Combustion air is air that provides the necessary oxygen for complete, clean combustion and maximum heating value. Combustion gases are the gaseous byproducts of combustion.
In the 17th and 18th centuries combustion was explained by the phlogiston theory, until the French chemist Antoine Lavoisier showed it to be due to combination with oxygen in the air. In fact the oxidizing agent need not be oxygen: it may be another oxidizing gas such as nitric oxide or fluorine, or oxygen-containing solids or liquids such as nitric acid (used in rocket fuels). If the fuel and oxidizer (oxidant) are premixed, as in a Bunsen burner, the combustion is more efficient, and little or no soot is produced. Very rapid combustion occurs in an explosion, when more heat is liberated than can be dissipated, or when a branched chain reaction occurs.
Each combustion reaction has its own ignition temperature below which it cannot take place, e.g., about 400°C for coal. Spontaneous combustion occurs if slow oxidation in large piles of such materials as coal or oily rags raises the temperature to the ignition point.
In rocketry, combustion commonly involves the chemical reaction of a fuel and an oxidizer, but may also may involve the decomposition of a monopropellant or the burning of solid propellants.
Lavoisier's experiments in combustion
From this experiment Lavoisier concluded that in the process of burning the mercury absorbed from the air that part of it that made it possible for animals to breathe and fuel to burn – that is, the gas oxygen, which makes up one-fifth of the air. The part that remains – nitrogen – is a gas which cannot support life or combustion.
When anything burns, the substances taking part in the combustion – fuel and oxygen – combine to form a new substance, such as the mercuric oxide formed in Lavoisier's experiment.
The nature of fire
Any chemical reaction will only take place if certain conditions are present. For the chemical reaction that is combustion, the necessary condition is heat. For a fuel to burn, it must first be brought to a certain temperature, which is called the ignition point. The combustion itself then produces enough heat (if sufficient oxygen is present) to keep the fire going.
Oxygen attacks the molecules of the fuel, breaking them down and combining with the fragments formed. The energy released by the combination of the oxygen with the fragments of the fuel molecules appears as heat.
Rapid combustion and slow combustionIn rapid combustion, heat and light are given off. In slow or latent combustion, on the other hand, oxidation takes place so slowly that the heat developed by the reaction is dispersed as rapidly as it is formed. In these conditions the fuel does not catch fire, and there is no flame.
An example of slow combustion is that which takes place in our bodies. The substances we eat, which give us energy and help build new cells, are partly "burned" by the oxygen that the blood absorbs from the lungs. During this process of slow combustion, energy is given off in the form of heat.
Simple experiments in combustion
Suppose we fasten a lighted candle to a piece of cork, and float the cork on water. If we now place a large glass jar over the candle in such a way that the edge of the jar is below the surface of the water, the candle will go on burning for a short time, then flicker and go out. At the same time the water will rise up inside the jar, and if we mark on the jar the old and new levels of the water we' find that the water has risen to fill one-fifth of the jar. This experiment shows that:
When a candle burns, the products of combustion are carbon dioxide and water. There is a substance, caustic soda, that has the property of absorbing both of these. Suppose we put some caustic soda in a glass tube arranged as shown in the diagram, light a candle under it, and put the whole apparatus on a balance, with weights on the other side to keep the balance arm level. Soon the balance will start to go down on the side of the candle; the weight on that side has been increased by the weight of the oxygen taken from the air.
Related categories• HEAT AND THERMODYNAMICS
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