Physical properties of pure hydrogen peroxide

1974 ◽  
Vol 51 (7) ◽  
pp. 470
Author(s):  
Paul A. Giguere
Keyword(s):  
Hydrogen Peroxide ◽  
Physical Properties ◽  
Pure Hydrogen

Production of Pure Hydrogen Peroxide Solutions in Water Activated by Plasma of an Electrodeless Microwave Discharge and Their Application for Controlling Plant Growth

2019 ◽  
Vol 64 (5) ◽  
pp. 222-224
Author(s):  
S. N. Andreev ◽  
L. M. Apasheva ◽  
M. Kh. Ashurov ◽  
N. A. Lukina ◽  
B. Sapaev ◽  
...  
Keyword(s):  
Hydrogen Peroxide ◽  
Plant Growth ◽  
Microwave Discharge ◽  
Pure Hydrogen

Studies on hydrogen–oxygen systems in the electrical discharge. III. Surface effects

1970 ◽  
Vol 48 (13) ◽  
pp. 2042-2046 ◽  
Author(s):  
Paul E. Brunet ◽  
Xavier Deglise ◽  
Paul A. Giguère
Keyword(s):  
Hydrogen Peroxide ◽  
Water Vapor ◽  
Power Level ◽  
Surface Effects ◽  
Surface Coatings ◽  
Pure Hydrogen ◽  
Pyrolysis Products ◽  
Electrodeless Discharge ◽  
Oxygen Gas ◽  
Hydrogen Peroxide Vapor

Surface effects in the reactions of dissociated hydrogen–oxygen systems and the products condensed therefrom have been investigated. Water vapor at about 0.1 Torr was streamed at high velocity through an electrodeless discharge confined in tubes of different materials or with various surface coatings. In all cases the products trapped in liquid nitrogen evolved oxygen gas on warming, but the relative amounts varied considerably from one type of surface to another. In some cases there was clear evidence that the walls of discharge tube were attacked by hydrogen atom bombardment. The decomposition, both thermal and electrical, of pure hydrogen peroxide vapor was studied likewise. The pyrolysis products gave off very little oxygen on warming. By contrast the products from electrical decomposition, even at low power level, evolved much oxygen, most of it above the melting point.It is concluded that there is always some decomposition of hydrogen peroxide in the trapped products. However, this does not seem sufficient to account for all the evolved oxygen; at least not in the case of dissociated water vapor.

THE PROPERTIES OF PURE HYDROGEN PEROXIDE. VI

1929 ◽  
Vol 51 (3) ◽  
pp. 674-687 ◽  
Author(s):  
G. L. Matheson ◽  
O. Maass
Keyword(s):  
Hydrogen Peroxide ◽  
Pure Hydrogen

THE PROPERTIES OF PURE HYDROGEN PEROXIDE. II.

1920 ◽  
Vol 42 (12) ◽  
pp. 2569-2570 ◽  
Author(s):  
O. Maass ◽  
O. W. Herzberg
Keyword(s):  
Hydrogen Peroxide ◽  
Pure Hydrogen

THE THERMAL DECOMPOSITION OF HYDROGEN PEROXIDE VAPOUR

1945 ◽  
Vol 23b (5) ◽  
pp. 167-182 ◽  
Author(s):  
Bruce E. Baker ◽  
C. Ouellet
Keyword(s):  
Hydrogen Peroxide ◽  
Temperature Coefficient ◽  
Pure Hydrogen ◽  
First Order ◽  
Soda Glass ◽  
Manometric Method ◽  
Apparent Activation Energies ◽  
Reaction Vessels ◽  
First Time ◽  
Kinetics Of

The kinetics of the decomposition of hydrogen peroxide in the vapour state have been studied by a manometric method, with pure hydrogen peroxide at a concentration of about 99.5%. The temperature coefficient of the reaction has been measured for the first time. The pressures ranged from 1 to 2 cm. of mercury and the temperatures from 70° to 200 °C. Pyrex reaction vessels of various sizes and shapes, and also a fused Pyrex and a soda-glass vessel, were used. The reaction was purely heterogeneous, of the first order up to 140 °C. but more complicated at higher temperatures. Identical vessels yielded consistent results. The rates were not affected by air, carbon dioxide, or water vapour, but they varied greatly with the size and shape of the vessel. The reaction was very slow on fused Pyrex and very rapid on soda-glass. In one vessel, the temperature coefficient became negligible above 120 °C. No explosion was detected up to 335 °C. at a pressure of 18 cm. of mercury. The apparent activation energies in various vessels ranged from 13.5 to 18.5 kcal. per mole. A tentative reaction mechanism is suggested.

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