write balanced half-reactions describing the oxidation and reduction that happen in this reaction 2Fe(s)+3Pb(NO3)2(aq)=3Pb(s)+2Fe(NO3 )3(aq)

Oxidation half-reaction: 2 Fe (s) > 2 Fe³+ (aq) + 6e-

Reduction half-reaction: 3 Pb²+ (aq) + 6 e- > 3 Pb (s)

Explanation:

A redox reaction reaction is one in which oxidation and reduction occur simultaneously and to the same extent.

Oxidation involves a loss of electron, hence, a positive increase in the oxidation number of the atom or ion. The oxidation half-reaction is as follows:

2 Fe (s) > 2 Fe³+ (aq)

The metallic element iron, Fe , having an oxidation number of zero, loses three electrons to form the Fe³+ ion with a charge of +3. Since each atom loses three electrons each, The number of moles of electrons lost is six.

2 Fe (s) > 2 Fe³+ (aq) + 6e-

Reduction involves a gain of electrons, hence, a decrease in the oxidation number of the atom or ion. The reduction half-reaction is given below:

3 Pb²+ (aq) ---> 3 Pb (s)

The lead (ii) ion, Pb²+ having a charge of +2 gains two electrons each to become the neutral metallic lead atom, Pb, with oxidation number of zero. Since 3 moles of Pb²+ are reacting, 6 moles of electrons are gained.

3 Pb²+ (aq) + 6 e- > 3 Pb (s)