scholarly journals Studies on Metal Hydroxy Compounds. XIV. Thermal Analyses, Calorimetry, and Decomposition Kinetics of Heterocationic Hydroxy Chloride Compounds

1973 ◽  
Vol 51 (23) ◽  
pp. 3882-3888 ◽  
Author(s):  
Ah-Dong Leu ◽  
Palepu Ramamurthy ◽  
Etalo A. Secco
Keyword(s):  
Thermal Decomposition ◽  
Rate Equation ◽  
Thermal Analyses ◽  
General Pattern ◽  
Type Equation ◽  
First Order ◽  
Order Rate ◽  
Kinetics Of ◽  
Order Rate Equation ◽  
Initial Mode

Studies were carried out on two series of mixed metal hydroxy chloride compounds of the type xMe(OH)2•yMCl2 where Me = Cd, Cu and M = Mn, Co, Ni, Cu, Zn, Cd, Mg, or Ca.Thermal analyses for the Cd–M series reveal that the initial mode of decomposition involves a dehydroxylation step with a concomitant metathetical reaction between MCl2 and CdO. The compound CdCl2•2CdO is formed and decomposes at higher temperature leading to the eventual volatilization of CdCl2. The kinetics of thermal decomposition follow a simple first-order rate equation. The sole exception to this general pattern of behavior is the Cd–Zn compound.The initial mode of thermal decomposition of the Cu–M series compounds follows a parallel pattern described for the Cd–M series. The kinetic data for the Cu–M series are fitted into three groups: (i) phase boundary control embracing the contracting sphere and contracting plate model equations, (ii) A-E type equation with n = 2, and (iii) first-order rate equation.

The trans-Effect in Octahedral Complexes. VI. Base Hydrolysis of trans-Hydroxybromo and trans-Hydroxychlorobis(ethylenediamine)-rhodium(III) Complexes

1975 ◽  
Vol 53 (12) ◽  
pp. 1842-1848 ◽  
Author(s):  
Anthony Poë ◽  
Carol Vuik
Keyword(s):  
Rate Equation ◽  
Base Hydrolysis ◽  
Small Contribution ◽  
Trans Effect ◽  
First Order ◽  
Order Rate ◽  
Pseudo First Order ◽  
Kinetics Of ◽  
Hydrolysis Of ◽  
Order Rate Equation

The kinetics of base hydrolysis of the complexes trans-[Rh(en)2(OH)X]+ (X = Br or Cl) follow the pseudo first order rate equation kobs = k1 + k2[OH−]. The small contribution of the [OH−]-dependent term is due to lower values of ΔS2≠ − ΔS1≠ than are observed for the complexes cis-[Rh(en)2(OH)Cl]+ and [Rh(NH3)5X]2+ (X = Cl, Br, or I ). The values of ΔH1≠ are used to obtain new values of the intrinsickinetictrans-effect (i.k.t.e.) of hydroxide that agree with that determined from aquation of trans.-[Rh(en)2(OH)I]+ and place hydroxide in the i.k.t.e. series [Formula: see text] The new data also allow hydroxide to be placed in a thermodynamic trans-effect (t.t.e.) series I > OH > NH3 > Br > Cl > OH2, and the different position of hydroxide in the two series is discussed.

Studies on metal hydroxy compounds. X. Thermal analyses, decomposition kinetics, and infrared spectra of lead halide (Cl, Br, I) derivatives

1970 ◽  
Vol 48 (16) ◽  
pp. 2617-2622 ◽  
Author(s):  
P. Ramamurthy ◽  
E. A. Secco ◽  
M. Badri
Keyword(s):  
Infrared Spectra ◽  
Rate Equation ◽  
Thermal Analyses ◽  
Decomposition Reaction ◽  
Diffusion Type ◽  
Type Rate ◽  
Hydroxy Compounds ◽  
Kinetics Of ◽  
Lead Halide ◽  
Order Rate Equation

The thermal analyses, thermogravimetry (TG), and differential thermal analysis (DTA) of PbOHCl, PbOHBr, and PbOHI reveal that the initial mode of decomposition is via dehydroxylation. Calorimetric measurements along with related enthalpy values for the decomposition reaction are given.The infrared spectra of these compounds are interpreted in terms of folded bands of (PbOH+)n tied together by halide ions consistent with their crystal structures.The kinetics of thermal decomposition of lead hydroxyhalides follow a diffusion-type rate equation which is in contrast to the simple first-order rate equation observed for most Cd, Zn, and Cu compounds. These two distinct rates are interpreted in terms of mobile OH or H species in the dehydroxylation step.

THE REDUCTION OF CYTOCHROMEcBY HYDROQUINONE

1963 ◽  
Vol 41 (1) ◽  
pp. 231-237 ◽  
Author(s):  
G. R. Williams
Keyword(s):  
Reaction Mechanism ◽  
Ionic Strength ◽  
Rate Equation ◽  
Second Order ◽  
Order Rate ◽  
Ferricytochrome C ◽  
Kinetics Of ◽  
Kinetics Of Reduction ◽  
Order Rate Equation

The kinetics of reduction of ferricytochrome c by hydroquinone have been studied. The reaction does not conform to a simple second-order rate equation and it is demonstrated that the deviations are brought about by the presence of p-quinone, one of the products of the reaction. The accelerating effect of p-quinone is explained tentatively on the basis of an involvement of the semi-quinone. The effects on the reaction of pH, ionic strength, and temperature are reported and used to suggest features of the reaction mechanism.

