Heat of Combustion of Candle Wax

7/28/2019 Heat of Combustion of Candle Wax

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Heat of Combustion of Candle Wax

The amount of heat released by the complete combustion of one mole of a

substance is defined as the heat of combustion, Hcomb. The amount of heat

released may be measured in calories (cal) or in joules (J). A calorie is the

amount of heat needed to raise the temperature of one gram of water onedegree Celsius. The SI unit of heat is the joule. One calorie = 4.184J

If a sample of pure carbon is burned in oxygen, the reaction is as follows:

C(s) + O2(g) CO2(g) Hcomb = -393.5 kJ

Some additional heats of combustion are provided in the table.

Heats of Combustion

Substance Formula Hcomb (kJ/mol)

Methane (g) CH4 -890.3

Propane (g) C3H8 -2219.9

Butane (g) C4H10 -3536.1Octane (l) C8H18 -5450.8

In this activity, you will calculate the heat of combustion of the fuel in a

candle. The burning candle will heat a measured quantity of water. Using

the specific heat of water, the mass of the water, and the increase in

temperature, you can calculate the amount of heat released by the burning

candle using the following relationship:

Quantity of heat in joules =

(mass of water)(change of temperature)(specific heat of water),where the specific heat of water is J/(g.C). You can then calculate the moles

of candle wax that burned to obtain the heat of combustion (Hcomb) in

kJ/mol.

Problem

How can you measure the heat released by a burning candle and calculate

the heat of combustion of candle wax?

Objectives

Measure the change in temperature of a mass of water during a

combustion reaction. Calculate the amount of heat released during a combustion reaction.

Calculate the energy released per mole of reactant during a combustion

reaction.

Materials

Candle

Small metal can Large metal can 1/2 in. steel nuts (4)

thermometer balance felt-tip marker

metric ruler Paper clips (2) Matches

Ring stand Ring Thermometer clamp

Glass stirring rod


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Safety Precautions

Always wear safety goggles.

Dispose of wax wastes as directed by your teacher.

Hot objects may not appear to be hot.

Open flames may ignite clothing or hair.

Pre-Lab

1. Define heat of combustion and specific heat

2. State the relationship between joules, mass of water, change of

temperature, and specific heat.

3. Define exothermic and endothermic reactions. What is the sign of H

for an exothermic reaction? An endothermic reaction?

4. Explain how you can calculate the heat of combustion if you know the

number of joules released, the mass of substance burned, and the molar

mass of the substance.

5. Compare the heats of combustion in the chart on page 1 of the lab.Which would you rather have stranded in the snow? Why?

6. Diesel engines are often used in large trucks because the diesel fuel

produces more heat per liter than gasoline. What does this imply about the

nature of the molecules of diesel fuel compared to gasoline (octane)?

Procedure

1. Light a candle and drip a few drops of molten wax onto a can lid Attach

the candle to the lid while the wax is liquid and blow out the candle.

2. Determine the mass of the candle and lid and record this value in a

Data Table.3. Refer to Figure A as you set up the apparatus. Unbend three paper clips

so that they are each in the shape of an S-hook. Use the paper clips to

attach the small can to the ring.

4. Position the candle assembly under the small can and adjust the ring so

that the bottom of the can is 4 or 5 cm above the top of the unlighted

candle.

5. Unhook the small can. Measure the mass of the can and record this

value in Data Table 1.

6. Fill the can approximately half full of distilled water.

7. Measure and record in Data Table 1 the mass of the can and the water.8. Place the large can over the candle.

9. Raise the large can off the base of the ring stand and insert the four

nuts evenly spaced under the can. This will allow air needed for the

combustion of the candle to enter around the base of the can.

10. Record the initial temperature of the water in your Data Table. Use a

match to light the candle.

11. Immediately replace the small can and water in its previous position.

Time the experiment for 10 minutes.

12. While the candle heats the water, gently stir the water with a glass

stirring rod.13. Blow out the candle and record in the Data Table the final temperature


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of the water.

14. Measure the final mass of the candle assembly and record in your

Data Table.

Heat of Combustion of Candle Wax

Data and ObservationsInitial mass of candle assembly (g)

Final mass of the candle assembly (g)

Mass of the empty can (g)

Mass of the small can and water (g)

Initial temperature of water (C)

Final temperature of water (C)

Calculations

Mass of the candle burned (g)

Mass of the water (g)Change in temperature of the water (C)

1. Calculate the number of joules of heat absorbed by the water. Convert

to kilojoules.

