Fire Triangle

Fire triangle
The fire triangle or combustion triangle is a simple model for understanding the ingredients necessary for most fires.[1]

The triangle illustrates a fire requires three elements: heat, fuel, and an oxidizing agent (usually oxygen). The fire is prevented or extinguished by removing any one of them. A fire naturally occurs when the elements are combined in the right mixture.

Without sufficient heat, a fire cannot begin, and it cannot continue. Heat can be removed by the application of a substance which reduces the amount of heat available to the fire reaction. This is often water, which requires heat for phase change from water to steam. Introducing sufficient quantities and types of powder or gas in the flame reduces the amount of heat available for the fire reaction in the same manner. Scraping embers from a burning structure also removes the heat source. Turning off the electricity in an electrical fire removes the ignition source.

Without fuel, a fire will stop. Fuel can be removed naturally, as where the fire has consumed all the burnable fuel, or manually, by mechanically or chemically removing the fuel from the fire. Fuel separation is an important factor in wildland fire suppression, and is the basis for most major tactics, such as controlled burns. The fire stops because a lower concentration of fuel vapor in the flame leads to a decrease in energy release and a lower temperature. Removing the fuel thereby decreases the heat.

Without sufficient oxygen, a fire cannot begin, and it cannot continue. With a decreased oxygen concentration, the combustion process slows. In most cases, there is plenty of air left when the fire goes out so this is commonly not a major factor.
Fire tetrahedron
The fire tetrahedron is an addition to the fire triangle. It adds the requirement for the presence of the chemical reaction which is the process of fire. For example, the suppression effect of Halon is due to its interference in the fire chemical inhibition.

Combustion is the chemical reaction that feeds a fire more heat and allows it to continue. When the fire involves burning metals like lithium, magnesium, titanium,[2] etc. (known as a class-D fire), it becomes even more important to consider the energy release. The metals react faster with water than with oxygen and thereby more energy is released. Putting water on such a fire results in the fire getting hotter or even exploding because the metals react with water in an exothermic reaction. Carbon dioxide extinguishers are ineffective against certain metals such as titanium.[2] Therefore, inert agents (e.g. dry sand) must be used to break the chain reaction of metallic combustion. In the same way, as soon as we remove one out of the 3 elements of the triangle, combustion stops.
Fire classes
Based on the combustible material involved, the fire can be classified. In the European Standard "Classification of fires" (EN 2:1992, incorporatiing amendment A1:2004), the fires are classified as:

* Class A fire: Ordinary combustibles such as wood, paper, carton, textile, and PVC;
* Class B fire: Flammable liquids and solids which can take a liquid form, such as benzene, gasoline, oil;
* Class C fire: Flammable gases, such as butane, propane, and natural gas;
* Class D fire: Combustible metals, such as iron, aluminum, sodium, and magnesium;
* Class F fire: Cooking media, such as oils and fats, in cooking appliances;

A fire involving energized electrical equipment is not classified by its electrical property.

In the American standard, fires are classified as:

* Class A fire: Ordinary combustibles such as wood, paper, carton, textile, and PVC;
* Class B fire: Flammable liquid or gaseous fuels such benzene, gasoline, oil, butane, propane, and natural gas;
* Class C fire: Involving energized electrical equipment, often caused by short circuits or overheated electrical cables;
* Class D fire: Combustible metals, such as iron, aluminum, sodium, and magnesium;
* Class K fire: Containing a fat element, such as cooking oil
Oxidizer
The oxidizer is the other reactive of the chemical reaction. In most cases, it is the ambient air, and in particular one of its components, Oxygen (O2). By depriving a fire of air, we extinguish it; for example, when covering the flame of a small candle with an empty glass, fire stops; to the contrary, if we blow over a wood fire, we activate it (by bringing more air). In certain torches, we bring dioxygen to improve combustion. In certain very particular cases (such as explosives like aluminum), the oxidizer and combustible are the same (i.e.nitroglycerin, an instable molecule made of one oxidizing part linked to a reducing part). Reaction is initiated by an activating energy, in most cases, it is heat. Several examples include friction, as in case of matches, heating an electrical wire, a flame (propagation of fire), or a spark (from a lighter or from any starting electrical device). There are also many other ways to bring sufficient activation energy including electricity, radiation, and pressure, all of which will lead to a temperature rise. In most cases, heat production enables self-sustainability of the reaction, and enables a chain reaction to grow. The temperature at which a liquid produces sufficient vapor to get a flammable mix with self-sustainable combustion is called its flash-point.
Extinction of the fire
To stop a combustion reaction, one of the three elements of the fire-triangle has to be removed:

* Suppression of the Combustible: by closing of the valve fueling the combustion, creating sufficient distance between fire and flame, exhausting hot smoke (containing unburned elements), …
* Suppression of the Oxidizer (also known as choking): by the use of a carbon dioxide fire-extinguisher, a blanket, or spraying sufficient water on a solid combustible (water vapor removes fresh air) …
* Suppression of the Activation Energy (cooling down): by spraying water in a mix of air + combustible particles), net absorbing the heat ("Davy" miner lamp), exhausting to remove hot smoke, …
Role of water in fire-fighting
Water can have two different roles:

