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Miller, Tierney C.; Richardson, John N.; Kegerreis, Jeb S. – Journal of Chemical Education, 2016

This manuscript presents an exercise that utilizes mathematical software to explore Fourier transforms in the context of model quantum mechanical systems, thus providing a deeper mathematical understanding of relevant information often introduced and treated as a "black-box" in analytical chemistry courses. The exercise is given to…

Descriptors: Science Instruction, Mathematics, Computer Software, Educational Technology

Perez-Benito, Joaquin F. – Journal of Chemical Education, 2017

The elementary reaction sequence A ? I ? Products is the simplest mechanism for which the steady-state and quasi-equilibrium kinetic approximations can be applied. The exact integrated solutions for this chemical system allow inferring the conditions that must fulfill the rate constants for the different approximations to hold. A graphical…

Descriptors: Chemistry, Kinetics, Scientific Concepts, Graduate Study

Srnec, Matthew N.; Upadhyay, Shiv; Madura, Jeffry D. – Journal of Chemical Education, 2017

In undergraduate physical chemistry, Schrödinger's equation is solved for a variety of cases. In doing so, the energies and wave functions of the system can be interpreted to provide connections with the physical system being studied. Solving this equation by hand for a one-dimensional system is a manageable task, but it becomes time-consuming…

Descriptors: Undergraduate Study, College Science, Chemistry, Science Instruction

Rittenhouse, Robert C. – Journal of Chemical Education, 2015

The "atoms first" philosophy, adopted by a growing number of General Chemistry textbook authors, places greater emphasis on atomic structure as a key to a deeper understanding of the field of chemistry. A pivotal concept needed to understand the behavior of atoms is the restriction of an atom's energy to specific allowed values. However,…

Descriptors: Science Instruction, Chemistry, Undergraduate Study, College Science

Hladky, Paul W. – Journal of Chemical Education, 2011

College students encounter a variety of first-order phenomena in their mathematics and science courses. Introductory chemistry textbooks that discuss first-order processes, usually in conjunction with chemical kinetics or radioactive decay, stop at single, discrete dose events. Although single-dose situations are important, multiple-dose events,…

Descriptors: Textbooks, Kinetics, Chemistry, Radiation

Contreras-Ortega, C.; Bustamante, N.; Guevara, J. L.; Portillo, C.; Kesternich, V. – Journal of Chemical Education, 2007

A general mathematical treatment for chemical systems is described that might help students to better understand the real scope of the mathematical equations. The extent to which an equation acceptably describes a chemical system is determined from the limiting values of practical chemical variables and the concordance value defined by given…

Descriptors: Equations (Mathematics), Chemistry, Science Instruction, College Science

Desjardins, Steven G. – Journal of Chemical Education, 2008

In this paper we describe an interdisciplinary course on dynamics that is appropriate for nonscience majors. This course introduces ideas about mathematical modeling using examples based on pendulums, chemical kinetics, and population dynamics. The unique emphasis for a nonmajors course is on chemical reactions as dynamical systems that do more…

Descriptors: Majors (Students), Kinetics, Chemistry, Spreadsheets

Herrington, Deborah G. – Journal of Chemical Education, 2011

A substantial number of upper-level science students and practicing physical science teachers demonstrate confusion about thermal equilibrium, heat transfer, heat capacity, and specific heat capacity. The traditional method of instruction, which involves learning the related definitions and equations, using equations to solve heat transfer…

Descriptors: Definitions, Chemistry, Heat, Science Laboratories

Vargas, Francisco M. – Journal of Chemical Education, 2014

The temperature dependence of the Gibbs energy and important quantities such as Henry's law constants, activity coefficients, and chemical equilibrium constants is usually calculated by using the Gibbs-Helmholtz equation. Although, this is a well-known approach and traditionally covered as part of any physical chemistry course, the required…

Descriptors: Computation, Climate, Energy, Chemistry

DePierro, Ed; Garafalo, Fred; Toomey, Rick – Journal of Chemical Education, 2008

This paper summarizes difficulties that chemistry students at all levels commonly exhibit when translating, manipulating, and interpreting mathematical expressions that contain logarithms, and offers approaches that the authors have found useful to help students overcome such difficulties. The online supplement provides problem sets created by the…

Descriptors: Advanced Students, Problem Sets, Chemistry, Equations (Mathematics)

Darvesh, Katherine V. – Journal of Chemical Education, 2013

The equilibrium between phases is a key concept from the introductory physical chemistry curriculum. Phase diagrams display which phase is the most stable at a given temperature and pressure. If more than one phase has the lowest Gibbs energy, then those phases are in equilibrium under those conditions. An activity designed to demonstrate the…

Descriptors: Science Instruction, College Science, Equations (Mathematics), Graphs

Hijnen, Hens – Journal of Chemical Education, 2009

A theoretical description of the influence of electroosmosis on the effective mobility of simple ions in capillary zone electrophoresis is presented. The mathematical equations derived from the space-charge model contain the pK[subscript a] value and the density of the weak acid surface groups as parameters characterizing the capillary. It is…

Descriptors: Prediction, Equations (Mathematics), Science Instruction, Chemistry

Struyf, Jef – Journal of Chemical Education, 2011

The boiling point of a monofunctional organic compound is expressed as the sum of two parts: a contribution to the boiling point due to the R group and a contribution due to the functional group. The boiling point in absolute temperature of the corresponding RH hydrocarbon is chosen for the contribution to the boiling point of the R group and is a…

Descriptors: Organic Chemistry, Mathematical Formulas, Demonstrations (Educational), Investigations

Williams, Brian Wesley – Journal of Chemical Education, 2010

The mathematical Lambert function W[a exp(a - bt)] is used to find integrated rate laws for several examples, including simple enzyme and Lindemann-Christiansen-Hinshelwood (LCH) unimolecular decay kinetics. The results derived here for the well-known LCH mechanism as well as for a dimer-monomer reaction mechanism appear to be novel. A nonlinear…

Descriptors: Kinetics, Biochemistry, Science Instruction, Equations (Mathematics)

Glaser, Rainer E.; Delarosa, Marco A.; Salau, Ahmed Olasunkanmi; Chicone, Carmen – Journal of Chemical Education, 2014

Mathematical methods are described for the determination of steady-state concentrations of all species in multiequilibria systems consisting of several acids and their conjugated bases in aqueous solutions. The main example consists of a mixture of a diprotic acid H[subscript 2]A, a monoprotic acid HB, and their conjugate bases. The reaction…

Descriptors: Chemistry, Equations (Mathematics), Computation, College Science