2. Assume that the formula for wax in the candle is C32H66.. Find the

moles of the candle burned.

3. Calculate the heat of combustion for wax. The accepted value is around

13,000kJ. There is variability in the components of wax so this is not an

exact amount.


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The Hydrocarbon composition of the wax varies and is a mix of C20 to C40 so an exact

equation can not be given. However, it is a standard combustion reaction. i.e. CxHy + (x

+ y/4) O2 ---> (y/2) H2O + (x) CO2

The little numbers (subscripts) are coefficients. A chemistry reaction is like a math

equation: whatever is on one side has to equal whatever is on the opposite side. Thecoefficients take care of that. They look confusing in the reaction shown because they

are letters, but if you stick numbers in there it would be much easier to understand. Let

us use an example of C25 which would be C25H52.

C25H52 + 38 O2 ------- 25CO2 + 26 H2O + energy (heat and light)

When you burn a candle, you are performing simple combustion reactions of this type.

The oxygen comes from the air and the heat initially comes from an outside source such

as a match. When this combustion reaction happens, it makes water and carbon dioxide

as shown as well as heat and light energy. The coefficients tell us how much of each

component is used and produced.

The wick in a candle is also mainly hydrocarbon with oxygen also present and this also

burns though at a much slower rate. When you light the wick, you provide a heat source

and oxygen from the air. The smoke formed contains carbon dioxide and water and also

some soot from inneficient combustion.

Read more:

http://wiki.answers.com/Q/What_chemical_reactions_occur_during_candle_burning#ix

zz1zexAdQY1
http://wiki.answers.com/Q/What_chemical_reactions_occur_during_candle_burning#ixzz1zexAdQY1http://wiki.answers.com/Q/What_chemical_reactions_occur_during_candle_burning#ixzz1zexAdQY1http://wiki.answers.com/Q/What_chemical_reactions_occur_during_candle_burning#ixzz1zexAdQY1http://wiki.answers.com/Q/What_chemical_reactions_occur_during_candle_burning#ixzz1zexAdQY1


5/14

How to find out Oxygen ratio in air by Candle

combustion

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How to find out Oxygen ratio in air by Candle

combustion Pakistan Science Club

How to find out Oxygen ratio in air by Candle combustion

Materials

candle, glass vessel or PET bottle, match, plate, sodium hydroxide, and water

Procedure

1. The sodium hydroxide is dissolved in water and the solution of 3% is made.

2. The candle is fixed in the plate.

3. Light the candle.

4. Cover it with the glass vessel or the PET bottle.

5. Confirm the water level and the ratio of the volume.

Science

When burning, the candle uses the oxygen in the air. The water made by burning reduce

the volume about 1/1700 after cooling and becoming the liquid. As for remaining

carbon dioxide, it reacts with the sodium hydroxide and the sodium carbonate is made.

It is absorbed to the solution. Therefore, water which is almost same volume of theoxygen rises in the container.
http://paksc.org/pk/media/k2/items/cache/274f1bf2bd18e7f0d33d6244e658426e_XL.jpg?t=943941600


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Why does the water rise?

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e

It's a very popular experiment (eg), from elementary school : put a burning

candle on a dish filled with water, cover the candle with an inverted glass: after

a little while, the candle flame goes out and the water level inside the glass rises.

The standard explanation (as I recall it) was that combustion "burns" oxygen,

and the consummed volume accounts for the extra water that goes inside the

glass. Is this correct? I remember feeling (years later) uncomfortable with the

explanation, because "to burn" is certainly not "to dissapear": I thought that

oxygen combustion produces (mainly) CO2 and hence one oxygen moleculewould produce anotherCO2 molecule, and the volume would remain basicallythe same. Perhaps CO2 dissolves into the water? I would doubt that.

To add to my confusion, others state that the main cause is not the oxygen

combustion but the changes of air temperature, that decreases when the flamegoes out and makes the air inside the glass contract... which would rather

invalidate the experiment as it was (and is) traditionally taught to students.

