Traduccion

The slope of this line gives the value of Kcat and the intercept is Knoncat (see eq3 ).Next construct a similar plot using the data collected at 1°C . The values of Kconcert. And Kcat at the twotemperatures are then used to calculate. Ea for the noncatalyzed and catalyzed reactions using the Arrhenius equation .
However, as stated in the background section, to determine the true Ea for thecatalyzed reaction, one must calculate KH while taking into account the value of K1 and its temperature dependence. Using Kcat = k1 KH and literature value of K1 at 25°C of 2,8x10-5, one finds thevalue of KH to be 8,5x103 L/mol-s (considerably higher than the k noncat values reported as y- intercept values in table 3). Next, using a literature value of H for the protonation of H2O2 ( + 17,6kj/mol), one obtains a K1 of 1,0 x10 -5 at 1°C, witch yields a KH at 1°C of 4,0 x103 L/mol.S. Comparing these values of KH lends to an Ea of 22Kj/mol for the true catalyzed reaction (eq 8)
Summary
It hasshown that this variation of the iodine clock reaction is a versatile experiment . It can be used to study reaction kinetics and the influence of a catalyst. Its unique feature is that one cancalculate the activation energy of the acid- catalyzed reaction independent of the noncatalyzed reaction that is occurring simultaneously . This experiment also provides the advantages of minimal chemicaland equipment requirements and the ability to cater to a variety of levels of students
La pendiente de esta línea da el valor de Kcat y la intersección esKnoncat (ver EQ3). A continuación construiruna gráfica similar conlos datos recogidos a 1 ° C. Los valores de Kconcert. Y Kcat en las dos temperaturas se utilizan entonces para calcular. Ea para la reacción catalizadapor noncatalyzed y utilizando la ecuación de Arrhenius.
Sin embargo, como se indica en la sección de antecedentes, para determinar la Ea cierto para la reacción catalizada, se debe calcular KH teniendo en cuenta el valor...