Question

Consider the following redox reaction: 2Ag+(aq) + Zn(s) --> Zn^2+ (s) + 2Ag(s)Which of the following statements are TRUE? (Select All That Apply)a) Ag+ is the oxidizing agentb) Ag+ is reduced to Agc) Zn oxidize to Zn^2+d) Zn is the reducing agente) Zn reduce to Zn^2+d) Ag+ oxidize to Zn^2+

Answer 1

Ag+ is the oxidizing agent

Ag+ is reduced to Ag

Zn is oxidized to zn^2+

Zn is the reducing agent

option ABCD

Explanation:

Given information

`2Ag^+_((aq))+Zn_{(s)\text{ }\rightarrow\text{ }}Zn^(2+)_((s))+2Ag_((s))`

From the above redox reaction, you will see that there is a change in the oxidation number of zinc and silver.

Zn goes from 0 to 2+ in its oxidation state

Hence, zinc has been oxidized, therefore, it is a reducing agent

Ag goes from +1 to 0 in its oxidation state

Hence, Ag has been reduced, therefore, it is an oxidizing agent