Respuesta :
Answer:
6
Explanation:
Oxidation reaction is defined as the chemical reaction in which an atom looses its electrons. The oxidation number of the atom gets increased during this reaction.
[tex]X\rightarrow X^{n+}+ne^-[/tex]
Reduction reaction is defined as the chemical reaction in which an atom gains electrons. The oxidation number of the atom gets reduced during this reaction.
[tex]X^{n+}+ne^-\rightarrow X[/tex]
For the given chemical reaction:
[tex]Mg(s)+Al^{3+}(aq.)\rightarrow Al(s)+Mg^{2+}(s)[/tex]
The half cell reactions for the above reaction follows:
Oxidation half reaction: [tex]Mg\rightarrow Mg^{2+}+2e^-[/tex]
Reduction half reaction: [tex]Al^{3+}+3e^-\rightarrow Al[/tex]
Magnesium is loosing 2 electrons to form the magnesium cation. Thus, it is getting oxidized. Aluminum anion is gaining 3 electrons to form Aluminum. Thus, it is getting reduced.
Thus, balancing the half-reactions as:-
Oxidation half reaction: [tex]3Mg\rightarrow 3Mg^{2+}+6e^-[/tex]
Reduction half reaction: [tex]2Al^{3+}+6e^-\rightarrow 2Al[/tex]
Thus, total number of electrons transferred = 6
Answer:
3Mg +2Al^3 ⇆ 3 Mg^2+ + 2Al
In this reaction 6 electrons are transferred
Explanation:
Step 1: The half reactions
Mg -2e- ⇆ Mg^2+
Al^3+ +3e- ⇆ Al
Step 2: Balance both equations
3*(Mg -2e- ⇆ Mg^2+)
2(Al^3+ +3e- ⇆ Al)
3Mg -6e- ⇆ 3Mg^2+
2Al^3+ +6e- ⇆ 2Al
Step 3: The netto reaction
3Mg +2Al^3 ⇆ 3 Mg^2+ + 2Al
In this reaction 6 electrons are transferred
