Introducing
Your new presentation assistant.
Refine, enhance, and tailor your content, source relevant images, and edit visuals quicker than ever before.
Trending searches
Candle Lab
165
Candle Lab
Materials
- Soda can
- Candle
- Chimney from can
- Computer
- Calorimeter
- Water
- Beaker
- Piece of glass
- Stick
Method
Conclusion
The reactants store more energy because this is an exothermic reaction.
We were group 6.
The value that we obtained for the heat combustion was the highest among all the lab groups and the amount of water we used was also the highest.
In addition, our value was closest to the true value of heat combustion (10.5*10^3) kJ/mol
First, we weighed the candle, the volume of water in the beaker and poured the water into the can. Then, we measured the temperature of the water and placed the candle on a piece of glass and put the chimney over it. We lit the candle and waited for 4 minutes. Then, we recorded the weight of the candle, the volume of water, and the temperature of the water again. Finally, we calculated the changes that occurred after combustion.
If we used a more sophisticated calorimeter, our answer would be higher than the result we got because our answer was less than the actual answer. Therefore, if we had a more sophisticated calorimeter, we would be able to get closer to the actual answer.
Introduction
Candles release heat into its surroundings. The objective of this lab was to observe and determine how much energy is released when candle wax and oxygen react to form carbon dioxide and water. We calculate the amount of energy transferred to the water from the candle with the amount of wax burned in our experiment.
Discussion
Data
The primary heat loss from the system was to its surroundings since the top metal container was open and the heat could escape from there. Some natural happenings that mimic this heat loss is breathing. When people breathe out, heat is released from the nose or mouth to the air. A man-made happening that mimics heat loss is coats with armpit zippers. These coats with this specific design allow heat to escape through this opening to cool people off if they get feel too hot. The Law of Conservation of Energy in thermodynamics states that in an isolated system, energy cannot be created or destroyed. Therefore, a possible problem with heat loss from any system is that heat isn't destroyed, but leaves and enters another system. A possible problem with this is when heat leaves a system where heat is needed, like to warm or cook food, then it makes the process less efficient. Also, when heat enters another system, it changes the temperature which can be problematic in some cases like when certain species only survive in a certain temperature range.
Evaluation of Data
Percent Error
Mass of Candle Burned:
|((8.42*10^3)-(10.5*10^3))/10.5*10^3|*100
=19.81%
0.21 g
Quantity of Heat That Would Be Produced if One Mole of the Wax Were Burned
Number of Moles of Wax Burned:
0.0005954 moles
5016 J/1000
= 5.016 kJ
5.016 kJ/ 0.0005954 moles
= 8.42 * 10^3 kJ/mole
Mass of Water Heated:
Quantity of Heat Absorbed by the Water in the Can
(200 mL)(4.18 J/(g*degrees Celsius))(6 degrees Celsius)
= 5016 J
200 mL
Temperature Change of Water: