Question

Half-reaction	E° (V)
Hg2+(aq) + 2e- -----> Hg(l)	0.855V
Ni2+(aq) + 2e- -----> Ni(s)	-0.250V
Zn2+(aq) + 2e- ----->  Zn(s)	-0.763V

(1) The weakest oxidizing agent is: ___

enter formula

(2) The strongest reducing agent is:

___

(3) The strongest oxidizing agent is:___

(4) The weakest reducing agent is: ___

(5) Will Zn(s) reduce Hg²⁺(aq) to Hg(l)? _____(yes)(no)

(6) Which species can be oxidized by Ni2+(aq)? ___ If none, leave box blank.

Answer 1

A species having the most positive reduction potential has the most tendency to get itself reduced and is a good oxidising agent. A species with the most negative reduction potential has the least tendency to itself get reduced and is a good reducing agent. So we can see that the conversion of Hg^{​​​​​2+}(aq) to Hg(l) has the maximum reduction potential (0.855 V) so Hg^{​​​​​2+} is the strongest oxidising agent (3) and weakest reducing agent (4). The conversion of Zn^{​​​​​2+}(aq) to Zn (s) has the least reduction potential (-0.763 V) so Zn^{​​​​​2+} is the strongest reducing agent (2) and weakest oxidising agent (1).

5) As Zn^{​​​​​2+} is the strongest reducing agent (as it has least reduction potential) from the given options so yes it can reduce Hg^{​​​​​2+} (as it has the maximum reduction potential among given options)

(6) As the conversion of Ni^{​​​​​2+}(aq) to Ni(s) has reduction potential more than that of conversion of Zn^{​​​​​2+}(aq) to Zn (s) but less than that of the conversion of Hg^{​​​​​2+}(aq) to Hg(l), so Ni²⁺(aq) has tendency to oxidise Zn(s) to Zn^{​​​​​2+}(aq) and in the process it will itself get reduced to Ni(s).