The Specific Heat Equations for Carbon Dioxide, Carbon Monoxide, Steam, Hydrogen, and Oxygen and the Free Energy Equation for the Water-Gas Reaction

1942 ◽  
Vol 82 (1) ◽  
pp. 397
Author(s):  
M. deKay Thompson
Keyword(s):  
Carbon Dioxide ◽  
Carbon Monoxide ◽  
Free Energy ◽  
Specific Heat ◽  
Energy Equation ◽  
Heat Equations ◽  
Water Gas

THE DECOMPOSITION OF ETHYL ALCOHOL OVER SOME POLY-COMPONENT CATALYSTS

1934 ◽  
Vol 10 (6) ◽  
pp. 743-758 ◽  
Author(s):  
E. H. Boomer ◽  
H. E. Morris
Keyword(s):  
Carbon Dioxide ◽  
Carbon Monoxide ◽  
Ethyl Alcohol ◽  
Quantitative Data ◽  
Carbon Oxides ◽  
Liquid Products ◽  
Secondary Reactions ◽  
Water Gas ◽  
Alcohol Alcohol ◽  
Hydrogenation Of Ethylene

Numerous experiments have been carried out on the decomposition of alcohol, alcohol and water, and alcohol and carbon dioxide mixtures over poly-component catalysts at temperatures up to 500 °C. Quantitative data on the gaseous and the liquid products were obtained. The properties of the poly-component catalysts, as evidenced by the simple primary and secondary reactions, have been shown to be qualitatively those of the single components.Methane can be produced in one or more of several secondary reactions, namely, the decomposition of acetaldehyde, the hydrogenation of carbon oxides and the decomposition of ethylene. Ethane can be produced in one or both of two reactions consisting of auto-oxidation and reduction of the alcohol, or the secondary hydrogenation of ethylene, confirming previous work. Carbon dioxide, in most cases, is formed as a result of the water-gas reaction and the decomposition of carbon monoxide. In other cases its origin is obscure. The results of certain experiments in which carbon dioxide and hydrogen were the major constituents of the off-gas cannot be explained in the same way. Reactions involving ketene decomposition and polymerization, and hydration of alcohol, have been suggested as possible explanations.

scholarly journals The determination of the specific heat of gases at high temperatures by the sound velocity method II—Carbon dioxide

1936 ◽  
Vol 156 (889) ◽  
pp. 504-517 ◽  
Keyword(s):  
Carbon Dioxide ◽  
Carbon Monoxide ◽  
Specific Heat ◽  
Sound Velocity ◽  
Quartz Crystal ◽  
Wave System ◽  
Sound Waves ◽  
Heated Tube ◽  
Specific Heats

In a previous paper an account was given of experiments to determine the specific heats of carbon monoxide up to a temperature of 1800° C. by the sound velocity method. The principle of the method employed was the setting up in a heated tube of a stationary train of sound waves; the source of the wave system being a quartz crystal vibrating piezo-electrically at a known frequency.

scholarly journals The kinetics of the reactions of the steam-carbon system

1946 ◽  
Vol 187 (1009) ◽  
pp. 129-151 ◽  
Keyword(s):  
Carbon Dioxide ◽  
Carbon Monoxide ◽  
Fractional Order ◽  
Kinetic Scheme ◽  
Correct Form ◽  
Different Types ◽  
Carbon Dioxide Reaction ◽  
Water Gas ◽  
Kinetics Of ◽  
Carbon System

The kinetics of the various individual reactions which may occur in the steam-carbon system have been studied. The pressures of the separate gases have been varied in the range 10-760 mm. Essentially similar results have been obtained with coconut shell charcoal at 700° C and coal charcoal at 800° C. The steam-carbon reaction, the primary product of which is carbon monoxide, is of fractional order with respect to steam and strongly retarded by hydrogen. The carbon dioxide-carbon reaction is of fractional order with respect to carbon dioxide and strongly retarded by carbon monoxide. The rates of both these reactions can be represented closely by an expression of the form rate = k 1 p 1 /1 + k 2 p 2 + k 3 p 1 where p 1 and p 2 are respectively the pressures of steam and hydrogen for the steam reaction, and of carbon dioxide and carbon monoxide for the carbon dioxide reaction. This kinetic scheme provides a consistent interpretation of the apparently conflicting results of previous work under a variety of conditions with many different types of carbon. Further experimental work, however, is necessary to elucidate without ambiguity the mechanisms of these reactions. The water-gas reaction, CO + H 2 O = CO 2 + H 2 , takes place predominantly on the charcoal surface, and the approach to equilibrium has been studied from both sides. The forward reaction is of nearly the first order with respect to carbon monoxide and of fractional order with respect to steam; it is retarded by hydrogen and to a lesser extent by carbon dioxide. The reverse reaction is of fractional order with respect to both carbon dioxide and hydrogen, retarded by steam and unaffected by carbon monoxide. The kinetic expressions for the forward and reverse components of this heterogeneous reversible reaction combine to give the thermodynamically correct form of the equilibrium constant.

scholarly journals Investigation of the Effects of Steam Injection on Equilibrium Products and Thermodynamic Properties of Diesel and Biodiesel Fuels

2020 ◽  
Vol 2020 ◽  
pp. 1-14
Author(s):  
Jean Paul Gram Shou ◽  
Marcel Obounou ◽  
Timoléon Crépin Kofané ◽  
Mahamat Hassane Babikir
Keyword(s):  
Nitric Oxide ◽  
Carbon Dioxide ◽  
Carbon Monoxide ◽  
Thermodynamic Properties ◽  
Specific Heat ◽  
Steam Injection ◽  
Combustion Products ◽  
Waste Cooking Oil ◽  
Cooking Oil ◽  
Biodiesel Fuels

The effects of steam injection on combustion products and thermodynamic properties of diesel fuel, soybean oil-based biodiesel (NBD), and waste cooking oil biodiesel (WCOB) are examined in this study by considering the chemical equilibrium. The model gives equilibrium mole fractions, specific heat of the exhaust mixtures of 10 combustion products, and adiabatic flame temperatures. The results show that the mole fractions of carbon monoxide (CO) and carbon dioxide (CO2) decrease with the steam injection ratios. Nitric oxide (NO) mole fractions decrease with the steam injections ratios for lean mixtures. The specific heat of combustion products increases with the steam injection ratios. The equilibrium combustion products obtained can be used to calculate the nonequilibrium values of NO in the exhaust gases using some existing correlations of NO kinetics.

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