Materials Required

Aluminium foil, Dilute hydrochloric acid, Conical flask, Rubber cork, Glass tube, Lighter, Candle, Measuring cylinder, Forceps, Glass stopper bottle with dropper and Stand.

Procedure

Real Lab Procedure:

Take a few pieces of aluminium foil in a dry conical flask.
Pour 3 ml of dilute hydrochloric acid into the conical flask using a measuring cylinder.
Place the rubber cork on the mouth of the test tube.
Insert the glass tube into the conical flask through the hole of the rubber cork.
Take a lighter and light the candle.
Bring the lightened candle into the mouth of the glass tube.

Simulation Procedure:

Drag the forceps onto the top of the watch glass containing aluminium foil. 
Drop the forceps to take a few pieces of aluminium foil. 
Drag the forceps containing aluminium foil towards the conical flask.
Drop the aluminium foil into a conical flask.
Drag and drop the dropper with 3 ml of diluted hydrochloric acid into the measuring cylinder.
Drag and drop measuring cylinder containing dil.HCl into a conical flask.
Drag and drop the rubber cork on the mouth of the conical flask. 
Drag and drop the glass tube into the conical flask through the hole of the rubber cork. 
Drag and drop a lighter towards the candle and light the candle. 
Drag and drop the lightened candle into the mouth of the glass tube.

Observation

On adding acid into a conical flask containing aluminium foil, bubbles of some gas evolve.
On bringing an ignited candle near the glass tube's mouth, the gas burns with a “Pop” sound.

Conclusion

Hydrogen gas evolved in the reaction between the aluminium foil and dilute hydrochloric acid.

Aluminium + dilute hydrochloric acid → Aluminium chloride+ hydrogen gas.

2Al + 6HCl →2AlCl₃ + 3H₂

Hydrogen gas burns, forming water, producing a pop sound.

Hydrogen gas + Oxygen gas → water (pop sound)

2H₂ + O₂ → H₂O + Energy

Precautions

Take necessary precautions in the laboratory.
Be careful while using the lightened candle.
Be careful while handling the acids.