxidising agent, while Cu is the reducing agent.

However, in the reverse reaction, when the roles of Cu and Ag are reversed, the reaction is not spontaneous. This means that when Ag is the reducing agent, it is not that effective than when Cu is the reducing agent.

Thus, the correct answer is: B) Copper is a better reducing agent than silver.

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