Report the practical using the following Harding title, aim, apparatus, introduction, precaution, procedure, observation with results in table, and equation of the reaction.

Practical Report: Investigating the Reactivity of Aluminium

Title: WEEK 12 INVESTIGATING THE REACTIVITY OF ALUMINIUM

Aim: To show that aluminium is more reactive than copper.

Apparatus and Materials:

• Conical flask
• Copper (II) Sulfate solution
• Aluminium foil
• Sodium chloride
• Spatula
• Measuring cylinder (implied for measuring solution volume)

Introduction:
This experiment illustrates the displacement of copper from copper(II) sulfate solution using aluminium foil.

Precaution:
Wear eye protection.

Procedure:

1. Measure approximately $20 \text{ cm}^3$ of copper(II) sulfate solution into the conical flask.
2. Add a square of aluminium foil.
3. Look for signs of a reaction.
4. Add a spatula of sodium chloride and stir to dissolve.
5. Observe any changes. If nothing happens, add more sodium chloride. Has displacement of copper from copper(II) sulfate occurred?

Observation with Results in Table:

Observations	Before sodium chloride is added	After sodium chloride is added
Bubbles observed	No	Yes
Colour changes	No (or very slow fading)	Yes (blue fades, becomes colorless)
Temperature change	No (or negligible)	Yes (temperature increases)
Copper observed	No	Yes (reddish-brown solid deposits)

Explanation of Observations:
Initially, aluminium is protected by a thin, unreactive layer of aluminium oxide, preventing it from reacting with copper(II) sulfate. Adding sodium chloride helps to break down this oxide layer, allowing the more reactive aluminium to displace copper from the copper(II) sulfate solution. This results in the formation of reddish-brown solid copper and aluminium sulfate solution, which is colorless. The reaction is exothermic, causing a temperature increase and potentially some bubbling.

Equation of the Reaction:

$$2\text{Al(s)} + 3\text{CuSO}_4\text{(aq)} \longrightarrow \text{Al}_2(\text{SO}_4)_3\text{(aq)} + 3\text{Cu(s)}$$