Category: Chemical equation for burning candle

Chemical equation for burning candle

Ok, just kidding. The following represents an "average" reaction. Of course, this is the ideal reaction where there is complete combustion. Anyone who has every watched a candle burn has seen smoke and soot come from the candle. This indicates that there is less than complete combustion, so there are actually a wide variety of shorter-chained carbon compounds being produced.

A complete and accurate equation cannot be given. Candle wax consists of a number of heavy hydrocarbon compounds ranging from C15 to C30 depending on the type of candle. A party candle will have fewer, smaller compounds low densitywhile a large Church candle will have a much higher density due to the larger molecules of wax.

When you see a candle burning, the amount of oxygen that can react with the wax vapour from the wick, is insufficient. The reaction therefore will not give complete combustion and results in a smoky, yellow flame indicating that Carbon 'C' as Soot is formed.

What is carbon magnetic moment spin when is it in atomic level after breaking of carbon-hydrogen chain and before interacting with oxygen?

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Candle Burning

Favorite Answer. Candle plus oxygen goes to carbon dioxide and water. Burning A Candle Chemical Reaction. Norrie Lv 7. How do you think about the answers? You can sign in to vote the answer. Source s : advanced level physics, 2nd ed by nelkon and parker. Dare Devil. Simple it is an oxidation reaction.

Still have questions? Get your answers by asking now.In fact, scientists have been fascinated by candles for hundreds of years. InMichael Faraday gave his now-famous lecture series on the Chemical History of a Candle, demonstrating dozens of scientific principles through his careful observations of a burning candle. In the late s, NASA took candle research to new heights, conducting space shuttle experiments to learn about the behavior of candle flames in microgravity.

Scientists in universities and research laboratories around the world continue to conduct experiments with candles to learn more about candle flames, emissions and combustion. And, of course, thousands of students every year investigate the principles of heat, light and combustion through school science projects involving candles. All waxes are essentially hydrocarbons, which means they are largely composed of hydrogen H and carbon C atoms.

When you light a candle, the heat of the flame melts the wax near the wick. This liquid wax is then drawn up the wick by capillary action. The heat of the flame vaporizes the liquid wax turns it into a hot gasand starts to break down the hydrocarbons into molecules of hydrogen and carbon.

These vaporized molecules are drawn up into the flame, where they react with oxygen from the air to create heat, light, water vapor H 2 O and carbon dioxide CO 2. Enough heat is created to radiate back and melt more wax to keep the combustion process going until the fuel is used up or the heat is eliminated. It takes a few minutes when you first light a candle for this combustion process to stabilize.

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The flame may flicker or smoke a bit at first, but once the process is stabilized, the flame will burn cleanly and steadily in a quiet teardrop shape, giving off carbon dioxide and water vapor. A quietly burning candle flame is a very efficient combustion machine.

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But if the flame gets too little or too much air or fuel, it can flicker or flare and unburned carbon particles soot will escape from the flame before they can fully combust.

The wisp of smoke you sometimes see when a candle flickers is actually caused by unburned soot particles that have escaped from the flame due to incomplete combustion. Click Here for Candle Research Studies. Above that is a small dark orange-brown section, and above that is the large yellow region that we associate with candle flames.

The oxygen-rich blue zone is where the hydrocarbon molecules vaporize and start to break apart into hydrogen and carbon atoms. The hydrogen is the first to separate here and reacts with the oxygen to form water vapor.

Some of the carbon burns here to form carbon dioxide. This is where the various forms of carbon continue to break down and small, hardened carbon particles start to form. As they rise, along with the water vapor and carbon dioxide created in the blue zone, they are heated to approximately degrees Centigrade.A candle flame is actually a chemical reaction in action!

Candle wax is one of the chemicals in the reaction. Can you guess what the wax reacts with? Find out in this experiment!

Candle Burning

Watch the candle flame start out small and get bigger. Notice how some of the wax near the wick melts. As the flame burns, the wax from the candle is reacting with something else to make the flame. Ask the adult you are working with to carefully place a glass jar over the candle and to leave it there.

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The substance that reacts with the candle wax is oxygen. It comes from the air. Putting the jar over the candle keeps oxygen from outside the jar from getting in. The reaction can only use the oxygen that is already in the jar. Running out of oxygen makes the flame go out. Another chemical reaction you probably know is the reaction between vinegar and baking soda. This reaction produces a gas called carbon dioxide. This gas can be used to put out a flame.

When you are ready, carefully pour all the vinegar from the cup into the jar with the baking soda. Ask the adult you are working with to carefully pour the carbon dioxide gas onto the flame. Be sure no liquid comes out ā€” just the gas. Carbon dioxide molecules are heavier than air. Because of this, they push the oxygen and other molecules in the air out of the way as they sink down over the flame and candle. This makes the flame go out.