What is the right explanation?
http://physics.stackexchange.com/questions/19083/why-does-the-water-risehttp://physics.stackexchange.com/questions/19083/why-does-the-water-risehttp://physics.stackexchange.com/questions/19083/why-does-the-water-risehttp://www.sciencefair-projects.org/chemistry-projects/combustion-in-air.htmlhttp://www.stevespanglerscience.com/experiment/00000198http://physics.stackexchange.com/questions/19083/why-does-the-water-risehttp://physics.stackexchange.com/questions/19083/why-does-the-water-risehttp://physics.stackexchange.com/questions/19083/why-does-the-water-risehttp://www.sciencefair-projects.org/chemistry-projects/combustion-in-air.htmlhttp://www.stevespanglerscience.com/experiment/00000198


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(image from here)

Update: As from webpage linked in accepted answer, there are several effects

here, but I think it's safe to say that the "traditional" explanation (consumption of

oxygen) is just wrong: oxygen turns into CO2 and water and -even assumingthat this is the complete chemical picture (it's not) and that all water condenses-

that would produce a slight decrease of volume (CO2 dissolves in water poorlyand very slowly). The main effect here is thermal expansion-contraction of air.

4 Answers

activeoldestvotes

up vote 7 I found two web pages that explain the phenomenon quite well, and even
http://www.vias.org/kas/en/air_pressure.htmlhttp://www.math.harvard.edu/~knill/pedagogy/waterexperiment/index.htmlhttp://physics.stackexchange.com/questions/19083/why-does-the-water-rise?answertab=active#tab-tophttp://physics.stackexchange.com/questions/19083/why-does-the-water-rise?answertab=oldest#tab-tophttp://physics.stackexchange.com/questions/19083/why-does-the-water-rise?answertab=votes#tab-tophttp://www.vias.org/kas/en/air_pressure.htmlhttp://www.math.harvard.edu/~knill/pedagogy/waterexperiment/index.htmlhttp://physics.stackexchange.com/questions/19083/why-does-the-water-rise?answertab=active#tab-tophttp://physics.stackexchange.com/questions/19083/why-does-the-water-rise?answertab=oldest#tab-tophttp://physics.stackexchange.com/questions/19083/why-does-the-water-rise?answertab=votes#tab-top


8/14

down vote

accepted

looks into the misconceptions people have.

The candle flame heats the air in the vase, and this hot air expands. Some of

the expanding air escapes out from under the vase you might see some

bubbles. When the flame goes out, the air in the vase cools down and the

cooler air contracts. The cooling air inside of the vase creates a vacuum.This imperfect vacuum is created due to the low pressure inside the vase and

the high pressure outside of the vase. We know what you're thinking, the

vacuum is sucking the water into the vase right? You have the right idea, but

scientists try to avoid using the term "suck" when describing a vacuum.

Instead, they explain it as gases exerting pressure from an area of high

pressure to an area of low pressure.

A common misconception regarding this experiment is that the consumption

of the oxygen inside of the bottle is also a factor in the water rising. Truth is,

there is a possibility that there would be a small rise in the water from the

flame burning up oxygen, but it is extremely minor compared to theexpansion and contraction of the gases within the bottle. Simply put, the

water would rise at a steady rate if the oxygen being consumed were the

main contributing factor (rather than experiencing the rapid rise when the

flame is extinguished).(1)

The page from Harvard goes into more detail on the argument versus the

error for the incorrect statement.

Argument: Oxygen is replaced by Carbon dioxide. So, there is the same

amount of gas added than taken away. Therefore, heat alone most be

responsible for the water level change.

Source of the Error: A simplified and wrong chemical equation is used,

which does not take into account the quantitative changes. The chemical

equation has to be balanced correctly. It is not true that each oxygen

molecule is replaced by one carbon dioxide molecule during the burning

process; two oxygen molecules result in one carbon dioxide molecule and

two water molecules (which condense). Remember oxygen is present in the

air as a diatomic molecule. [A reader clarifies the water condensation in an

email to me as follows: If the experiment were done with the sealing fluid

able to support a temperature greater than 212 F and the whole system heldabove this temperature then the water product of combustion would remain

gaseous and the pressure within the vessel would increase as a result of three

gaseous molecules for every two prior to combustion and the sealing fluid

would be pushed out.]

Argument: Carbon dioxide is absorbed by the water. Thats why the oxygen

depletion has an effect.

Source of the Error: This idea is triggered from the fact that water can be

carbonized or that the oceans absorb much of the carbon dioxide in the air.

But carbon dioxide is not absorbed so fast by water. The air would have togo through the water and pressure would need to be applied so that the
http://www.stevespanglerscience.com/experiment/00000198http://www.stevespanglerscience.com/experiment/00000198


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carbon dioxide is absorbed during the short time span of the experiment.

Argument: The experiment can be explained by physics alone. During the

heating stage, air escapes. Afterwards, the air volume decreases and pulls

the water up.

Source of the Error: the argument could work, if indeed the heating of the

air would produce enough pressure that some air could leave. In that case,

some air would be lost through the water. But one can observe that the water

level stays up even if everything has gone back to normal temperature (say

10 minutes). No bubbles can be seen.

