An Introduction to Fire Dynamics, Third Edition by Dougal Drysdale(auth.)

By Dougal Drysdale(auth.)

Content material:
Chapter 1 hearth technological know-how and Combustion (pages 1–34):
Chapter 2 warmth move (pages 35–82):
Chapter three Limits of Flammability and Premixed Flames (pages 83–119):
Chapter four Diffusion Flames and fireplace Plumes (pages 121–179):
Chapter five regular Burning of beverages and Solids (pages 181–223):
Chapter 6 Ignition: The Initiation of Flaming Combustion (pages 225–275):
Chapter 7 unfold of Flame (pages 277–315):
Chapter eight Spontaneous Ignition inside Solids and Smouldering Combustion (pages 317–348):
Chapter nine The Pre?Flashover Compartment hearth (pages 349–386):
Chapter 10 The Post?Flashover Compartment fireplace (pages 387–439):
Chapter eleven Smoke: Its Formation, Composition and flow (pages 441–474):

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Extra info for An Introduction to Fire Dynamics, Third Edition

Example text

4), provided that the product m ˙ · Af · χ is known. This is seldom the case for fires burning in enclosures, but the rate may be estimated if the rate of air inflow (m ˙ air ) is known. 2). The only situation where it is reasonable to ignore heat loss (at least to a first approximation) is in premixed burning, when the fuel and air are intimately mixed and the reaction rates are high, independent of diffusive or mixing processes. This is the ‘adiabatic’ model, in which it is assumed that none of the heat generated within the system is lost to the environment, thus producing the maximum theoretical rise in temperature.

27 g of air for stoichiometric burning to CO2 and water. 11). More generally, we can write: 1 kg fuel + r kg air → (1 + r) kg products where r is the stoichiometric air requirement for the fuel in question. 2. The stoichiometric air requirement can be used to estimate the heat of combustion of any fuel, if this is not known. 13. R7) define the stoichiometry of the complete reaction but hide the complexity of the overall process. 16 Mechanism of the gas-phase oxidation of methane (after Bowman, 1975) H• H• H• + + + CH4 CH4 CH4 CH4 O2 • CH3 CH2 O CH2 O CH2 O H2 H2 • CHO • CHO • CHO CO • OH H• O2 + + + + + + + + + + + + + + + + + + M OH H• • • O H• O2 • • O • OH H• • • O • OH • • O • OH H• • OH M M M • = = = = = = = = = = = = = = = = = = • CH3 CH3 • CH3 • CH3 • • O CH2 O • CHO • CHO • CHO H• H• CO CO CO CO2 H2 O H2 HO•2 • + + + + + + + + + + + + + + + + + + H• H2 O H2 • OH • OH • OH • OH H2 O H2 • OH H2 O • OH H2 O H2 H• M M M + M a b c d e f g h i j k l m n o p q r This reaction scheme is by no means complete.

Assuming that there is no heat loss (the system is adiabatic), the quantity of heat released is calculated from the temperature rise of the calorimeter and its contents, whose thermal capacities are accurately known. R4). The difference between the enthalpy change ( H ) and the internal energy change ( U ) exists because at constant pressure some of the chemical energy is effectively lost as work done (P V ) in the expansion process. e. 18) U are negative. 5) where n is the number of moles of gas involved.

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