Next time you blow out a candle, think about what your breath is actually doing. Why do you think blowing on a candle flame makes it go out? If you do not respond, everything you entered on this page will be lost and you will have to login again.

Flame Out. Experiment 1 A candle flame is actually a chemical reaction in action! What to do. Ask the adult you are working with to light the candle. What do you think it might be?

chemical equation for burning candle

Why does the flame go out when the jar is covering it? Experiment 2 Another chemical reaction you probably know is the reaction between vinegar and baking soda. Ask the adult you are working with to light the tealight candle. Place about two teaspoons of baking soda in the jar. Next pour about two tablespoons of vinegar in a cup.When paraffin comes into contact with oxygen with enough energy, it burns completely and becomes water and carbon dioxide. The fire is a result of this reaction happening very quickly and is known as combustion.

The fire is so hot that the wax actually turns from a solid to a vapor. It is the wax vapor that is actually participating in the chemical reaction.

A candle is made of wax, which is made of hydrocarbons. This means that it's composed of compounds with a carbon backbone and hydrogen atoms that dangle off of the backbone. Other examples of hydrocarbons are gasoline, propane, and even things like paper and plant matter are largely composed of hydrocarbon type compounds. The chemical reaction involved in burning is the oxidation of these hydrocarbons. In an ideal reaction, the reactants are the hydrocarbon and oxygen and the products are water, carbon dioxide and energy in the form of light and heat.

In reality, burning is not totally ideal and there are additionally side reactions and secondary products like nitrogen oxides from reactions with air and partially oxidized hydrocarbons like ash. The candle is made of wax, which is a combination of different kinds of hydrocarbons i. The reaction combines atmospheric oxygen with the hydrocarbons to create carbon dioxide and water just the same way as burning any other hydrocarbon e. Please help me and explain briefly on the burning of a candle, what is the chemical reaction involved?

Answer 2: A candle is made of wax, which is made of hydrocarbons. Answer 3: The candle is made of wax, which is a combination of different kinds of hydrocarbons i. Click Here to return to the search form.A burning candle seems far removed from the suspenseful world of chemistrysince it would appear to amount to nothing more than combustion of an organic compound:.

An equation like the one above does indeed provide a straightforward description of the beginning and end of this combustion, but we are more interested here in the steps in between! There is no better, there is no more open door by which you can enter into the study of natural philosophy, than by considering the physical phenomena of a candle.

Until the middle of the 18th century, high-quality candles were made almost exclusively from beeswax. Such candles produced a superb flame, were attractive, and dispensed a pleasant fragrance, but they were considered a luxury item reserved primarily for churches, monasteries, and houses of the nobility. Ordinary people had to depend upon inferior, greasy candles based on ox-kidney fat and mutton tallow, which upon burning would give off large amounts of sooty smoke, and must have smelled horrible.

Justus Liebig was the first to look into the chemical nature of beeswax, and waxes in general were subsequently described as mixtures of esters derived from long-chain carboxylic acids and long-chain alcohols. The true chemical composition of beeswax shows this definition was in fact incorrect, since free long-chain carboxylic acids as well as long-chain hydrocarbons are normally also present Table 1. The trivial names applied to long-chain acids and alcohols are dizzying. Until relatively recently, the latter trivial name was also applied to corresponding C 31 compounds.

A host of natural and synthetic materials display wax-like characteristics, and are suited to the manufacture of candles. The First Semi-Synthetic Wax. The first semi-synthetic wax was prepared by M. Chevreul in the early 19th century [4, 5].

His stearin was hard at room temperature, and displayed the white opacity cherished by chandlers candle-makers. Stearin is today understood to be a mixture of palmitic and stearic acids. This fatty acid later proved again to be a mixture: of hexa- and octadecanoic acids.

Paraffin has been employed for the manufacture of candles since the middle of the 19th century. A mixture of saturated hydrocarbons, it is now obtained almost exclusively from petroleum.

The melting point of paraffin varies with the chain lengths of its constituents. Pure paraffins are colorless and transparent, and display a wide range of softening points.Admiring a burning candle, perhaps surrounded by sprays from a fir tree, cautiously blowing on the flame, and watching as liquid wax drips, is a fascinating treat for almost everyone. We now trace the fate of individual wax molecules in a burning candle.

In Zone I, wax vaporizes directly from the surface of the wick Fig. Wax vaporization is easy to demonstrate by holding one end of a glass tube in the lower part of Zone I.

Outside the actual flame we see deposition of unconsumed wax, which can ultimately be ignited Fig.

