Chemical Kinetics
K.D. Zerna
Department of Chemical Engineering, College of Engineering, University of the Philippines, Diliman, Quezon City 1101
Performed 29 January 2019; Submitted 7 February 2019
ABSTRACT
The obj
...
Chemical Kinetics
K.D. Zerna
Department of Chemical Engineering, College of Engineering, University of the Philippines, Diliman, Quezon City 1101
Performed 29 January 2019; Submitted 7 February 2019
ABSTRACT
The objective of this experiment is to describe the kinetics of the reaction of S2O82- and I- through observing
how the rate of the reaction is influenced by concentration, temperature and the presence of a catalyst.
Seven solutions were prepared for the three parts of the experiment. The first part had five runs each with
varying concentrations of the reagents, the second part involved subjecting the system into different
temperature conditions and the third part involved the addition of a catalyst. For all three parts, the
reaction rate as well as the rate constant was calculated. From the data obtained in terms of concentration,
the reaction can be defined by the differential rate law: 𝑟𝑎𝑡𝑒 = 0.0112[𝑆2𝑂82-]1.112[𝐼-]1.0572. Through
varying the temperatures of the setups, it is observed that ln k is inversely proportional to the reciprocal of
the temperature in Kelvin which shows that as temperature is increased, the rate constant also increases.
Applying the correlations to the Arrhenius equation, the calculated activation energy (Ea) and Arrhenius
constant for the reaction are 68.9812 kJ/mol and 1.75971x1010, respectively. Given all the kinetic
parameters to define the kinetics of the given reaction, it can be affirmed and concluded that concentration,
temperature and the presence of a catalyst significantly alters the rate of the reaction.
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