Carbon dioxide specific heat

Fuel economy is measured usiag a carbon balance method calculation. The carbon content of the exhaust is calculated by adding up the carbon monoxide (qv), carbon dioxide (qv), and unbumed hydrocarbons (qv) concentrations. Then usiag the percent carbon ia the fuel, a volumetric fuel economy is calculated. If the heating value of the fuel is known, an energy specific fuel economy ia units such as km/MJ can be calculated as well. 

Available data on the thermodynamic and transport properties of carbon dioxide have been reviewed and tables compiled giving specific volume, enthalpy, and entropy values for carbon dioxide at temperatures from 255 K to 1088 K and at pressures from atmospheric to 27,600 kPa (4,000 psia). Diagrams of compressibiHty factor, specific heat at constant pressure, specific heat at constant volume, specific heat ratio, velocity of sound in carbon dioxide, viscosity, and thermal conductivity have also been prepared (5). 

At the other temperature extreme we have the measurements of specific heats executed at the temperatures of liquefied gases. A known mass of the substance is dropped into liquid carbon dioxide (— 78°), oxygen (— 183°), or hydrogen (— 250°), and the volume of gas liberated is measured. 

The method just described leads to the mean specific heats over a fairly large range. Nernst, Koref, and Lindemann (1910) have recently described a method of measuring the true specific heat at a given low temperature. The substance is contained in a block of copper cooled to the requisite temperature in liquid carbon dioxide, liquid air, etc., and energy is supplied by a heating spiral of platinum wire carrying an electric current, the measurement of the resistance of which serves at the same time to determine the temperature. 

A. Michels and J. Strijland, "The Specific Heat at Constant Volume of Compressed Carbon Dioxide , Physica, 18, 613-628 (1952). 

The penetration and cooling action of water is required with Class A fires, e.g. those involving paper, wood, textiles, refuse. Water is applied in the form of a jet or spray foam or multi-purpose powder extinguishers are alternatives. Extinguishment of a Class B fire can be achieved by the smothering action of dry chemical, carbon dioxide or foam. Most flammable liquids will float on water (refer to Table 6.1 under Specific gravity ), so that water as a jet is unsuitable a mist may, however, be effective. Water is also widely used to protect equipment exposed to heat. Dry powders are effective on flammable liquid or electrical fires. 

Polyacrylonitrile (C3H3N) bums to form vapor, carbon dioxide and nitrogen. The heat of formation of the polyacrylonitrile is +15.85 kcal/g mol (1 cal= 4.186 kJ). Use data from Tables 2.1 and 2.2 use specific heat values at 1000 K. 

Nitrogen dioxide can be identified by color, odor, and physical properties. It is dissolved in warm water and converted to nitric acid. The latter may be measured by acid-base titration or from analysis of nitrate ion by nitrate ion-specific electrode or by ion chromatography. Alternatively, nitrogen dioxide may be passed over heated charcoal to produce nitrogen and carbon dioxide that may be analysed by GC-TCD or GC/MS (See Nitrogen, Analysis). The characteristic masses for N2 and CO2 formed for their identification are 28 and 44, respectively. 

Scottish chemist, physicist, and physician. Professor of chemistry at Glasgow. He clearly characterized carbon dioxide ( fixed air ) as the gas which makes caustic alkalies mild, and distinguished between magnesia and lime. He discovered the latent heats of fusion and vaporization, measured the specific heats of many substances, and invented an ice calorimeter. 

Still another decomposition giving rise to ethylene oxide involves die pyrolysis f 0-hydrvjxyethyl -V,N-dialkylaminopolymethylehe carbamates. A specific illustration (Eq. 318) is -hydroxyethyl y-morpho-Kuopropyl carbamate, which on heating at 130-140° yields ethylene xide. carbon dioxide, and a urea derivative.4 Although interesting, this decomposition is of little preparative value in epoxide synthesis. 

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