Question

Study this chemical reaction: \[ \mathrm{ZnCl}_{2}(a q)+2 \mathrm{Na}(s) \rightarrow \mathrm{Zn}(s)+2 \mathrm{NaCl}(a q) \] Then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction.

          Study this chemical reaction:
\[
\mathrm{ZnCl}_{2}(a q)+2 \mathrm{Na}(s) \rightarrow \mathrm{Zn}(s)+2 \mathrm{NaCl}(a q)
\]

Then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction.

Study this chemical reaction:

ZnCl2(a q)+2 Na(s) →Zn(s)+2 NaCl(a q)

Then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction.

Added by John Paul O.

General Chemistry

Darrell Ebbing, Steven D. Gammon 9th Edition

Chapter 4

Instant Answer

Solved by Expert Md.Daniyal Arshad

Step 1

In \(\mathrm{ZnCl}_{2}\), zinc (Zn) has an oxidation state of +2, and chlorine (Cl) has an oxidation state of -1. Sodium (Na) is in its elemental form, so its oxidation state is 0. In the products, Zn is in its elemental form, so its oxidation state is 0, and in Show more…

Show all steps