What is the oxidation half-reaction for Mg(s) + ZnCl2(aq) MgCl2(aq) + Zn(s)?
A. Zn(s) Zn2+ + 2e-
B. Zn2+ + 2e- Zn(s)
C. Mg(s) Mg2+ + 2e-
D. Mg2+ + 2e- Mg(s)
To determine the oxidation half-reaction for the given chemical equation Mg(s) + ZnCl2(aq) -> MgCl2(aq) + Zn(s), we need to identify the element that is being oxidized.
In this case, the element that is being oxidized is magnesium (Mg), as it is going from its elemental state (Mg(s)) to its ionic state (Mg2+).
Therefore, the correct oxidation half-reaction is:
C. Mg(s) -> Mg2+ + 2e-
To determine the oxidation half-reaction for the given chemical equation, we need to identify the element that is being oxidized.
In this case, magnesium (Mg) is being oxidized as it goes from its elemental state (Mg(s)) to Mg2+ in solution (Mg2+ + 2e-). The half-reaction for this oxidation process is:
C. Mg(s) → Mg2+ + 2e-
Therefore, option C. Mg(s) → Mg2+ + 2e- is the correct oxidation half-reaction for the given equation.
The half cells are
Mg ==> Mg^2+ + 2e
Zn^2+ + 2e ==> Zn
Oxidation is the loss of electrons.