Based on the activity series, which of the following pairs of reactants will result in a chemical reaction?

• A. Ag(s) + HCl(aq)
• B. Cu(s) + ZnSO_4(aq)
• C. Au(s) + FeSO_4(aq)
• D. Zn(s) + CuSO_4(aq)

Answer: (D)

Verified step by step guidance

1. Understand that the activity series is a list of metals ranked by their ability to displace other metals from compounds in solution. A metal can displace another metal ion from solution if it is higher in the activity series.
2. For each pair of reactants, identify the metal in its elemental form and the metal ion in the aqueous solution. For example, in Ag(s) + HCl(aq), Ag is the metal and H^+ from HCl is the ion in solution.
3. Check the position of the elemental metal and the metal ion in the activity series. If the elemental metal is above the metal ion in the series, a displacement reaction will occur; otherwise, it will not.
4. Apply this to each pair: For Ag(s) + HCl(aq), silver is below hydrogen in the activity series, so no reaction occurs. For Cu(s) + ZnSO_4(aq), copper is below zinc, so no reaction. For Au(s) + FeSO_4(aq), gold is below iron, so no reaction.
5. For Zn(s) + CuSO_4(aq), zinc is above copper in the activity series, so zinc can displace copper ions from solution, resulting in a chemical reaction.