Question

Consider the redox reaction below.

Answer 1

Answer:

$Zn^0\rightarrow Zn^{+2}+2e^-$

Explanation:

Hello,

In this case, the described chemical reaction is:

$Zn(s)+HCl(aq)\rightarrow ZnCl_2(aq)+H_2(g)$

Then, to identify the half reactions we must assign the oxidation state for each element as shown below:

$Zn^0(s)+H^+Cl^-(aq)\rightarrow Zn^{+2}Cl_2^-(aq)+H_2^0(g)$

In such a way, we can notice zinc's oxidation state changes from 0 to +2, therefore, it is the oxidizes species for which the half reaction which correctly describes the oxidation that is taking place is:

$Zn^0\rightarrow Zn^{+2}+2e^-$

Best regards.

Answer 2

The answer is A..........