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The auxiliary electrode may be isolated from the working electrode using a glass frit. Such isolation prevents any byproducts generated at the auxiliary electrode from contaminating the main test solution: for example, if a reduction is being performed at the working electrode in aqueous solution, oxygen may be evolved from the auxiliary electrode.
The current at the working electrode is plotted versus the voltage at the working electrode to yield the cyclic voltammogram (see Figure 1). Cyclic voltammetry is generally used to study the electrochemical properties of an analyte in solution [2] [3] [4] [1] or of a molecule that is adsorbed onto the electrode.
This isolates the undesired redox events taking place at the auxiliary electrode. During bulk electrolysis, the analyte undergoes a redox event at the working electrode. If the system was open, then it would be possible for the product of that reaction to diffuse back to the auxiliary electrode and undergo the inverse redox reaction.
Silver chloride electrode (E = +0.22249 V in 3.0 mol KCl/L) [2] pH-electrode (in case of pH buffered solutions, see buffer solution) Palladium-hydrogen electrode; Dynamic hydrogen electrode (DHE) Mercury-mercurous sulfate electrode (MSE) (E = +0.64 V in sat'd K 2 SO 4, E = +0.68 V in 0.5 M H 2 SO 4) Cu-Cu(II) reference electrode Ag-AgCl ...
The electrode current is kept fairly constant during operation by automatically raising and lowering the electrodes. When current increases, the electrodes are raised, increasing the electrical resistance between the electrodes and the furnace floor. Hence reducing the current, produces the opposite effect when the voltage is kept constant.
Both of these electrodes are balanced by a single reference and auxiliary combination for an overall four-electrode design. More complicated experiments may add working electrodes, reference, or auxiliary electrodes as required. [7] In practice it can be important to have a working electrode with known dimensions and surface characteristics.