Robert J. Noll
- Courses2
- Reviews4
- School: Indiana State University
- Campus:
- Department: Chemistry & Physics
- Email address: Join to see
- Phone: Join to see
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Location:
200 N 7th St
Terre Haute, IN - 47809 - Dates at Indiana State University: April 2014 - December 2017
- Office Hours: Join to see
Biography
Indiana State University - Chemistry & Physics
Associate Professor at Indiana State University
Higher Education
Robert
Noll
Terre Haute, Indiana
Specialties: Physical and analytical chemistry, gas-phase reactions, mass spectrometry, chemometrics, spectroscopy. Developing some new interests in thermodynamics.
Experience
University of Wisconsin-Madison
Teaching Assistant
General Chemistry and Physical Chemistry
University of Wisconsin-Madison
Post-doctoral Research Associate
Robert worked at University of Wisconsin-Madison as a Post-doctoral Research Associate
Purdue University
Proposal Coordinator, Office of the Vice President for Research
Robert worked at Purdue University as a Proposal Coordinator, Office of the Vice President for Research
Purdue University
Associate Research Scientist
Research scientist in large analytical chemistry group. Conduct research on and develop novel mass spectrometry instrumentation, assist and supervise graduate students, write grant proposals, carry out administrative work.
Lawrence University, Appleton, WI
Assistant Professor
Tenure-track, Assistant Professor of Chemistry at small, nationally-ranked liberal arts college of 1200 students. Responsible for analytical and physical chemistry, including quantitative analysis and theory and experimental optical spectroscopy.
Indiana State University
Assistant Professor of Chemistry
Robert worked at Indiana State University as a Assistant Professor of Chemistry
Indiana State University
Associate Professor
Robert worked at Indiana State University as a Associate Professor
Education
Wooster High School
High School Diploma
Carleton College
B.A.
Chemistry
magna cum laude, graduated with distinction in major (Chemistry) and distinction in comprehensive exercise, Certificate of Advanced Study in German Language and LiteratureUniversity of Wisconsin-Madison
Ph.D.
Physical Chemistry
Studied ion/molecule reactions under single collision conditions using pulsed, crossed molecular beams. Used laser two-photon techniques to prepare metal cations in spin-orbit level specific electronic states. Extensive experience with ns lasers, vacuum techniques, high voltage methods, and fast (ns) signal acquisition, TOF-MS.University of Wisconsin-Madison
Teaching Assistant
General Chemistry and Physical ChemistryUniversity of Wisconsin-Madison
Post-doctoral Research Associate
Publications
Heat Evolution and Electrical Work of Batteries as a Function of Discharge Rate: Spontaneous and Reversible Processes and Maximum Work
Journal of Chemical Education
Many types of batteries power an ever-growing number of devices. Electrochemical devices like batteries and fuel cells can, in principle, exceed Carnot efficiency for energy conversion. In this novel laboratory experiment, students explore the partitioning of the enthalpy change of a battery’s electrochemical reaction between useful electrical work and waste heat, ΔH = welec + q. Work is measured by monitoring cell potential and current during battery discharge; waste heat evolved at the battery is simultaneously measured in a calorimeter. Results from discharging AA-size “alkaline” batteries are presented. Data for nickel–cadmium, nickel–metal hydride; a D-size, single cell, lead-acid storage battery; and Zn/Ag2O watch batteries are also presented in the Supporting Information. Keywords: Upper-Division Undergraduate, Physical Chemistry, Hands-On Learning/Manipulatives, Thermodynamics, Laboratory Instruction, Calorimetry/Thermochemistry, Electrochemistry, Electrolytic/Galvanic Cells/Potentials
Heat Evolution and Electrical Work of Batteries as a Function of Discharge Rate: Spontaneous and Reversible Processes and Maximum Work
Journal of Chemical Education
Many types of batteries power an ever-growing number of devices. Electrochemical devices like batteries and fuel cells can, in principle, exceed Carnot efficiency for energy conversion. In this novel laboratory experiment, students explore the partitioning of the enthalpy change of a battery’s electrochemical reaction between useful electrical work and waste heat, ΔH = welec + q. Work is measured by monitoring cell potential and current during battery discharge; waste heat evolved at the battery is simultaneously measured in a calorimeter. Results from discharging AA-size “alkaline” batteries are presented. Data for nickel–cadmium, nickel–metal hydride; a D-size, single cell, lead-acid storage battery; and Zn/Ag2O watch batteries are also presented in the Supporting Information. Keywords: Upper-Division Undergraduate, Physical Chemistry, Hands-On Learning/Manipulatives, Thermodynamics, Laboratory Instruction, Calorimetry/Thermochemistry, Electrochemistry, Electrolytic/Galvanic Cells/Potentials
Cross-Course Collaboration in the Undergraduate Chemistry Curriculum: Primary Kinetic Isotope Effect in the Hypochlorite Oxidation of 1-Phenylethanol in the Physical Chemistry Laboratory
Journal of Chemical Education
