HYDROGEN PEROXIDE AND ITS ANALOGUES: IV. SOME THERMAL PROPERTIES OF HYDROGEN PEROXIDE

1951 ◽  
Vol 29 (10) ◽  
pp. 895-903 ◽  
Author(s):  
William T. Foley ◽  
Paul A. Giguère
Keyword(s):  
Hydrogen Peroxide ◽  
Thermal Properties ◽  
Heat Of Fusion ◽  
Pure Hydrogen ◽  
Platinum Black ◽  
Concentrated Solutions ◽  
Heat Of Vaporization ◽  
Freezing Points ◽  
A Value ◽  
Thermal Data

Using a Bunsen ice calorimeter the following thermal data were obtained for pure hydrogen peroxide:Specific heat of liquid between0°and25°C …................... 0.632 ± 0. 003 cal. per.gm. per degreeSpecific heat of solid between−20°and −10°C.................. 0.41 ± 0.02 cal. per gm. per degreeLatent heat of fusion at meltingpoint, −0.46°C................... 85.83 ± 0.18 cal. per gm.Latent heat of vaporization at 0°C...... 370.17 ± 0.18 cal. per gm.The freezing points of very concentrated solutions of hydrogen peroxide calculated from these data agree closely with the experimental ones. Preliminary measurements of the heat of decomposition of hydrogen peroxide catalyzed by platinum black were also made at 0° and at various concentrations. The results point to 23.54 ± 0.04 kcal. per mole for the heat of the reaction[Formula: see text]a value slightly higher than those found by previous experimenters.

scholarly journals THE DECOMPOSITION OF HYDROGEN PEROXIDE BY LIVER CATALASE

1928 ◽  
Vol 11 (4) ◽  
pp. 309-337 ◽  
Author(s):  
John Williams
Keyword(s):  
Hydrogen Peroxide ◽  
Catalytic Decomposition ◽  
Hydrogen Ion ◽  
Ion Concentration ◽  
Concentrated Solutions ◽  
Hydrogen Ion Concentration ◽  
A Value ◽  
Optimum Ph ◽  
Adsorption Of Hydrogen ◽  
New Interpretation

1. The velocity of decomposition of hydrogen peroxide by catalase as a function of (a) concentration of catalase, (b) concentration of hydrogen peroxide, (c) hydrogen ion concentration, (d) temperature has been studied in an attempt to correlate these variables as far as possible. It is concluded that the reaction involves primarily adsorption of hydrogen peroxide at the catalase surface. 2. The decomposition of hydrogen peroxide by catalase is regarded as involving two reactions, namely, the catalytic decomposition of hydrogen peroxide, which is a maximum at the optimum pH 6.8 to 7.0, and the "induced inactivation" of catalase by the "nascent" oxygen produced by the hydrogen peroxide and still adhering to the catalase surface. This differs from the more generally accepted view, namely that the induced inactivation is due to the H2O2 itself. On the basis of the above view, a new interpretation is given to the equation of Yamasaki and the connection between the equations of Yamasaki and of Northrop is pointed out. It is shown that the velocity of induced inactivation is a minimum at the pH which is optimal for the decomposition of hydrogen peroxide. 3. The critical increment of the catalytic decomposition of hydrogen peroxide by catalase is of the order 3000 calories. The critical increment of induced inactivation is low in dilute hydrogen peroxide solutions but increases to a value of 30,000 calories in concentrated solutions of peroxide.

THE REFRACTIVE INDICES OF HYDROGEN PEROXIDE AND ITS AQUEOUS SOLUTIONS

1943 ◽  
Vol 21b (8) ◽  
pp. 156-162 ◽  
Author(s):  
Paul A. Giguère
Keyword(s):  
Hydrogen Peroxide ◽  
Refractive Index ◽  
Aqueous Solutions ◽  
Accurate Method ◽  
Refractive Indices ◽  
Pure Hydrogen ◽  
A Value ◽  
Concentration Of Solutions ◽  
Hydrogen Lines ◽  
Good Agreement

The refractive indices of aqueous solutions of hydrogen peroxide for the C-, F-, and G-lines of hydrogen and the sodium D-line have been measured over the whole range of concentration at four temperatures: 16°, 20°, 24°, and 28 °C. The results obtained with the hydrogen lines are somewhat different from those of Cuthbertson and Maass. A possible explanation of this discrepancy is given. By extrapolation it was found that for pure hydrogen peroxide nD = 1.4087 at 20°, a value in good agreement with previous determinations. The refractive index affords a rapid and fairly accurate method for determining the concentration of solutions of hydrogen peroxide.

HYDROGEN PEROXIDE: THE LOW TEMPERATURE HEAT CAPACITY OF THE SOLID AND THE THIRD LAW ENTROPY

1954 ◽  
Vol 32 (2) ◽  
pp. 117-128 ◽  
Author(s):  
Paul A. Giguère ◽  
I. D. Liu ◽  
J. S. Dugdale ◽  
J. A. Morrison
Keyword(s):  
Hydrogen Peroxide ◽  
Heat Capacity ◽  
Low Temperature ◽  
Adiabatic Calorimeter ◽  
Ideal Gas ◽  
Heat Of Fusion ◽  
A Value ◽  
Two Samples ◽  
Thermal Measurements ◽  
Heat Capacity Measurements

The heat capacity of crystalline hydrogen peroxide between 12° K. and the melting point has been determined with a low temperature adiabatic calorimeter. The heat of fusion was also measured and found to be 2987 ± 3 cal./mole. The two samples of hydrogen peroxide used were 99.97 mole % pure as deduced from behavior on melting and from premelting heat capacities; the triple point was estimated to be 272.74 K.The only anomaly observed in the heat capacity measurements was the absorption of 1.3 cal./mole at 216.8 ± 0.15° K., the lower eutectic temperature of H2O-H2O2 solutions. Such an effect is to be expected if the only significant impurity is water. The entropy of hydrogen peroxide as an ideal gas at 1 atm. pressure and 25° C. computed from the thermal measurements is 55.76 ± 0.12 cal./mole deg. Comparison of this datum with the recalculated statistical entropy leads to a value of 3.5 kcal./mole for the height of a hypothetical single barrier hindering internal rotation in the molecule. From these results it is concluded that hydrogen peroxide does not consist of two tautomeric modifications.

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

Zn:Tl PHASE DIAGRAM AT VERY LOW THALLIUM CONCENTRATIONS

1961 ◽  
Vol 39 (4) ◽  
pp. 588-595 ◽  
Author(s):  
E. H. McLaren ◽  
F. Weinberg
Keyword(s):  
Phase Diagram ◽  
Freezing Point ◽  
Solubility Limit ◽  
Heat Of Fusion ◽  
Kcal Mole ◽  
Solid Solubility Limit ◽  
Pure Zinc ◽  
Latent Heat Of Fusion ◽  
A Value ◽  
Resistance Thermometry

The Zn:Tl liquidus has been accurately determined from pure Zn (419.505 °C) to the monotectic transition temperature (416.926 °C at 0.42 at.% Tl) using precision resistance thermometry. The upper solidus was determined approximately from measurements of the distribution coefficient (~0.01) and the solid solubility limit (~0.004 at.% Tl) of thallium in zinc. A value 1.53 ± 0.1 kcal/mole for the latent heat of fusion of pure zinc was calculated from the freezing point depressions.

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.

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