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Electrochemical engineering is the branch of chemical engineering dealing with the technological applications of electrochemical phenomena, such as electrosynthesis of chemicals, electrowinning and refining of metals, flow batteries and fuel cells, surface modification by electrodeposition, electrochemical separations and corrosion.
Electroanalytical methods are a class of techniques in analytical chemistry which study an analyte by measuring the potential and/or current in an electrochemical cell containing the analyte.
The electrochemical cell voltage is also referred to as electromotive force or emf. A cell diagram can be used to trace the path of the electrons in the electrochemical cell. For example, here is a cell diagram of a Daniell cell: Zn(s) | Zn 2+ (1 M) || Cu 2+ (1 M) | Cu(s) First, the reduced form of the metal to be oxidized at the anode (Zn) is ...
The course is usually run with a concurrent lab section that gives students an opportunity to experience a laboratory environment and carry out experiments with the material learned in the course. These labs can consist of acid-base titrations, kinetics, equilibrium reactions, and electrochemical reactions.
After working in Liebig's laboratory, Horsford returned to the United States and helped establish the Lawrence Scientific School at Harvard University. The school was modeled after Liebig's methodology and established the first chemistry laboratory course. Two years later, Charles W. Eliot started to volunteer at the laboratory. Eliot's ...
The department offers undergraduate and graduate programs leading to the degree of chemical engineering: Bachelor of Science in Chemical Engineering (BS ChE) — five-year program leading to the understanding of transport processes, chemical engineering thermodynamics and their applications to unit operations design, thermodynamics and reaction kinetics.
The electrochemical mechanisms of electrocatalytic processes are a common research subject for various fields of chemistry and associated sciences. This is important to the development of water oxidation and fuel cells catalysts. For example, half the water oxidation reaction is the reduction of protons to hydrogen, the subsequent half reaction.
The upper graph shows the current density as function of the overpotential η . The anodic and cathodic current densities are shown as j a and j c, respectively for α=α a =α c =0.5 and j 0 =1mAcm −2 (close to values for platinum and palladium).