Judd Christian F. Bañas
This experiment investigates the rate of the chemical reaction involving the decomposition of sodium thiosulfate (Na2S2O3) and hydrochloric acid (HCl) to form colloidal sulfur particles (S), sulfur dioxide (SO2), water (H2O), and sodium chloride (NaCl). The objective was to explore the rate constant (k) as a function of temperature and the reaction rate's dependence on reactant concentration over time. Methodologically, the reaction was modeled to ascertain its order, revealing it as second order, and the activation energy (Ea) was calculated using the Arrhenius equation based on reaction rates monitored at various temperatures. Results indicated the activation energy of the reaction to be 27.3 kJ with a rate constant (k) of 0.2046 M−1s−1. The experiment elucidated how concentration and temperature affect the rate of reaction, thereby enhancing the understanding of the kinetics of the sodium thiosulfate and hydrochloric acid reaction.
@article{afc995a9-3097-4460-9e07-e29dc07a2a90,
title={2-Kinetics: Rates of Chemical Reactions},
author={Judd Christian F. Bañas},
year={2024},
language={en}
}TY - JOUR TI - 2-Kinetics: Rates of Chemical Reactions AU - Judd Christian F. Bañas PY - 2024 LA - en ER -
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