Kinetics of Oxidation of Benzyl Alcohol with Dilute Nitric Acid

2005 ◽  
Vol 44 (2) ◽  
pp. 325-333 ◽  
Author(s):  
Sudhir R. Joshi ◽  
Kamal L. Kataria ◽  
Sudhirprakash B. Sawant ◽  
Jyeshtharaj B. Joshi
Keyword(s):  
Nitric Acid ◽  
Benzyl Alcohol ◽  
Kinetics Of Oxidation ◽  
Oxidation Of Benzyl Alcohol ◽  
Kinetics Of ◽  
Dilute Nitric Acid

scholarly journals Kinetics and Mechanism of Oxidation of Benzyl Alcohol by Benzimidazolium Fluorochromate

2008 ◽  
Vol 5 (4) ◽  
pp. 754-760
Author(s):  
J. Dharmaraja ◽  
K. Krishnasamy ◽  
M. Shanmugam
Keyword(s):  
Benzyl Alcohol ◽  
Sodium Perchlorate ◽  
Activation Parameters ◽  
Aqueous Acetic Acid ◽  
Hydrogen Ions ◽  
Acetic Acid Medium ◽  
Kinetics Of Oxidation ◽  
First Order ◽  
Oxidation Of Benzyl Alcohol ◽  
Kinetics Of

The kinetics of oxidation of benzyl alcohol (BzOH) by benzimidazolium fluorochromate (BIFC) has been studied in 50% aqueous acetic acid medium at 308 K. The reaction is first order with respect to [oxidant] and [benzyl alcohol]. The reaction is catalysed by hydrogen ions. The decrease in dielectric constant of the medium increases the rate of the reaction. Addition of sodium perchlorate increases the rate of the reaction appreciably. No polymerization with acrylonitrile. The reaction has been conducted at four different temperature and the activation parameters were calculated. From the observed kinetic results a suitable mechanism was proposed.

scholarly journals Kinetics and Mechanism of Slurry Phase Air Oxidation of Benzyl Alcohol over Zirconium Vanadate Catalyst

2020 ◽  
Vol 33 (1) ◽  
pp. 108-112
Author(s):  
Shweta Kanungo Joshi ◽  
Neena Sohani ◽  
Savita Khare ◽  
Rajendra Prasad
Keyword(s):  
Benzyl Alcohol ◽  
Kinetics And Mechanism ◽  
Air Oxidation ◽  
Redox Mechanism ◽  
Rate Law ◽  
Oxidation Of Benzyl Alcohol ◽  
Slurry Phase ◽  
Partial Pressures ◽  
Kinetics Of ◽  
Zirconium Vanadate

The kinetics of slurry phase air oxidation of benzyl alcohol to benzaldehyde over zirconium vanadate catalyst is reported in this study. Initial rates for the formation of product were determined by varying the partial pressures of the reactants. The data collected were found to satisfy a rate law: R = [(k1PBk2Po)/(k1PB + k2Po)]. The study suggests that reaction follows a Mars-Van Krevelen type of redox mechanism.

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