A kinetic isotope effect (KIE) experiment is described for the physical chemistry laboratory. Students conduct a hypochlorite (household bleach) oxidation of an equimolar mixture of 1-phenylethanol and 1-deuterio-1-phenylethanol to acetophenone. The reaction occurs in a biphasic reaction mixture and follows first-order kinetics with respect to either isotopomer of 1-phenylethanol. Reaction progress is measured by gas chromatography–mass spectrometry (GC–MS). Alternatively, the experiment could be conducted with each isotopomer serially and followed by GC alone. The reaction rate constant for the disappearance of 1-phenylethanol, kH, ranges from 3 × 10–4 to 2 × 10–3 s–1, while kD, for 1-deuterio-1-phenylethanol, ranges from 9 × 10–5 to 5 × 10–4 s–1. The observed KIE, the ratio kH/kD, is remarkably robust, ranging between 2.3 and 3.6, with a mean of 2.9 and standard deviation of 0.4 over three years of student data. The robustness of the observed KIE stems from using competing reactions. The experiment can be completed in about 3 h; GC–MS data is conveniently acquired overnight using an autosampler. The experiment, as presented here, can stand alone, but is well-suited to cross-course collaboration between the organic and physical chemistry laboratories. The preceding companion paper describes the synthesis of 1-phenylethanol and 1-deuterio-1-phenylethanol using borohydride or borodeuteride reduction of acetophenone as an experiment for the organic laboratory. Keywords: Upper Division Undergraduate, Laboratory Instruction, Physical Chemistry, Organic Chemistry, Collaborative/Cooperative Learning, Gas Chromatography, Isotopes, Kinetics, Mass Spectrometry, Mechanisms of Reactions
Heat Evolution and Electrical Work of Batteries as a Function of Discharge Rate: Spontaneous and Reversible Processes and Maximum Work
Journal of Chemical Education
Many types of batteries power an ever-growing number of devices. Electrochemical devices like batteries and fuel cells can, in principle, exceed Carnot efficiency for energy conversion. In this novel laboratory experiment, students explore the partitioning of the enthalpy change of a battery’s electrochemical reaction between useful electrical work and waste heat, ΔH = welec + q. Work is measured by monitoring cell potential and current during battery discharge; waste heat evolved at the battery is simultaneously measured in a calorimeter. Results from discharging AA-size “alkaline” batteries are presented. Data for nickel–cadmium, nickel–metal hydride; a D-size, single cell, lead-acid storage battery; and Zn/Ag2O watch batteries are also presented in the Supporting Information. Keywords: Upper-Division Undergraduate, Physical Chemistry, Hands-On Learning/Manipulatives, Thermodynamics, Laboratory Instruction, Calorimetry/Thermochemistry, Electrochemistry, Electrolytic/Galvanic Cells/Potentials
Cross-Course Collaboration in the Undergraduate Chemistry Curriculum: Primary Kinetic Isotope Effect in the Hypochlorite Oxidation of 1-Phenylethanol in the Physical Chemistry Laboratory
Journal of Chemical Education
A kinetic isotope effect (KIE) experiment is described for the physical chemistry laboratory. Students conduct a hypochlorite (household bleach) oxidation of an equimolar mixture of 1-phenylethanol and 1-deuterio-1-phenylethanol to acetophenone. The reaction occurs in a biphasic reaction mixture and follows first-order kinetics with respect to either isotopomer of 1-phenylethanol. Reaction progress is measured by gas chromatography–mass spectrometry (GC–MS). Alternatively, the experiment could be conducted with each isotopomer serially and followed by GC alone. The reaction rate constant for the disappearance of 1-phenylethanol, kH, ranges from 3 × 10–4 to 2 × 10–3 s–1, while kD, for 1-deuterio-1-phenylethanol, ranges from 9 × 10–5 to 5 × 10–4 s–1. The observed KIE, the ratio kH/kD, is remarkably robust, ranging between 2.3 and 3.6, with a mean of 2.9 and standard deviation of 0.4 over three years of student data. The robustness of the observed KIE stems from using competing reactions. The experiment can be completed in about 3 h; GC–MS data is conveniently acquired overnight using an autosampler. The experiment, as presented here, can stand alone, but is well-suited to cross-course collaboration between the organic and physical chemistry laboratories. The preceding companion paper describes the synthesis of 1-phenylethanol and 1-deuterio-1-phenylethanol using borohydride or borodeuteride reduction of acetophenone as an experiment for the organic laboratory. Keywords: Upper Division Undergraduate, Laboratory Instruction, Physical Chemistry, Organic Chemistry, Collaborative/Cooperative Learning, Gas Chromatography, Isotopes, Kinetics, Mass Spectrometry, Mechanisms of Reactions
Orbitrap Mass Spectrometry: Instrumentation, Ion Motion and Applications
Mass Spectrom. Rev.
Since its introduction, the orbitrap has proven to be a robust mass analyzer that can routinely deliver high resolving power and mass accuracy. Unlike conventional ion traps such as the Paul and Penning traps, the orbitrap uses only electrostatic fields to confine and to analyze injected ion populations. In addition, its relatively low cost, simple design and high space-charge capacity make it suitable for tackling complex scientific problems in which high performance is required. This review begins with a brief account of the set of inventions that led to the orbitrap, followed by a qualitative description of ion capture, ion motion in the trap and modes of detection. Various orbitrap instruments, including the commercially available linear ion trap–orbitrap hybrid mass spectrometers, are also discussed with emphasis on the different methods used to inject ions into the trap. Figures of merit such as resolving power, mass accuracy, dynamic range and sensitivity of each type of instrument are compared. In addition, experimental techniques that allow mass-selective manipulation of the motion of confined ions and their potential application in tandem mass spectrometry in the orbitrap are described. Finally, some specific applications are reviewed to illustrate the performance and versatility of the orbitrap mass spectrometers.
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