The thermal decomposition of hydrogen peroxide vapour

1959 ◽  
Vol 55 ◽  
pp. 548 ◽  
Author(s):  
D. E. Hoare ◽  
J. B. Protheroe ◽  
A. D. Walsh
Keyword(s):  
Hydrogen Peroxide ◽  
Thermal Decomposition

THE THERMAL DECOMPOSITION OF HYDROGEN PEROXIDE VAPOR

1968 ◽  
Author(s):  
K. R. Bilwakesh ◽  
W. A. Strauss ◽  
R. Edse ◽  
E. S. Fishburne
Keyword(s):  
Hydrogen Peroxide ◽  
Thermal Decomposition ◽  
Hydrogen Peroxide Vapor

THE THERMAL DECOMPOSITION OF HYDROGEN PEROXIDE VAPOUR. II.

1947 ◽  
Vol 25b (2) ◽  
pp. 135-150 ◽  
Author(s):  
Paul A. Giguère
Keyword(s):  
Activation Energy ◽  
Hydrogen Peroxide ◽  
Thermal Decomposition ◽  
Low Temperatures ◽  
Hydrocyanic Acid ◽  
Quartz Surface ◽  
First Order ◽  
Acid Washing ◽  
Reaction Vessels ◽  
Low Pressures

The decomposition of hydrogen peroxide vapour has been investigated at low pressures (5 to 6 mm.) in the temperature range 50° to 420 °C., for the purpose of determining the effect of the nature and treatment of the active surfaces. The reaction was followed in an all-glass apparatus and, except in one case, with one-litre round flasks as reaction vessels. Soft glass, Pyrex, quartz, and metallized surfaces variously treated were used. In most cases the decomposition was found to be mainly of the first order but the rates varied markedly from one vessel to another, even with vessels made of the same type of glass. On a quartz surface the decomposition was preceded by an induction period at low temperatures. Fusing the glass vessels slowed the reaction considerably and increased its apparent activation energy; this effect was destroyed by acid washing. Attempts to poison the surface with hydrocyanic acid gave no noticeable result. The marked importance of surface effects at all temperatures is considered as an indication that the reaction was predominantly heterogeneous under the prevailing conditions. Values ranging from 8 to 20 kcal. were found for the apparent energy of activation. It is concluded that the decomposition of hydrogen peroxide vapour is not very specific as far as the nature of the catalyst is concerned.

The Thermal Decomposition of Gaseous Hydrogen Peroxide

1937 ◽  
Vol 59 (2) ◽  
pp. 422-422 ◽  
Author(s):  
G. B. Kistiakowsky ◽  
S. L. Rosenberg
Keyword(s):  
Hydrogen Peroxide ◽  
Thermal Decomposition ◽  
Gaseous Hydrogen

Thermal Decomposition of Hydrogen Peroxide in the Vapour Phase

Nature ◽  
1949 ◽  
Vol 163 (4153) ◽  
pp. 876-877 ◽  
Author(s):  
A. B. HART
Keyword(s):  
Hydrogen Peroxide ◽  
Thermal Decomposition ◽  
Vapour Phase

A Model for Thermal Decomposition of Hydrogen Peroxide

2004 ◽  
Author(s):  
Jeremy Corpening ◽  
Stephen Heister ◽  
Willam Anderson ◽  
Benjamin Austin
Keyword(s):  
Hydrogen Peroxide ◽  
Thermal Decomposition

Synthese und Kristallstruktur von Dinatrium-di-μ/-oxo-bis[trihydroxo-methylantimonat(V)] / Synthesis and Crystal Structure of Disodium-di-μ-oxo-bis[trihydroxo-methylantimonate(V)]

1991 ◽  
Vol 46 (2) ◽  
pp. 139-142 ◽  
Author(s):  
Markus Wieber ◽  
Udo Simonis ◽  
Dieter Kraft
Keyword(s):  
Crystal Structure ◽  
Aqueous Solution ◽  
Hydrogen Peroxide ◽  
Thermal Decomposition ◽  
Sodium Hydroxide ◽  
Spectroscopic Properties ◽  
Membered Ring ◽  
Dimeric Molecule ◽  
Synthesis And Crystal Structure

The oxidation of dialkoxymethylstibine with hydrogen peroxide in the presence of sodium hydroxide leads to the formation of disodium-di-μ-oxo-bis[trihydroxo-methylantimonate(V)]. The salt can be synthesized also by dissolving methanestibonic acid in an aqueous solution of sodium hydroxide. The crystal structure has been determined; it shows a dimeric molecule containing a four-membered ring with Sb -O -Sb linkages. Thermal decomposition and spectroscopic properties o f the com pound are discussed.

Photolysis of hydrogen peroxide, photocatalytic effects of Cu(II) and reaction kinetics

1986 ◽  
Vol 51 (5) ◽  
pp. 973-981 ◽  
Author(s):  
Stanislav Luňák ◽  
Petr Sedlák ◽  
Josef Vepřek-Šiška
Keyword(s):  
Hydrogen Peroxide ◽  
Thermal Decomposition ◽  
Quantum Yield ◽  
Reaction Kinetics ◽  
Copper Ions ◽  
Oxidation States ◽  
Radiation Temperature ◽  
Quantum Yields ◽  
High Quantum ◽  
Catalytically Active

The quantum yield of hydrogen peroxide photolysis has been measured as a function of the concentration of photocatalytically active Cu2+ ions, intensity of photolytic radiation, temperature, and hydrogen peroxide concentration. The results obtained are consistent with the concept that high quantum yields of hydrogen peroxide photolysis (Φ >> 1) are due to thermal decomposition of hydrogen peroxide catalyzed by photochemically generated copper ions in oxidation states which are catalytically active.

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