Argument: It can not be that the oxygen depletion is responsible for the

water raising, because the water does not rise immediately. The water rises

only after the candle dims. If gas would be going away, this would lead to a

steady rise of the water level, not the rapid rise at the end, when the candlegoes out.

Source of the Error: It is not "only" the oxygen depletion which matters.

There are two effects which matter: the chemical process of the burning as

well as a physical process from the temperature change. These effects cancel

each other initially. Since these effect hide each other partially, they are

more difficult to detect. (2)

It clearly has more to do with the temperature differences than any

conversion of gases. Especially considering that a volume of oxygen and

carbon dioxide will be nearly identical to human eye observation.

linkimprove this

answer

editedJan 4 at

23:42

answered Jan 4 at

3:07

Larian LeQuella

4,72621438

4I'd trust Harvard (second footnote I am guessing). SkavaJan

4 at 3:11

1 Yes "Skava", now go to bed! Larian LeQuellaJan 4 at 3:12

3

This answer is useful in pointing the best explanation I've

seen (the second link), but the text is plainly copied other

pages (should be formatted as quotes) and does not makeclear the general summary/conclusion. leonbloyJan 4 at
http://www.math.harvard.edu/~knill/pedagogy/waterexperiment/index.htmlhttp://physics.stackexchange.com/a/19095http://physics.stackexchange.com/posts/19095/edithttp://physics.stackexchange.com/posts/19095/edithttp://physics.stackexchange.com/posts/19095/revisionshttp://physics.stackexchange.com/posts/19095/revisionshttp://physics.stackexchange.com/users/2715/larian-lequellahttp://physics.stackexchange.com/users/5138/skavahttp://physics.stackexchange.com/questions/19083/why-does-the-water-rise#comment45106_19095http://physics.stackexchange.com/questions/19083/why-does-the-water-rise#comment45106_19095http://physics.stackexchange.com/users/2715/larian-lequellahttp://physics.stackexchange.com/questions/19083/why-does-the-water-rise#comment45107_19095http://physics.stackexchange.com/users/1064/leonbloyhttp://physics.stackexchange.com/questions/19083/why-does-the-water-rise#comment45143_19095http://www.math.harvard.edu/~knill/pedagogy/waterexperiment/index.htmlhttp://physics.stackexchange.com/a/19095http://physics.stackexchange.com/posts/19095/edithttp://physics.stackexchange.com/posts/19095/edithttp://physics.stackexchange.com/posts/19095/revisionshttp://physics.stackexchange.com/posts/19095/revisionshttp://physics.stackexchange.com/users/2715/larian-lequellahttp://physics.stackexchange.com/users/5138/skavahttp://physics.stackexchange.com/questions/19083/why-does-the-water-rise#comment45106_19095http://physics.stackexchange.com/questions/19083/why-does-the-water-rise#comment45106_19095http://physics.stackexchange.com/users/2715/larian-lequellahttp://physics.stackexchange.com/questions/19083/why-does-the-water-rise#comment45107_19095http://physics.stackexchange.com/users/1064/leonbloyhttp://physics.stackexchange.com/questions/19083/why-does-the-water-rise#comment45143_19095


10/14

13:49

I'd question one thing from that answer, though: Nowhere is a

vacuum created. There's always air in the glass, and it always

fills the whole space not occupied by water. When the air

cools down, it doesn't contract by itself, only itspressure goesdown (intuitively: Since the molecules get slower, they

hammer less onto the water surface). As result the water is

pressed more in by the air outside than out by the air inside,

and thus flows inside. This rising watercompresses the air

inside, which causes air density and thus pressure inside to

rise again until equilibrium is reached. celtschkJan 18 at

5:47

feedback

upvote 4

down

vote

I have not actually tried this experiment, but I will make at least a fewobservations:

Hypothesis 1: The burning of oxygen is responsible for the reduced air pressure.

Prediction - if the burning of oxygen is the sole cause of the change in pressure,

we should expect to see the water in the glass rise at a more or less constant rate

from the moment the environment is sealed until the burning stops. After the

candle extinguishes, there should be no more change in water level.

Hypothesis 2: The reduction in temperature after the candle extinguishes is

responsible for the reduced air pressure.

Prediction - if the temperature change is the sole cause of the change in pressure,

we should expect to see no change in water level while the candle is burning (in

the limit that the glass was lowered very slowly). After the burning stops, the

water should rise at a rate related to the temperature drop and eventually stop as

the experimental setup comes to room temperature.

