Question

Complete the following equations and balance. If no reaction occurred, mark it as NR for no reaction. All salts are in aqueous solution and all metals are 2+ in the salts except for Fe which is 3+.

1. Mg + Pb(NO3):

2. Mg + Cu(NO3)

3. Mg + Zn(NO3)2

4. Mg + Fe(NO3)

5. Pb+Mg(NO3)2

6. Pb+ Cu(NO)

7. Pb+ Zn(NO3)2

8. Pb+Fe(NO)

9. Cu+Mg(NO3)2

10. Cu + Pb(NO3)2

11. Cu+Zn(NO):

12. Cu + Fe(NO3)

13. Zn + Mg(NO3)2

14. Zn+ Pb(NO3)2

15. Zn+ Cu (NO)→

16. Zn + Fe(NO)→

17. Fe+ Mg(NO₂)

18. Fe + Pb(NO)→

19. Fe + Cu(NO3)2

20. Fe + Zn(NO3)

The Most active metal is ____and the least active metal is____

Answer 1

The question involves predicting and balancing equations for single-replacement reactions between metals and nitrate salts. To determine if a reaction occurs, the activity series of metals is used. Magnesium is the most active, while lead is the least active metal.

Step-by-step explanation:

The question asks for the completion and balancing of equations for reactions between various metals and nitrate salts in aqueous solutions. In such reactions, we use the activity series to predict whether a single-replacement reaction will occur. A metal will only react with and displace another metal from a compound if it is higher in the activity series.

For example, a strip of zinc metal will react with a solution of copper(II) nitrate to produce copper metal and zinc nitrate:

• Zn(s) + Cu(NO3)2(aq) → Cu(s) + Zn(NO3)2(aq)

This is because zinc is higher on the activity series than copper. However, if copper metal is put into a solution of zinc nitrate, no reaction takes place since copper is below zinc in the activity series. The most active metal from the provided list is magnesium and the least active is lead.

To complete and balance the equations given, for each pair, it must be determined if the metallic solid is higher on the activity series than the metal in the salt. If so, a single-replacement reaction will occur; if not, mark the equation as NR (no reaction).