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Which reaction will most likely take place based on the activity series?

[tex]\[
Li \ \textgreater \ K \ \textgreater \ Ba \ \textgreater \ Ca \ \textgreater \ Na \ \textgreater \ Mn \ \textgreater \ Zn \ \textgreater \ Cr \ \textgreater \ Fe \ \textgreater \ Cd \ \textgreater \ Ni \ \textgreater \ H \ \textgreater \ Sb \ \textgreater \ Cu \ \textgreater \ Ag \ \textgreater \ Pd \ \textgreater \ Hg \ \textgreater \ Pt
\][/tex]

A. [tex]\(\text{Pt} + \text{FeCl}_3\)[/tex]

B. [tex]\(\text{Mn} + \text{CaO}\)[/tex]

C. [tex]\(\text{Li} + \text{ZnCO}_3\)[/tex]

D. [tex]\(\text{Cu} + 2\text{KNO}_3\)[/tex]

Sagot :

GinnyAnswer
When analyzing chemical reactions using the activity series, the key idea is that a more reactive metal can replace a less reactive metal in a compound. Here, I will go through each given reaction and determine whether it can occur based on the provided activity series:

1. Reaction: Pt + FeCl3

- Activity Series Position: Pt (Platinum) is at the bottom of the series, whereas Fe (Iron) is higher up.
- Analysis: Platinum is less reactive than Iron. Hence, Platinum cannot replace Iron in the compound.
- Conclusion: This reaction will not occur.

2. Reaction: Mn + CaO

- Activity Series Position: Mn (Manganese) is less reactive than Ca (Calcium), with Calcium higher in the series.
- Analysis: Manganese cannot replace Calcium because it is less reactive.
- Conclusion: This reaction will not occur.

3. Reaction: Li + ZnCO3

- Activity Series Position: Li (Lithium) is at the very top of the series, while Zn (Zinc) is lower down.
- Analysis: Lithium is more reactive than Zinc and can replace Zinc in the compound.
- Conclusion: This reaction will occur.

4. Reaction: Cu + 2 KNO3

- Activity Series Position: Cu (Copper) is significantly lower than K (Potassium) on the activity series.
- Analysis: Copper is less reactive than Potassium and cannot replace it in the compound.
- Conclusion: This reaction will not occur.

Based on these analyses, only the reaction between Lithium and Zinc Carbonate (Li + ZnCO3) will take place. Therefore, the answer is:

[tex]\[ \boxed{3} \][/tex]
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