Question

Consider the redox reaction below.

Upper Z n (s) plus 2 upper H upper C l (a q) right arrow upper Z n upper C l subscript 2 (a q) plus upper H subscript 2 (g 0).


Which half reaction correctly describes the oxidation that is taking place?

Answer 1

B. Upper Z n (s) right arrow upper Z n superscript 2 plus (a q) plus 2 e superscript minus.

Step-by-step explanation:

Answer 2

`Zn^0\rightarrow Zn^(+2)+2e^-`

Step-by-step 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.