1 / 40

Fires and Explosions

Fires and Explosions. Fires and Explosions. Definitions Flammability Flash Points Flammability limits Mixtures Temperature Dependence Pressure Dependence Minimum Oxygen Concentration Minimum Ignition Energy Adiabatic Compression Ignition Sources. Introduction.

edda
Download Presentation

Fires and Explosions

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Fires and Explosions

  2. Fires and Explosions • Definitions • Flammability • Flash Points • Flammability limits • Mixtures • Temperature Dependence • Pressure Dependence • Minimum Oxygen Concentration • Minimum Ignition Energy • Adiabatic Compression • Ignition Sources

  3. Introduction • We have been talking about source models for the release of materials and about dispersion models if the material is a toxicant. • Another concern is a release of flammable materials where we need to worry about fires and explosions.

  4. Fire Triangle • Most are familiar with the Fire Triangle. • In order for a fire to start or be sustained you need to have a Fuel, an oxidizer and an ignition source. • If one of the three components is eliminated, then there will not be a fire (or explosion)

  5. Fuel • Fuel must be present in certain concentrations. • Typical cases where fuel occur are if there is a leak, during filling operations, transfer operations, or excessive dusts. • Although we often cannot always eliminate these sources we can help by having good ventilation to keep vapors from building up. • Often we locate things out-doors, use grating on floors so vapors don’t build up.

  6. Oxidizers • Oxygen is the most common oxidizer, especially that found in ambient air. • For oxygen, we often use “inerting” with nitrogen, helium blankets over flammable materials to reduce O2 content below that where you can have combustion.

  7. Ignition Sources • Heat is a common ignition source. • “Ignition sources are free!!!” • Although we can eliminate ignition sources, it is almost inevitable that an ignition source will be available if there is a large release of flammable material that cannot be diluted quickly.

  8. Fire Tetrahedron • The fire tetrahedron or fire pyramid adds a fourth component—chemical chain reaction—as a necessity in the prevention and control of fires. • The free radicals formed during combustion are important intermediates in the initiation and propagation of the combustion reaction. Fire suppression materials scavenge these free radicals

  9. Definitions • Combustion – a chemical reaction in which a substance combines with an oxidizer and releases energy. • Explosion – rapid expansion of gases resulting in a rapid moving pressure or shock wave. • Mechanical Explosion – due to failure of vessel with high pressure non reactive gas.

  10. Explosions • Detonation – explosion (chemical reaction) with shock wave greater than speed of sound • Deflagration – explosion (chemical reaction) with shock wave less than speed of sound • BLEVE – Boiling Liquid Expanding Vapor Explosion – when liquid is at a temperature above its atmospheric boiling point. Vessel ruptures – flammable liquid flashes and results in a fire/explosion

  11. Explosions • Confined explosion – an explosion occurring within a vessel or a building. Usually results in injury to the building inhabitants and extensive damage. • Unconfined explosion – an explosion occurring in the open. Usually results from spill of a flammable gas spill. These explosions are rarer than confined since dilution occurs.

  12. Explosions • Dust Explosions - This explosion results from the rapid combustion of fine solid particles. Many solid materials become very flammable when reduced to a fine powder.

  13. Fires and Explosions • Definitions • Flammability • Flash Point • Flammability limits • Mixtures • Temperature Dependence • Pressure Dependence • Minimum Oxygen Concentration • Minimum Ignition Energy • Adiabatic Compression • Ignition Sources

  14. Flammability • Flash Point (FP) – a property of material used to determine the fire and explosive hazard. The lowest temperature of a liquid at which it gives off enough vapor to form an ignitable mixture with air. • Needs to be determined experimentally. • Different methods to determine, open cup and closed cup. Open cup is usually a few degrees higher.

  15. National Fire Protection AssociationFlammability classification • Flammable IA – Flash point < 73°F, boiling point < 100 °F • Flammable IB – Flash point < 73°F, boiling point > 100 °F • Flammable IC – 73°F < Flash point < 100 °F • Combustible II – 100 °F < Flash point < 140 °F • Combustible IIIA – 140 °F < Flash point < 200 °F • Combustible IIIB – Flash point > 200 °F

  16. Mixture Flash Points • Flash Points of mixtures can be estimated only IF one of the components is flammable. If more than one is flammable then need to determine experimentally. • For mixtures: • Determine the temperature at which the vapor pressure of the flammable in the liquid is equal to the pure component vapor pressure at its flash point.

