Abstract
Abstract The stoichiometry of equations was revisited in light of the Law of Conservation of Matter at an atomic, elemental level. For a balanced chemical equation following the simplest general model aA → bB, the fact that a b = n A n B ${a \over b} = {{{n_A}} \over {{n_B}}}$ , where nA is the number of moles of A consumed and nB is the number of moles of B produced in the reaction during the experiment, was used to address the de Donder relation, introduced by Theophile de Donder (1873–1957). While crediting the Belgian scientist for pointing out that “the reaction-ratio method” may be utilized for stoichiometry, the inverse de Donder relation was applied to problems in reaction stoichiometry. Several examples were used to show that the latter relation can be used to form proportions in order to rapidly solve such stoichiometry problems and to do so with fundamental chemical understanding. Educators in general chemistry were encouraged to teach the discussed method in their courses.
Highlights
The most fundamental chemical observation of the 18th century, stated by Antoine Lavoisier (1743–1794), is the law of mass conservation (Silberberg & Amateis, 2018), called the Law of Conservation of Matter
Several examples were used to show that the latter relation can be used to form proportions in order to rapidly solve such stoichiometry problems and to do so with fundamental chemical understanding
Which is a on the two sides of the clear example of the de latter proportion may be inversed in order to yield Donder relation (Tykodi, 1987), which is that for the general balanced equation α1A1 + α2A2 + ... → β1B1 + β2B2 + ..., the numbers of moles of the reactants consumed and the products produced in the reaction during the experiment are related according to the following: nA1 α1
Summary
The most fundamental chemical observation of the 18th century, stated by Antoine Lavoisier (1743–1794), is the law of mass conservation (Silberberg & Amateis, 2018), called the Law of Conservation of Matter. Several examples were used to show that the latter relation can be used to form proportions in order to rapidly solve such stoichiometry problems and to do so with fundamental chemical understanding. According to DeToma (1994), in the article “Symbolic Algebra and Stoichiometry” published in Journal of Chemical Education, the 1994 trend in modern general chemistry textbooks was to treat basic problems in reaction stoichiometry as a part of a class “to be done exclusively by factor-label methods.” The current trend seems to be the same.
Sign-in/Register to view highlights & summary Talk to us
Join us for a 30 min session where you can share your feedback and ask us any queries you have
Schedule a callDisclaimer: All third-party content on this website/platform is and will remain the property of their respective owners and is provided on "as is" basis without any warranties, express or implied. Use of third-party content does not indicate any affiliation, sponsorship with or endorsement by them. Any references to third-party content is to identify the corresponding services and shall be considered fair use under The CopyrightLaw.
