Periodic Table Based on the understanding of the way the metals are placed in the activity series, the student correctly predicted the outcome of four reactions. According to the student, which reactions are most likely to take place? Select all that apply. A. Zn and CuSO_(4) B. Ag and CuSO_(4) C. Fe and ZnSO_(4) D. Mg and ZnSO_(4)

To determine which reactions are most likely to take place, we need to consider the activity series of metals. The activity series is a list of metals arranged in order of their reactivity from highest to lowest. Metals higher in the series can displace metals lower in the series from their compounds.Here is a simplified version of the activity series:1. Potassium (K)2. Calcium (Ca)3. Sodium (Na)4. Magnesium (Mg)5. Aluminum (Al)6. Zinc (Zn)7. Iron (Fe)8. Nickel (Ni)9. Tin (Sn)10. Lead (Pb)11. Hydrogen (H)12. Copper (Cu)13. Silver (Ag)14. Gold (Au)Now let's analyze each reaction:A. **Zn and ** - Zinc (Zn) is higher in the activity series than Copper (Cu). - Therefore, Zinc can displace Copper from Copper sulfate. - Reaction: - This reaction is likely to take place.B. **Ag and ** - Silver (Ag) is lower in the activity series than Copper (Cu). - Therefore, Silver cannot displace Copper from Copper sulfate. - This reaction is unlikely to take place.C. **Fe and ** - Iron (Fe) is lower in the activity series than Zinc (Zn). - Therefore, Iron cannot displace Zinc from Zinc sulfate. - This reaction is unlikely to take place.D. **Mg and ** - Magnesium (Mg) is higher in the activity series than Zinc (Zn). - Therefore, Magnesium can Zinc from Zinc sulfate. - Reaction: - This reaction is likely to take place.Based on the analysis, the reactions that are most likely to take place are:- A. Zn and - D.