@article{wjce2014222,
author={{Wu, Ya Hong and Tong, Shan Ling and Hu, Sheng and Wu, Mao Ying and Hao, Zhi Feng and Yan, Yan},
title={Thermodynamics and Kinetics, Possibility and Actuality},
journal={World Journal of Chemical Education},
volume={2},
number={2},
pages={26--28},
year={2014},
url={http://pubs.sciepub.com/wjce/2/2/2},
abstract={A typical kinetic experiment, the persulfate¨Ciodide clock reaction, is selected as an example to illustrate applications of thermodynamic possibility and kinetic actuality in chemical reactions. In the experiment, the strongest reducer, sodium thiosulfate Na<SUB>2</SUB>S<SUB>2</SUB>O<SUB>3</SUB><SUB>,</SUB> cannot be directly oxidized by the strongest oxidizer ammonium persulfate (NH<SUB>4</SUB>)<SUB>2</SUB>S<SUB>2</SUB>O<SUB>8</SUB>, and this redox must be realized by an intermediate iodine I<SUB>2</SUB> [presenting in I<SUB>3</SUB><SUP>-</SUP> anion, a weaker oxidizer than (NH<SUB>4</SUB>)<SUB>2</SUB>S<SUB>2</SUB>O<SUB>8</SUB>]. After I<SUB>2</SUB> molecules being reduced by Na<SUB>2</SUB>S<SUB>2</SUB>O<SUB>3</SUB> molecules to form I<SUP>-</SUP> ions (a weaker reducer than S<SUB>2</SUB>O<SUB>3</SUB><SUP>2-</SUP>), the strongest oxidizer begins to oxidize the weaker reducer I<SUP>-</SUP> ions to form I<SUB>2</SUB> molecules again, which is keeping on the redox circles until the stronger reducer Na<SUB>2</SUB>S<SUB>2</SUB>O<SUB>3</SUB> has been exhausted completely. Why the strongest reducer was not being oxidized by the strongest oxidizer? In this paper we attempt to explain this situation based on the chemical theories of thermodynamics and kinetics.},
doi={10.12691/wjce-2-2-2}
publisher={Science and Education Publishing}
}