The reaction represented by the equation [tex]\( \text{Mg} + \text{ZnCl}_2 \)[/tex] is an example of a single replacement reaction. In this type of reaction, one element replaces another element in a compound.
1. Identify the elements involved: We have magnesium (Mg) and zinc chloride (ZnCl[tex]\(_2\)[/tex]).
2. Determine the type of reaction: Since magnesium is a more reactive metal than zinc, it can replace zinc in zinc chloride. This is because magnesium is higher than zinc in the reactivity series.
3. Predict the products:
- Magnesium (Mg) will replace zinc (Zn) in the compound zinc chloride (ZnCl[tex]\(_2\)[/tex]).
- The zinc will be displaced and come out as a free metal.
- Magnesium will form a new compound with chlorine, which is magnesium chloride (MgCl[tex]\(_2\)[/tex]).
4. Write the chemical equation:
- Reactants: [tex]\( \text{Mg} + \text{ZnCl}_2 \)[/tex]
- Products: [tex]\( \text{MgCl}_2 + \text{Zn} \)[/tex]
Thus, the balanced chemical equation for the reaction is:
[tex]\[ \text{Mg} + \text{ZnCl}_2 \rightarrow \text{MgCl}_2 + \text{Zn} \][/tex]
The most likely result of the reaction between magnesium (Mg) and zinc chloride (ZnCl[tex]\(_2\)[/tex]) is the formation of magnesium chloride (MgCl[tex]\(_2\)[/tex]) and zinc (Zn). Therefore, the correct answer is:
[tex]\[ \text{MgCl}_2 + \text{Zn} \][/tex]
