Thermal Decomposition of Tobacco: V. Influence of Temperature on the Formation of Carbon Monoxide and Carbon Dioxide

1975 ◽  
Vol 8 (2) ◽  
Author(s):  
H. R. Burton
Keyword(s):  
Carbon Dioxide ◽  
Thermal Decomposition ◽  
Carbon Monoxide ◽  
Influence Of Temperature ◽  
Influence Of Temperature On

AbstractThe temperature-yield profiles of CO and CO

Influence of temperature on the integral intensities of vibration-rotation absorption bands of water vapor and carbon dioxide

1981 ◽  
Vol 34 (3) ◽  
pp. 320-324 ◽  
Author(s):  
N. I. Moskalenko ◽  
Yu. A. Il'in ◽  
N. K. Pokotilo ◽  
S. A. Sementsov ◽  
V. T. Pushkin
Keyword(s):  
Carbon Dioxide ◽  
Water Vapor ◽  
Absorption Bands ◽  
Influence Of Temperature ◽  
Influence Of Temperature On ◽  
Vibration Rotation

Preparation of Nickel Nanoparticles by the Thermal Decomposition of NiC2O4. 2H2O Precursor in the Argon Gas

2011 ◽  
Vol 403-408 ◽  
pp. 3136-3139
Author(s):  
Xiao Ming Fu
Keyword(s):  
Thermal Decomposition ◽  
Particle Size ◽  
Nickel Powder ◽  
Nickel Nanoparticles ◽  
Crystal Water ◽  
Argon Gas ◽  
Influence Of Temperature ◽  
Pyrolytic Decomposition ◽  
Influence Of Temperature On ◽  
Two Stages

Nickel nanoparticles are successfully obtained by the pyrolytic decomposition of NiC2O4. 2H2O in the argon gas. The pyrolysates of NiC2O4. 2H2O in the argon gas are investigated by TG-DSC and TEM. The results show that there are two stages in the process of the pyrolytic decomposition of NiC2O4. 2H2O in the argon gas. The crystal water in NiC2O4. 2H2O is lost from 200 °C to 300 °C. NiC2O4 is pyrolysized into nickel powder from 325 °C to 425 °C. At the same time, the influence of temperature on the particle size of the decomposition is more from 254.4 °C to 407.5 °C. The influence of temperature on the particle size of the decomposition is less from 407.5 °C to 450.0 °C. Therefore, the pyrolytic condition of NiC2O4. 2H2O in the air is controlled if nickel nanoparticles are prepared.

scholarly journals Thermal decomposition of potassium titanium oxalate

2011 ◽  
Vol 76 (7) ◽  
pp. 1015-1026 ◽  
Author(s):  
Karuvanthodi Muraleedharan ◽  
Labeeb Pasha
Keyword(s):  
Carbon Dioxide ◽  
Thermal Decomposition ◽  
Carbon Monoxide ◽  
Model Fitting ◽  
Nitrogen Atmosphere ◽  
Single Step ◽  
Heating Rates ◽  
Decomposition Stage ◽  
Model Free ◽  
Good Agreement

The thermal decomposition of potassium titanium oxalate (PTO) was studied using non-isothermal thermogravimetry at different heating rates under a nitrogen atmosphere. The thermal decomposition of PTO proceeds mainly through five stages forming potassium titanate. The theoretical and experimental mass loss data are in good agreement for all stages of the thermal decomposition of PTO. The third thermal decomposition stage of PTO, the combined elimination of carbon monoxide and carbon dioxide, were subjected to kinetic analyses both by the method of model fitting and by the model free approach, which is based on the isoconversional principle. The model free analyses showed that the combined elimination of carbon monoxide and carbon dioxide and formation of final titanate in the thermal decomposition of PTO proceeds through a single step with an activation energy value of about 315 kJ mol-1.

THE THERMAL DECOMPOSITION OF CARBOHYDRATES

1948 ◽  
Vol 26b (4) ◽  
pp. 415-431 ◽  
Author(s):  
I. E. Puddington
Keyword(s):  
Carbon Dioxide ◽  
Thermal Decomposition ◽  
Carbon Monoxide ◽  
Reaction Temperature ◽  
Potato Starch ◽  
Second Step ◽  
Volatile Solids ◽  
Volatile Products ◽  
Separate Step ◽  
Rapid Reaction

The thermal decompositions of cellobiose, maltose, dextrose, and potato starch have been studied over a temperature range, by following the production of volatile products. Carbon dioxide, carbon monoxide, and water with small quantities of acids, aldehydes, and volatile solids were produced in all cases. With cellobiose, the first step of the reaction, which involved the elimination of two moles of water per mole of sugar, could be separated from the second step, where the oxides of carbon were produced, by controlling the reaction temperature. Dextrose first dimerized by a rapid reaction and then decomposed in much the same manner as cellobiose. The behavior of maltose was anomalous and no dehydration by a separate step could be detected. The decomposition of potato starch was similar to the second step of the cellobiose reaction.

THE THERMAL DECOMPOSITION OF PHENYLACETIC ACID

1960 ◽  
Vol 38 (8) ◽  
pp. 1261-1270 ◽  
Author(s):  
Margaret H. Back ◽  
A. H. Sehon
Keyword(s):  
Carbon Dioxide ◽  
Activation Energy ◽  
Thermal Decomposition ◽  
Carbon Monoxide ◽  
Rate Constant ◽  
Phenylacetic Acid ◽  
Order Process ◽  
First Order ◽  
Kinetics Of ◽  
Dissociation Step

The thermal decomposition of phenylacetic acid was investigated by the toluene-carrier technique over the temperature range 587 to 722 °C. The products of the pyrolysis were carbon dioxide, carbon monoxide, hydrogen, methane, dibenzyl, and phenylketene. From the kinetics of the decomposition it was concluded that the reaction[Formula: see text]was a homogeneous, first-order process and that the rate constant of this dissociation step was represented by the expression k = 8 × 1012.e−55,000/RT sec−1. The activation energy of this reaction may be identified with D(C6H5CH2—COOH). The possible reactions of carboxyl radicals are discussed.

The reaction of methanol vapour with silver(I) oxide

1964 ◽  
Vol 17 (5) ◽  
pp. 529
Author(s):  
JA Allen
Keyword(s):  
Carbon Dioxide ◽  
Thermal Decomposition ◽  
Carbon Monoxide ◽  
Gas Phase ◽  
Kinetic Data ◽  
Kcal Mole ◽  
Collision Model ◽  
Temperature Range ◽  
Methanol Vapour ◽  
The Mean

The reaction of methanol with silver(I) oxide has been studied in the temperature range 56.5-78.4�. For complete reduction of the oxide at 78.4�, the available oxygen is fully accounted for by the products, formaldehyde, formic acid, carbon monoxide, carbon dioxide, and water. In the temperature range 56.5-70.2� the net measured rates of formation of these products are expressed by equations of the form, ������������������ rate = Aexp(-E/RT), and the kinetic data are interpreted as the consecutive formation of the products on the surface without complete desorption to the gas phase between each step. For the dominant product, carbon dioxide, at the mean temperature the values of A and E are 1028.5 μg oxygen per minute and 41.3 kcal mole-1 respectively. The former is interpreted in terms of a simple collision model and the latter compared with values obtained for the thermal decomposition of the oxide.

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