  17. Mixture Flash Points • Example • Methanol FP=54°F, Vapor Pressure @ 54°F is 62 mmHg Determine the flash point of a solution that is 75wt% MeOH in water. Solution: Since only one component is flammable, can estimate mixture FP:

  18. Mixture Flash Point Example Continued

  19. Mixture Flash Point Example Continued

  20. Flammability Limits • There is usually a range of compositions of a flammable vapor and air where combustion occurs. • Too little fuel (lean mixture) not enough fuel to burn. • Too much fuel (rich mixture) not enough oxygen to burn

  21. Flammability Limits • Table 6-1 gives upper flammability limits and lower flammability limits for several common substances. • Experimentally determined. • LFL can be estimated from Flash Point:.

  22. Mixture Flammability Limits • If you have a mixture of flammable components you can calculate Lower Flammability Limit of the mixture LFLmixusing Le Chatelier’s relationship:

  23. Mixture Flammability Limits • You can also calculate an Upper Flammability Limit of the mixture UFLmixusing Le Chatelier’s relationship:

  24. Flammability Limits – Temperature effect • Table 6-1 gives flammability limits for 25°C and atmospheric pressure. If you are at a different temperature you can modify flammability limits

  25. Flammability Limits – Pressure effects • LFL is not affected by pressure • UFL does depend on the pressure • Procedure • Correct for Temperature • Correct for Pressure • Calculate for mixture

  26. Fires and Explosions • Definitions • Flammability • Flash Points • Flammability limits • Mixtures • Temperature Dependence • Pressure Dependence • Minimum Oxygen Concentration • Minimum Ignition Energy • Adiabatic Compression • Ignition Sources

  27. Minimum Oxygen Concentration (MOC) • LFL is based on “air” but actually it is O2 that is important. Often in industry they “inert” to dilute the O2 concentration. • Below the MOC the reaction cannot generate enough energy to heat the entire mixture to the extent required for self propagation.

  28. MOC

  29. Fires and Explosions • Definitions • Flammability • Flash Points • Flammability limits • Mixtures • Temperature Dependence • Pressure Dependence • Minimum Oxygen Concentration • Minimum Ignition Energy • Adiabatic Compression • Ignition Sources

  30. Minimum Ignition Energy (MIE) • Minimum energy input needed to initiate combustion • Most hydrocarbons have low MIE~0.25 mJ • Whereas the “spark” from walking across the room is 22mJ (almost 100X too much) • Again, we always assume that an ignition source will exist • Table 6-2 gives MIEs for some substances

  31. Fires and Explosions • Definitions • Flammability • Flash Points • Flammability limits • Mixtures • Temperature Dependence • Pressure Dependence • Minimum Oxygen Concentration • Minimum Ignition Energy • Adiabatic Compression • Ignition Sources

  32. Adiabatic Compression • When gases are compressed they heat up and can ignite (this is how a diesel engine works, also the cause of “knocking” in gasoline engines) • The adiabatic temperature rise is:

  33. Fires and Explosions • Definitions • Flammability • Flash Points • Flammability limits • Mixtures • Temperature Dependence • Pressure Dependence • Minimum Oxygen Concentration • Minimum Ignition Energy • Adiabatic Compression • Ignition Sources

  34. Ignition Sources • Ignition sources are free!!! • Table 6-3 gives the results of a study by Factory Mutual Engineering Corporation who studied over 25,000 industrial fires to determine the source of ignition.

  35. In Class Problem What is the UFL of a gas mixture composed of 1% methane, 2% ethane and 3% propane by volume at 50°C and 2 atmospheres: Data: Component MW Heat of Combustion (kcal/mol) Methane 16.04 212.79 Ethane 30.07 372.81 Propane 44.09 526.74

  36. Solution • Procedure: • Correct for temperature • Correct for pressure (only for UFL) • Find for mixture.

  37. Solution • Correction for Temperature : UFL from Table 6-1

  38. Solution cont. • Correction for Pressure (UFL only)

  39. Solution cont. • Mixture calculation • Equation 6-2 for mixtures

  40. Solution Continued Since total combustibles in air 1+2+3=6 < 18 then the system is in the combustible range (below UFL)

More Related