Candle experiment - Lab Assignment PDF

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Chemistry 217 Laboratory Report Short Report Title: Candle Experiment By: Emine Imre, #3423232 April 21, 2020

Purpose: To understand chemistry and physics through the use of candles and simple kitchen chemistry, to practice the process of lab reports, and to use observational skills to complete an experiment. Procedure: This experiment was carried out as outlined in Candle Experiment of the Chemistry 217 Home Lab Manual, pp. 52-57.

Observations: Part A: Re-igniting a Candle 1.

The candle was lit and then blown out.

2.

Smoke trail is created.

3.

Put new flame into the smoke trail, spark flew down smoke and re-ignited the candlewick.

Part B: Water Suck Up 1.

Candle was lit.

2.

Cup was placed on flame, flame remained lit.

3.

Water rises and flame burned out.

Part C: Extinguishing a Candle with Aluminum Foil 1.

Candle was lit

2.

Placed aluminum foil on top of the flame.

3.

Flamed burned out

Part D: Candle Condensation 1.

Candle was lit

2.

Placed the ice in the foil and put above flame.

3.

Bottom of aluminum foil gets wet, burning out the flame

Part E: Extinguishing a Candle with Carbon Dioxide 1.

Candle was lit

2.

Combined baking soda and vinegar, creating a chemical reaction which produced CO2

3.

When CO2 gas poured onto flame, it immediately extinguished.

Results: Part A: Re-igniting a Candle 1. Due to the vaporized wax from candle in the smoke from the flame, the flame traveled down smoke and re-lit the candle. Part B: Water Suck Up 1. Due to the lack of oxygen, once cup was placed on top of flame, the flame extinguished. Part C: Extinguishing a Candle with Aluminum Foil 1. Due to the lack of oxygen to wax, once foil was placed around flame, it extinguished. Part D: Candle Condensation

1. Due to warmth of flame rising and reaching ice pack, air condenses and forms water molecules, extinguishing the flame. Part E: Extinguishing a Candle with Carbon Dioxide 1. Due to the release of carbon dioxide, oxygen was pushed away from flame causing it to extinguish.

Answer to Questions: 1.

The smoke trail contained wax that was never burned, therefore when a new lame is introduced the unburned wax caught fire, leading the trail back to the wick and reigniting the candle.

2. A. Since carbon dioxide is heavier than oxygen it was able to push the oxygen away from the flame causing it to extinguish due to lack of oxygen B. Pouring water directly onto the flame will remove the oxygen molecules, this will not allow the fire to continue burning and decrease heat moving it away from the wick, making sure it will not re-ignite. C. CaCO3 (s) + 2HCI (aq) —> CaCI2 (aq) + H2O (l) + CO2 (g)

3. Candles are hydrocarbons. When foil is placed above flame, water molecules in the candle are attracted to water molecules in the foil and are shown as condensation. Water does not affect a candle's ability to burn but it does extinguish the oxygen molecules.

4. A. Due to the depletion of oxygen, water is sucked up into the jar. When the cup is placed on top of the flame, it burns the oxygen up within the cup causing the flame to extinguish, as air is decreasing in the cup, water is rising, like a suction. B. Water molecules left inside the cup may be attaching themselves to those on the ones outside of the cup, this will allow them to move towards the high water concentration which in this case is inside of the cup.

5. In a normal candle, the flame uses the available oxygen molecules to fuel the flame. The shape of the flame is equalized by the hot air that rises and the cool air that is left behind. Gravity helps to equalize it creating the oval shape. In the microgravity candle, all the available oxygen is not used, the oxygen goes to the flame. It forms a sphere because the flame burns close rather than further away from its source.

Conclusion: To cause a chemical reaction to successfully occur, all of the reactants must be able to be used to the fullest. This experiment teaches us that a reactant can be disturbed by many factors, eventually causing the prevention of the reaction. There is also plenty of basic factors that can affect the reaction such as pressure, oxygen supply, the density of air etc....