In order to test which explaination is correct, you should be able to merely

perform the experiment and match the observation with the prediction. Ofcourse, in real life it may be a combination of these two factors or perhaps

include other reasons not listed here.

Additional measures such as putting an oxygen indicator in the glass (say a fresh

slice of apple) or a thermometer would provide further insight.

Good luck!

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answered Jan 3 at

21:23
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11/14

AdamRedwine

1,914114

1As oxygen is burned - how many moles of CO2 do you get for

each mole of O2 used? Martin BeckettJan 3 at 23:15

1@MartinBeckett: Not to mention it's mostly carbon monoxide

because it's imperfect burning. Mike DunlaveyJan 4 at 3:15

1

@MartinBeckett: The pertinent equation seems to be something

like C25H52+38O2=>25CO2+26H2O. So for 1 mole of

oxygen we have 0.65 moles ofCO2 - a moderate reduction, andthis assuming water condenses. leonbloyJan 4 at 14:40

@leonbloy - although with a smoky candle you do get a lot of CO.

Plus since O2 is only 20% of air it would at most be a (1-

0.65)*0.21 = 7% change in volume even with full combustion

Martin BeckettJan 4 at 16:26

@MartinBeckett: you are right, of course. See the Harvard link in

the other answer for the complete picture. leonbloyJan 4 at16:36

feedback

up

vote 4

down

vote

I will make this into an answer because the idea behind this question is used in

an ancient medical method which was still used by practical nurses and even

prescribed by old fashioned doctors when I was a child more than half a century

ago in Greece. It is now used in alternative medicine practices

The air inside the cup is heated and the rim is then applied to the skin, forming

an airtight seal. As the air inside the cup cools, it contracts, forming a partialvacuum and enabling the cup to suck the skin, pulling in soft tissue, and

drawing blood to that area.

I think it was the invention of antibiotics which diminished rapidly its use,

which was mainly for bronchitis pneumonia and similar afflictions, at least in

Greece.

As far as the question goes, no liquids to confuse the issue of its being a

strongly temperature dependent effect.

linkimprove thisanswer

answered Jan 4 at
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12/14

5:27

anna v

14.4k1925

Indeed, the practice is known as "cupping" and is often offered at

spas and other health resorts. AdamRedwineJan 4 at 13:15

+1 In spanish: "ventosa". I've seen it applied by my grandmother

many years ago. leonbloyJan 4 at 13:37

feedback

up vote

0 down

vote

answer is not oxygen its temperature change in the glass it cool rapidly which

means it cools fast. DONE COPY ANSWER i dont know if its the right answer

WARNING#1 DONT COPY DONT KNOW IF ITS THE RIGHT ANSWER i

did this experiencement 2 times.
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13/14

Faraday's Candle

In 1860 Michael Faraday gave the following series of Christmas Lectures at the Royal

Instution of Great Britain, called "The Chemical History of a Candle":

Lecture I: A Candle: The Flame - Its Sources - Structure Mobility -Brightness

Lecture II: Brightness of The Flame - Air Necessary For Combustion -Production of Water

Lecture III: Products: Water From The Combustion - Nature of Water -A Compound - Hydrogen

Lecture IV: Hydrogen in The Candle - Burns Into Water - The OtherPart of Water - Oxygen

Lecture V: Oxygen Present in The Air - Nature of The Atmosphere -

Carbonic Acid

Lecture VI: Carbon or Charcoal - Coal Gas - Respiration and ItsAnalogy to A Candle

You can read the lectures here.

They included 26 experiments, and among other things he showed how you could see

the structure of a flame better by projecting its shadow on a wall. I tried this and here

are the results. If you want to try this yourself, my tips are that bright sunlight works

best for casting the shadow, and if you are going to photograph it, try reducing the

exposure.

If you see something you like, and would like to use or have a print of, email photos

at subjectline dot co dot uk.
http://www.rigb.org.uk/http://www.rigb.org.uk/http://www.rigb.org.uk/http://www.fordham.edu/halsall/mod/1860Faraday-candle.htmlhttp://www.subjectline.co.uk/faradayscandle/large_tall.jpghttp://www.subjectline.co.uk/faradayscandle/large_dark.jpghttp://www.subjectline.co.uk/faradayscandle/large_cloud.jpghttp://www.rigb.org.uk/http://www.rigb.org.uk/http://www.fordham.edu/halsall/mod/1860Faraday-candle.html


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Heat of Combustion of Candle Wax

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