Curriculum
- 5 Sections
- 22 Lessons
- 65 Weeks
Expand all sectionsCollapse all sections
- Understanding IFE Level 2 Certificate in Fire Science, Operations and Safety1
- Fire Engineering Science7
- Fire and Rescue Operations9
- Fire Safety4
- Preparing & Booking for Exams2
Heat and Temperature
Heat and Temperature
Measuring Temperature
Measuring temperature is fundamental in fire science, as it allows accurate monitoring of heat conditions in environments affected by fire. Temperature is a measure of the average kinetic energy of particles in a substance. In fire and rescue operations, reliable temperature readings are critical for assessing fire development, ensuring firefighter safety, and evaluating the effectiveness of fire suppression. Temperature can be measured using a variety of instruments, depending on the required range and application.
Thermometric Scales: Celsius, Fahrenheit, Kelvin
Thermometric scales allow temperature to be expressed numerically. The Celsius (Centigrade) scale is the most commonly used in scientific and fire service applications, where water freezes at 0°C and boils at 100°C under standard pressure. Fahrenheit is still used in some countries, where the freezing point of water is 32°F and boiling point is 212°F. Kelvin, or the Absolute scale, begins at absolute zero (0 K), where all molecular motion theoretically ceases. It is often used in scientific calculations, especially those involving gas laws and thermodynamic properties in fire scenarios.
Other Methods of Measuring Temperature
Various other methods are employed depending on the situation. Air or gas thermometers measure the expansion of gases with temperature changes. Solids like bimetallic strips respond to temperature by bending, making them useful in thermostats. Thermocouples and thermistors are commonly used in fire detection systems — thermocouples generate a voltage when exposed to heat, while thermistors change resistance. Brightness comparison techniques use visual estimation of glowing objects, such as metals or coals. Infrared thermometers and thermal imaging cameras are widely used in modern firefighting to detect heat sources and locate individuals in smoke-filled environments.
Joule and Calorie
Heat energy is quantified using units such as the joule and the calorie. One calorie is the amount of energy required to raise the temperature of one gram of water by one degree Celsius. The joule, the SI unit of energy, is used more widely in scientific contexts. One calorie is approximately equal to 4.18 joules. Understanding these units allows fire professionals to calculate energy outputs of fuels and assess the energy transfer involved in heating, combustion, and cooling.
Specific Heat
Specific heat is the amount of heat required to raise the temperature of one kilogram of a substance by one degree Celsius. Substances with high specific heat, like water, absorb large amounts of energy before their temperature increases significantly. This property is crucial in firefighting, as water’s high specific heat makes it an effective cooling agent. Firefighters must also consider specific heat when assessing how different materials in a building respond to heat.
Changes of State and Latent Heat
Changes of state involve energy transfer without a change in temperature. Latent heat is the energy required for a substance to change its phase. The latent heat of vaporisation refers to the energy needed to convert a liquid to a gas, which is significant during the application of water onto hot surfaces, where steam formation absorbs large amounts of heat. Pressure changes also affect boiling points and latent heat, a factor relevant in confined fires or sealed environments. The latent heat of fusion refers to the energy required to change a solid to a liquid. Cooling processes, such as water evaporation, remove heat from a system, aiding fire suppression and temperature control.
Gases of Different Density
Gases differ in density based on their molecular weight and temperature. Heavier gases such as propane accumulate in low areas, potentially creating hazardous conditions, whereas lighter gases disperse upwards. Recognising these differences is essential for effective fire control and personnel safety.
Thermal Expansion of Solids
Solids expand when heated due to increased particle vibration. The coefficient of linear expansion quantifies this increase in length. In fire safety, thermal expansion must be considered in metal beams, rails, and structural supports. Invar, a nickel-iron alloy, is used in precision instruments because of its very low expansion. In large structures, expansion joints are added to accommodate changes. Thermostats use bimetallic strips that bend with temperature due to differing expansion rates of metals. Solids also have superficial and cubical expansion properties, which affect volume and surface area under heat.
Thermal Expansion of Liquids
Liquids expand cubically when heated, and this expansion reduces their density. This principle affects fuel behaviour and storage in fire safety. For example, petrol tanks must allow space for thermal expansion to prevent pressure buildup. In fire protection systems, thermal expansion can alter the operation of liquid-based detectors or sprinkler systems, which rely on precise pressure balances.
Expansion of Gases
Gases expand significantly with temperature increases. According to gas laws, gas volume increases with temperature if pressure is constant. In enclosed systems, this can lead to pressure buildup, posing explosion risks. Firefighters must understand how pressurised gases behave under heat to manage cylinder storage, gas leak incidents, or confined fires safely.
Liquefaction of Gases
Gases can be liquefied by increasing pressure or decreasing temperature. Critical temperature is the maximum temperature at which a gas can be liquefied, regardless of pressure. Understanding this is vital when handling gases in cylinders, such as LPG or CO₂ used in firefighting systems. These gases are stored in liquefied form under pressure, and their behaviour under fire conditions must be carefully managed to prevent rupture or explosion.
Boyle’s Law
Boyle’s Law states that for a fixed mass of gas at constant temperature, the pressure is inversely proportional to volume. This is critical in compressed air systems and breathing apparatus. When a cylinder is opened and pressure drops, the volume of gas available to the user increases. Understanding this law helps in calculating safe operating durations for breathing gear.
Charles’s Law
Charles’s Law states that for a fixed mass of gas at constant pressure, the volume is directly proportional to its temperature. In firefighting, this explains how gas expansion occurs during heating, contributing to the rapid growth of fire and flashover conditions. It also impacts the safe storage and transport of gases.
Law of Pressures
The Law of Pressures relates to the total pressure exerted by a mixture of gases, stating that the total is the sum of the individual gas pressures. This is important when assessing environments filled with smoke and multiple combustion gases, which collectively increase pressure and toxicity. Gas monitors used by firefighters rely on this principle to assess atmosphere composition.
The General Gas Law
The General Gas Law combines Boyle’s and Charles’s Laws, showing the relationship between pressure, volume, and temperature. It helps firefighters predict how gases behave under varying fire conditions. This knowledge supports decisions about venting, containment, and the use of gas suppression systems.