Publication

Conversion and shrinkage analysis of acrylated hyperbranched polymer nanocomposites

Yves Leterrier, Valérie Geiser
2009
Journal Articles

Résumé

The photo-curing behavior of composites containing nanosized SiO2 in an acrylated hyperbranched polymer matrix was investigated by means of photo differential scanning calorimetry. The chemical conversion data were analyzed using an autocatalytic model, paying close attention to the influence of composition and UV intensity. It was shown that the reaction order and the autocatalytic exponent were independent of UV intensity and filler fraction, whereas the rate constant showed strong intensity dependence, but weak filler dependence. Maximum conversion was independent of UV intensity, but was reduced when a filler was present. The dispersion state influenced the gel-point of the composites, but had no influence on the overall cure kinetics. Cure shrinkage reduction of ~33% could be achieved by adding 20 vol% of filler. This was attributed to the reduced double bond conversion of the matrix due to the presence of the filler. © 2009 Wiley Periodicals, Inc. J Appl Polym Sci 114: 1954–1963, 2009

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https://infoscience.epfl.ch/entities/publication/a8a2ff89-da05-4d7e-b305-b6d5727019cb

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Yves Leterrier, Valérie Geiser
2009
Journal Articles

Résumé

Source officielle

https://infoscience.epfl.ch/entities/publication/a8a2ff89-da05-4d7e-b305-b6d5727019cb

À propos de ce résultat

Concepts associés (16)

Mécanisme réactionnel

En chimie, un mécanisme réactionnel est l'enchainement d'étapes, de réactions élémentaires, par lequel un changement chimique a lieu. Bien que, pour la plupart des réactions, seul le bilan global (transformation des réactifs en produits) soit observable directement, des expériences permettent de déterminer la séquence possible des étapes du mécanisme réactionnel associé. Un mécanisme réactionnel décrit en détail ce qui se passe à chaque étape d'une transformation chimique.

Reaction rate

The reaction rate or rate of reaction is the speed at which a chemical reaction takes place, defined as proportional to the increase in the concentration of a product per unit time and to the decrease in the concentration of a reactant per unit time. Reaction rates can vary dramatically. For example, the oxidative rusting of iron under Earth's atmosphere is a slow reaction that can take many years, but the combustion of cellulose in a fire is a reaction that takes place in fractions of a second.

Rate equation

In chemistry, the rate law or rate equation for a chemical reaction is a mathematical equation that links the rate of forward reaction with the concentrations or pressures of the reactants and constant parameters (normally rate coefficients and partial reaction orders). For many reactions, the initial rate is given by a power law such as where [\mathrm{A}] and [\mathrm{B}] express the concentration of the species \mathrm{A} and \mathrm{B}, usually in moles per liter (molarity, M).

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