Combustion of Hydrogen

The temperature in the dark Zone I increases as one moves either up or toward the outside, since the distance to the hot reaction zones thereby decreases. Here no oxygen is available, so increasing temperature leads only to more thermal decomposition. In the first reaction step, Cā€”C bonds break to produce pairs of radicals Fig.

These hydrocarbon radicals are highly reactive: subsequent elimination of hydrogen atoms leads to olefins, elimination of ethylene gives shorter radicals, and finally, diradicals can cyclize, after which more hydrogen atoms can be eliminated, etc. Overall there is a confusing tangle of reactions, leading to a mixture of smaller, unsaturated aliphatic, alicyclic, and aromatic hydrocarbons. The free hydrogen atoms that result might, on the one hand, generate new hydrocarbon radicals, or, due to their tiny atomic mass, rapidly diffuse into the reaction zones.

In any case, in the hot parts of Zone I, any wax molecules are thermally cleaved, so in the flame of a candle, no intact wax molecules will come in contact with oxygen! Now we come to the chemical heart of a candle flame: the reaction zones.

Chemical Reactions

Here, pyrolytic decomposition products from wax molecules, as they arrive from the interior, encounter oxygen diffusing in from the surroundings. The highly exothermic oxidation reactions that take place here are limited only by the supply, through diffusion, of appropriate reaction partners. The flame of a candle thus corresponds to a typical diffusion flame. A candle flame that is not smoking is completely enclosed by its reaction zones.

So why is it that the lower part of the reaction region, Zone II, appears to burn blue-green, while Zone III seems to give off no light whatsoever, even though in all the reaction zones exactly the same processes are taking place?

The answer is rather surprising: this is an optical illusion! The bright yellow emission from Zone IV completely outshines the weak, bluish light from the adjoining reaction zones. As a result, our eyes are only able to distinguish bluish light coming from Zone II, the region farthest removed from the bright yellow source.

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Two unusual molecules betray their existence through this bluish light, a color familiar to us already from the natural-gas flame of a gas stove or a Bunsen burner. In these devices, natural gas is mixed ahead of the flame with air, and it is the resulting mixture that is combusted.

The characteristic band spectrum produced by such a flame [6] is derived from two molecular sources. Excited C 2 molecules form mostly via reactions of oxygen atoms with higher hydrogen-deficient hydrocarbon radicals. All the excited species spontaneously release their excess energy in the form of light chemiluminescence.

The primary oxidizing agent here turns out to be not oxygen itself, but rather the hydroxyl radical OH [8]. One recognizes here a kind of reaction chain, which becomes even more effective as a consequence of the oxygen atoms formed in the first step Eq.Combustion is another name for burning.

It is an example of an exothermic reaction, a reaction that releases energy to the surroundings. This is mostly thermal energy, but light energy and sound energy are also released. Note that some other reactions are endothermic reactions ā€” they take in energy from their surroundings. The fire triangle shows the three things needed for a fire to start and keep going. If one of the sides of the fire triangle is removed, a fire will not start, and a fire that is already burning will go out.

Fire-fighting relies on this principle. The fire will go out when the fuel runs out, but it is often unsafe to leave a fire that long. Different types of fires need to be tackled in different ways.

chemical equation for burning candle

Coal, oil and natural gas are fuels that are widely used. They contain hydrocarbonswhich are compounds of hydrogen and carbon only. When the fuel burns, its hydrocarbons react with oxygen. If there is plenty of air, complete combustion happens:. Natural gas is mostly methane, CH 4.

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Here are the equations that model its complete combustion:. Candles are made from hydrocarbons. The diagram shows how they can be used in the laboratory to investigate combustion. The carbon dioxide produced can be detected using limewater. This turns milky cloudy white when carbon dioxide is bubbled through it.

If there is not enough air or oxygen for complete combustion, incomplete combustion happens instead. Water vapour and carbon dioxide are still produced, but two other products are also produced:. Combustion reactions Combustion is another name for burning. A fire needs a fuel, oxygen or airand heat If one of the sides of the fire triangle is removed, a fire will not start, and a fire that is already burning will go out.

Fire How to put it out Part removed Chip pan oil fire Cover the pan with a damp cloth Oxygen Forest fire Make a fire break cut down a line of trees Fuel Forest fire Spray with water Heat Complete combustion Coal, oil and natural gas are fuels that are widely used. If there is plenty of air, complete combustion happens: the hydrogen atoms combine with oxygen to make water vapour, H 2 O the carbon atoms combine with oxygen to make carbon dioxide, CO 2 the maximum amount of energy is released Natural gas is mostly methane, CH 4.

chemical equation for burning candle

Investigating combustion The carbon dioxide produced can be detected using limewater. The limewater test for carbon dioxide. Chip pan oil fire. Cover the pan with a damp cloth.

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