Q26. Using the activity series, write balanced chemical equations for the following reactions. If no reaction occurs, write NR.

Background

Topic: Activity Series and Single Displacement Reactions

This question tests your understanding of how to use the activity series of metals to predict whether a single displacement (redox) reaction will occur when a metal is placed in a solution containing another metal's ions.

Key Terms and Concepts:

• Activity Series: A list of metals ranked by their ability to be oxidized (lose electrons). A metal higher in the series will displace a metal ion lower in the series from solution.

• Single Displacement Reaction: A reaction where an element reacts with a compound and displaces another element from it.

• NR: No Reaction occurs if the metal is below the ion in the activity series.

Step-by-Step Guidance

1. Refer to the activity series table to determine the relative reactivity of the metals involved in each reaction.

2. Part (a): Iron metal is added to a solution of copper(II) nitrate

   • Find iron (Fe) and copper (Cu) on the activity series.

   • Compare their positions: If Fe is above Cu, Fe can displace Cu2+ from solution.

   • Write the unbalanced equation:

   • Balance the equation for mass and charge.

3. Part (b): Zinc metal is added to a solution of magnesium sulfate

   • Find zinc (Zn) and magnesium (Mg) on the activity series.

   • Compare their positions: If Zn is below Mg, no reaction will occur.

   • If Zn is above Mg, write the unbalanced equation:

   • Balance the equation if a reaction occurs.

4. For each part, use the activity series to justify whether a reaction occurs or not, and set up the balanced equation if it does.

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