Question

Consider the reaction below.

Upper Z n (s) plus upper C u superscript 2 plus (a q) right arrow upper Z n superscript 2 plus (a q) plus upper C u (s).

Which half reaction correctly describes the oxidation that is taking place?
Z n (s) right arrow upper Z n superscript 2 plus (a q) plus e superscript minus.
Upper Z n (s) right arrow upper Z n superscript 2 plus (a q) plus 2 e superscript minus.
Upper C u superscript 2 plus (a q) plus 2 e superscript minus right arrow upper C u (s).
Upper C u superscript 2 plus (a q) plus e superscript minus right arrow upper C u (s).

Answer 1

The oxidation half-reaction in the provided chemical reaction is: Zn(s) → Zn²+(aq) + 2e⁻. This shows the zinc atom being oxidized by losing two electrons to become a zinc ion with a charge of 2+.

Step-by-step explanation:

In the given reaction, zinc is being oxidized to zinc ions. The oxidation half-reaction that correctly describes this process is:

Zn(s) → Zn²+(aq) + 2e⁻

This half reaction is balanced in terms of the number of zinc atoms, and it also shows the two electrons that are produced. These two electrons account for the zinc atom losing two negative charges to become a zinc ion with a 2+ charge. In this reaction, zinc serves as the reducing agent because it is losing electrons, which is evidenced by the presence of two electrons on the product side of the oxidation half reaction.

Answer 2

The answer is B. ) Zn(s) ------> Zn²±(aq) + 2e-

Step-by-step explanation: