Which condition is required for a displacement reaction between a metal and salt solution?
Metal must be higher in reactivity series
A displacement reaction involves a more reactive metal displacing a less reactive metal from its compound. This principle is based on the reactivity series of metals, which ranks metals from most to least reactive.
Let's analyze the given options to determine the condition necessary for a displacement reaction:
- Metal must be higher in reactivity series: This is correct. For a displacement reaction to take place, the metal that replaces the other must be more reactive. This means it must be positioned higher in the reactivity series compared to the metal in the salt solution. For example, if we have a copper sulfate solution and we add zinc metal, zinc is higher than copper in the reactivity series and can displace copper from the solution.
- Metal must be same as salt constituent: This is incorrect. If the metal were the same as in the salt constituent, no reaction would occur as there is nothing to be displaced.
- Reaction must be endothermic: This is incorrect. The thermicity (endothermic or exothermic nature) of the reaction is not a requirement for a displacement reaction. Most displacement reactions are exothermic, releasing energy as bonds form.
- Salt must be insoluble in water: This is incorrect. The solubility of the salt doesn't dictate whether a displacement reaction will occur. The critical factor is the position of the metal in the reactivity series.
Conclusion: The correct condition for a displacement reaction is that the metal must be higher in the reactivity series.
| Reactivity Series (from highest to lowest) |
|---|
| Potassium (K) |
| Sodium (Na) |
| Calcium (Ca) |
| Magnesium (Mg) |
| Aluminium (Al) |
| Zinc (Zn) |
| Iron (Fe) |
| Lead (Pb) |
| Hydrogen (H) |
| Copper (Cu) |
| Silver (Ag) |
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