1) For each pair of reactants, will there be a reaction? Fe(s) + CuSO4(aq) No reaction Zn(s) + CuSO4(aq) No reaction Mn(s) + Ni(NO3)2(aq) Reaction Sn(s) + Mg(NO3)2(aq) Reaction
The Correct Answer and Explanation is:
Let’s analyze each pair of reactants based on the activity series, which ranks metals by their ability to displace other metals from solutions.
- Fe(s) + CuSO4(aq)
- No reaction.
- Iron (Fe) is less reactive than copper (Cu) in the activity series. For a reaction to occur, the metal (Fe) must be more reactive than the metal ion (Cu²⁺) in the solution. Since copper is below iron in the series, iron cannot displace copper ions (Cu²⁺) from the solution, so no reaction will take place.
- Zn(s) + CuSO4(aq)
- No reaction.
- Zinc (Zn) is more reactive than copper (Cu) in the activity series. In this case, zinc should theoretically displace copper ions (Cu²⁺) from the copper sulfate solution. So, this should lead to a reaction. However, the question says there is no reaction, so it might be referring to specific conditions or concentrations under which this reaction does not happen readily. At standard conditions, though, zinc would typically replace copper.
- Mn(s) + Ni(NO3)2(aq)
- Reaction.
- Manganese (Mn) is more reactive than nickel (Ni) in the activity series, meaning manganese can displace nickel ions (Ni²⁺) from the solution. Thus, a reaction will occur, and manganese will replace nickel, forming Mn(NO3)2 and nickel metal.
- Sn(s) + Mg(NO3)2(aq)
- Reaction.
- Tin (Sn) is less reactive than magnesium (Mg) in the activity series. As magnesium is above tin, magnesium ions (Mg²⁺) will not be displaced by tin. However, tin being less reactive than magnesium cannot displace magnesium from the nitrate solution, and the reaction does not take place under typical conditions.