THE REDUCTION OF CYTOCHROMEcBY HYDROQUINONE

1963 ◽  
Vol 41 (1) ◽  
pp. 231-237 ◽  
Author(s):  
G. R. Williams
Keyword(s):  
Reaction Mechanism ◽  
Ionic Strength ◽  
Rate Equation ◽  
Second Order ◽  
Order Rate ◽  
Ferricytochrome C ◽  
Kinetics Of ◽  
Kinetics Of Reduction ◽  
Order Rate Equation

The kinetics of reduction of ferricytochrome c by hydroquinone have been studied. The reaction does not conform to a simple second-order rate equation and it is demonstrated that the deviations are brought about by the presence of p-quinone, one of the products of the reaction. The accelerating effect of p-quinone is explained tentatively on the basis of an involvement of the semi-quinone. The effects on the reaction of pH, ionic strength, and temperature are reported and used to suggest features of the reaction mechanism.

Biosorption of Lignin Compounds Using Biomass Derived from Eichhornia crassipes: Batch Studies

2008 ◽  
Vol 6 (1) ◽  
Author(s):  
Renganathan Sahadevan ◽  
Ajit Balaji Kannavadi Devaraj ◽  
Dharmendira Kumar Mahendradas ◽  
Baskar Gurunathan ◽  
Manickam Velan
Keyword(s):  
Rate Equation ◽  
Eichhornia Crassipes ◽  
Second Order ◽  
Isotherm Model ◽  
Batch Studies ◽  
First Order ◽  
Order Rate ◽  
Pseudo Second Order ◽  
Pseudo First Order ◽  
Order Rate Equation

Biosorption of lignin compounds by the Eichhornia crassipes was investigated in batch studies. Batch experiments were conducted to study the effect of initial sorbent dosage, solution pH and lignin compounds concentration. Langmuir and Freundlich adsorption isotherm models were used to represent the equilibrium data. The Freundlich isotherm model was found to be fitted very well with the experimental data when compared to Langmuir isotherm model. The results showed that the equilibrium uptake capacity was found to be increased with decrease in biomass dosage. The lignin compound removal was influenced by the initial lignin compounds concentration. The sorption results were analysed for pseudo first order and pseudo second order kinetic model. It was observed that the kinetic data fitted very well with the pseudo second order rate equation when compared to the pseudo first order rate equation. Sorption results were analyzed for the intra particle diffusion model.

Development and application of a first order rate equation for modelling the dissolution of gold in cyanide solution

1991 ◽  
Vol 4 (12) ◽  
pp. 1305-1314 ◽  
Author(s):  
J. McLaughlin ◽  
G.E. Agar
Keyword(s):  
Rate Equation ◽  
Cyanide Solution ◽  
First Order ◽  
Order Rate ◽  
Order Rate Equation

On the kinetics of cellulose degradation: looking beyond the pseudo zero order rate equation

Cellulose ◽  
2007 ◽  
Vol 15 (2) ◽  
pp. 193-203 ◽  
Author(s):  
Paolo Calvini ◽  
Andrea Gorassini ◽  
Antonio Luigi Merlani
Keyword(s):  
Rate Equation ◽  
Cellulose Degradation ◽  
Zero Order ◽  
Order Rate ◽  
Kinetics Of ◽  
Order Rate Equation

THE KINETICS OF THE THERMAL DECOMPOSITION OF ETHYL BROMIDE AND ETHYL BROMIDE-d5

1958 ◽  
Vol 36 (7) ◽  
pp. 1043-1048 ◽  
Author(s):  
Arthur T. Blades
Keyword(s):  
Thermal Decomposition ◽  
Rate Constants ◽  
Pressure Effect ◽  
Ethyl Bromide ◽  
Carrier Gas ◽  
First Order ◽  
Order Rate ◽  
Kinetics Of

The kinetics of the pyrolysis of ethyl bromide and ethyl bromide-d5 have been studied using the toluene carrier gas technique. Variation of the pressure in the range 0.6 to 4.4 cm. Hg reveals what is believed to be a legitimate pressure effect on the first-order rate constants. The Arrhenius rate expressions determined at 4 cm. Hg pressure are: k(ethyl bromide) = 8.5 ± 1.6 × 1012e−52,200±300/RTsec−1 (T = 523°–633 °C);k(ethyl bromide-d5) = 2.1 ± 0.4 × 1013e−54,840±300/RT sec−1 (T = 531°–635 °C).The differences in the two rate expressions are discussed.

Calculator least squares evaluation of k for the first order rate equation

1978 ◽  
Vol 2 (1) ◽  
pp. 39-41 ◽  
Author(s):  
Delos F. Detar
Keyword(s):  
Least Squares ◽  
Rate Equation ◽  
First Order ◽  
Order Rate ◽  
Order Rate Equation
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