Chemical reaction, iodine, propanon, rate equation, pharmaceutical industry, acid catalyst, Reactant Concentrations, Overall Rate
Knowing the kinetics of chemical reactions is critical in fields such as pharmaceuticals and materials engineering. Kinetics are the quantity that allows the optimization of a process and manufacturing effective products. By calculating reaction rates, scientists can understand those reactions via mechanisms and kinetics that distinguish reaction rates from their influencing factors (Miller et al., 2021). Various parameters can modulate the reaction rate, making such reactions more or less volatile; these include the concentration of reactants, temperature, pressure, and the presence of catalysts (Noël et al., 2023). These elements are as critical as enzymes and cofactors for product reaction rate and formation. Likewise, in the pharmaceutical industry, understanding the rate of a drug synthesis reaction is vital to the production of medications and the efficiency and cost-effectiveness of its production.
[...] Experimental Determination of Rate Equation for Iodine-Propanone Reaction Introduction Knowing the kinetics of chemical reactions is critical in fields such as pharmaceuticals and materials engineering. Kinetics are the quantity that allows the optimization of a process and manufacturing effective products. By calculating reaction rates, scientists can understand those reactions via mechanisms and kinetics that distinguish reaction rates from their influencing factors (Miller et al., 2021). Several parameters can modulate reaction rate, making such reactions more or less volatile; these include the concentration of reactants, temperature, pressure, and the presence of catalysts (Noël et al., 2023). [...]
[...] [CH3COCH3] is the concentration of propanone. Conclusion The experiments to calculate the rate equation of the iodine and propanone reaction reveal that the reaction is first-order concerning hydrogen ions, between first and second-order concerning propanone and zero-order concerning iodine. Overall, it was found that the rate of the reaction was second-order. The proposed rate law, Rate = k[H+][CH3COCH3], has been derived based on the above-observed findings and established the basis for a further investigation of the kinetics of this reaction. References Miller, J. [...]
[...] et al., 2021). When running tests 1 and conducted at different iodine concentrations, no considerable difference in reaction rate was detected, provided that other reactant concentrations were kept constant. This reflection indicates a simple kinetic dependency on the iodine concentration, which suggests it is a zero-order reaction with respect to iodine. Order of Reaction for Each Component Regarding HCl, the order in reaction corresponds to first-order, and doubling the concentration of HCl in experiment 2 led to almost doubling the reaction rate. [...]
[...] https://doi.org/10.1039/d3sc00992k Sajid, M., & P?otka-Wasylka, J. (2022). Green analytical chemistry metrics: A review. Talanta https://doi.org/10.1016/j.talanta.2021.123046 Tran Hong Thai, Nguyen Anh Dai, & Pham Tuan Anh. (2021). Global dynamics of some system of second-order difference equations. Electronic Research Archive, 4159-4175. [...]
[...] H., Raghu Sivaramakrishnan, T., Y., C. Franklin Goldsmith, Burke, M. G., Jasper, A. W., Hansen, N., Labbé, N., Glarborg, P., & Judit Zádor. (2021). Combustion chemistry in the twenty-first century: Developing theory-informed chemical kinetics models 100886-100886. https://doi.org/10.1016/j.pecs.2020.100886 Noël, T., Capaldo, L., & Wen, Z. (2023). A field guide to flow chemistry for synthetic organic chemists. Chemical Science, 14(16), 4230-4247. [...]
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