1. In the case of a solid combustible, the solid fuel produce pyrolyzing products under the influence of heat, commonly radiation. This process is halted by the application of water, since water is more easily evaporated than the fuel is pyrolyzed. Thereby energy is removed from the fuel surface and it is cooled and the pyrolyze is stopped, removing the fuel supply to the flames. In fire fighting, this is referred to as surface cooling

2. In the gas phase, i.e. in the flames or in the smoke, the combustible can not be separated from the oxidizer, the only possible action consists of cooling down. In this case, water droplets are evaporated in the gas phase, thereby lowering the temperature and adding water vapour making the gas mixture non combustible. This requires droplets of a size less than about 0.2 mm. In fire fighting, this is referred to as gas cooling or smoke cooling. There also exist cases where the ignition factor is not the activation energy. For example, smoke explosion is a very violent combustion of unburned gases contained in the smoke created by a sudden fresh air input (oxidizer input). The interval in which an air/gas mix can burn is limited by the explosivity limits of the air. This interval can be very small (kerosene) or large (acetylene).
Role of water additives
The role of water in extinguishing a fire can be summarized as follows: The main effect is cooling down the fire by absorption of heat energy either at the fuel surface or in the gas phase. A contributing effect is diluting the atmosphere by adding vapor and thereby removing oxygen from the fire The main limits to the use of water are directly linked to the physical-chemical characteristics of water itself: - Water can’t be used on certain type of fires :

* Hydrocarbon fires (B class) - as it will only spread the fire because of the difference in density
* Metal fires (D class) - as these fires produce huge amounts of energy (up to 7.550 calories/kg for Aluminum) and water can also create violent chemical reaction with burning metal (by oxidization)
* Fat fires (F class) - as vapor will carry and spread burning oil everywhere.

Since these reactions are well-understood, it has been possible to create specific water-additives which will allow:

* A better heat absorption with a higher density than water
* Carrying free radical catchers on the fire
* Carrying foaming agents to enable water to stay on the surface of a liquid fire and prevent gas release
* Carrying specific reactives which will react and change the nature of the burning material

Water-additives are generally designed to be effective on several categories of fires (class A + class B or even class A + class B + class F), meaning a better global performance and polyvalence of the fire-extinguisher.
Chemistry of Combustion
Combustion is a chemical reaction in which complex molecules are broken down into smaller, more stable molecules through a rearrangement of atomic bonds. A major component of the chemistry of high-temperature combustion involves radical reactions. However, it is possible to consider combustion as a single overall reaction.

Example : H3C-CH2-CH3 + 5O2 → 3CO2 + 4H2O

Carbon dioxide and water are more stable than oxygen and propane. Combustion is an oxidation-reduction reaction, meaning oxidization of a combustible by an oxidizer; • combustible is being oxidized during combustion, it is a reducer as it loses electrons; • Oxidizer is the part being reduced; it is an oxidizer as it gains electrons. As with any chemical reaction, a catalyst encourages combustion and as it has a high activation energy level, the use of a catalyst enables working at lower temperature. This leads to more complete combustion as in the catalyst of the exhaust of a car, where catalytic metals burn residues contained in the exhaust smoke at lower temperature than in the engine. Concerning solid combustible, the activation energy allows for vaporization or pyrolysis of the combustible. Gas produced will then mix with an oxidizer resulting in a combustible mixture. If the energy produced by the combustion is higher or equal to the quantity of energy required for the combustion, the reaction is then self-sustainable.
Produced energy and calorific power
The quantity of energy produced by the reaction is higher than the quantity of energy requested to start it. The quantity of energy produced by the combustion is given in Joules (J); it is the enthalpy of the reaction. In the application domains (oven, burner, engine with internal combustion, fire-fighting), we use the notion of calorific power, what is basically the enthalpy of the chemical reaction per unit of weight of combustible or the obtained energy given by the combustion of one kilogram of combustible, expressed in kilojoules per kilogram (kJ/kg or kJ•kg-1). Combustion of hydrocarbon produces water in its vapor form. ; This water vapor contains huge amount of energy and this parameter has to be taken into account in a specific way to evaluate correctly the calorific power. We define: • Superior Calorific Power (SCP): « Quantity of energy produced during a complete combustion of a combustible unit, water vapor is said condensed and heat collected »2. • Inferior Calorific Power (ICP): « Quantity of energy produced during a complete combustion of a combustible unit, Water vapor is said non-condensed and heat not collected »3. Difference between ICP and SCP is the latent heat of water vaporization (Lv) multiplied by the quantity of produced vapor (m), what equals +/- 2 250 kJ•kg-1 (this value is influenced by pressure and temperature). We have the relation SCP = ICP + m•Lv.