Energy release table

Table 14.9 Likely energy released at different magnitudes of an earthquake...

Some environmentalists have also touted natural gas as a way station on the road to a hydrogen fuel (carbon dioxide-free) economy. As seen in Table 1, per unit of energy released, natural gas generates about 23 percent less carbon dioxide than gasoline and about 30 percent less than heavy fuel oil. This is helpful in reducing greenhouse emissions, but the other excellent properties of natural gas are even... 

When one considers the potential high-energy release on rupture of a carborane unit, together with the thermodynamic stability of combustion products, it is hardly surprising that there is a body of literature that reports on the use of carbo-ranes within propellant compositions. Their use in energetic applications is to be expected when the enthalpy of formation (AH/) data for the products of combustion for boron are compared to those of carbon. Thermodynamic data for the enthalpy of formation of o-carborane and of typical boron and carbon combustion products is shown in Table 4. Measurements of the standard enthalpy of combustion32 for crystalline samples of ortho-carborane show that complete combustion is a highly exothermic reaction, AH = — 8994 KJmol. ... 

U-shaped curve, we have mixtures that can be ignited for a sufficiently high spark energy. From Equation (4.25) and the dependence of the kinetics on both temperatures and reactant concentrations, it is possible to see why the experimental curve may have this shape. The lowest spark energy occurs near the stoichiometric mixture of XCUi =9.5%. In principle, it should be possible to use Equation (4.25) and data from Table 4.1 to compute these ignitability limits, but the complexities of temperature gradients and induced flows due to buoyancy tend to make such analysis only qualitative. From the theory described, it is possible to illustrate the process as a quasi-steady state (dT/dt = 0). From Equation (4.21) the energy release term represented as... 

A burning rate of common materials and products in fire can only be specifically and accurately established through measurement. Estimates from various sources are listed in Table 9.4. Also, oxygen consumption calorimeters are used to measure the energy release rate of complex fuel packages directly. In most cases, the results are a combination of effects ignition, spread and burning rate. 

TABLE 2.4 Structure of High Energy Release Compounds ... 

The enthalpy A W((lcUi is the energy required to melt 1 mol of material at constant pressure. We need to be careful when obtaining data from tables, because many books cite the enthalpy of fusion, which is the energy released during the opposite process of solidification. We do not need to worry, though, because we know from Hess s law that AH elt) = — A//( lsion). The molar enthalpy of melting water is +6.0 kJmol-1. 

Table 1. The critical mass and energy released in the conversion process of an HS into a QS for several values of the Bag constant and the surface tension. Column labeled MQs,max denotes the maximum gravitational mass of the final QS sequence. The value of the critical gravitational mass of the initial HS is reported on column labeled Mcr whereas those of the mass of the final QS and the energy released in the stellar conversion process are shown on columns labeled Mfi and Econv respectively. BH denotes those cases in which the baryonic mass of the critical mass configuration is larger than the maximum baryonic mass of the QS sequence (M r > MQS>max). In these cases the stellar conversion process leads to the formation of a black hole. Units of B and a are MeV/fm3 and MeV/fm2 respectively. All masses are given in solar mass units and the energy released is given in units of 10B1 erg. The hadronic phase is described with the GM1 model, ms and as are always taken equal to 150 MeV and 0 respectively. The GM1 model predicts a maximum mass for the pure HS of 1.807 M .

The more recent editions of NFPA 704 provide some objective criteria (Table 5) for assignment of ratings. The degree of instability hazard is ranked based on ease, rate, and quantity of energy release of the substance (NFPA, 1996). Onset temperature, instantaneous power density (IPD Hofelich et al.,... 

Chemical reactions have two independent properties, their energy and their rate. Table 1-8-2 compares these two properties. AG represents the amount of energy released or required per mole of reactant. The amount or sign of AG indicates nothing about the rate of the reaction. 

Table 2.3 Energy released on oxidation of one gram of the major fuels...

The data in the two previous tables do permit some complex calculations of energy for changes of both state and temperature. Take a mole of water vapor at 100° C and cool it to ice at 0°. The energy released, which must be removed by the refrigeration process, comes from three distinct changes listed in Table 7-4. 

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