The statement for the overall equation by considering half reactions for this chemical reaction "Upper M g (s) plus 2 upper H superscript plus (a q) right arrow upper M g superscript 2 plus (a q) plus upper H subscript 2 (g)."
A redox reaction's half reaction is either the oxidation or reduction reaction aspect. Redox reactions can be balanced using the half-reaction method. It entails decomposing the total equation into an oxidation and a reduction component.
The reactions take place in an electrochemical cell, where electrons are lost at the anode via oxidation and consumed at the cathode via reduction.
In the given equation, at the Mg anode, oxidation takes place which shows that the metal loses electrons. This is represented in the following oxidation half-reaction:
Mg → [tex]Mg^{2+} \;+\;2e^{-}[/tex]
Reduction half-reaction which involves in the gain of electrons:
[tex]2H^{+} \;+\;2e^{-}[/tex] → H2
The overall equation comes out to be,
[tex]Mg\;+\;H^{2+}[/tex] → [tex]Mg^{2+} \;+\;H2[/tex]
Hence the correct answer is upper M g (s) plus 2 upper H superscript plus (a q) right arrow upper M g superscript 2 plus (a q) plus upper H subscript 2 (g).
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