Search results
Results from the WOW.Com Content Network
An electrolytic cell is an electrochemical cell in which applied electrical energy drives a non-spontaneous redox reaction. [5] A modern electrolytic cell consisting of two half reactions, two electrodes, a salt bridge, voltmeter, and a battery. They are often used to decompose chemical compounds, in a process called electrolysis.
Industrially this process takes place in a special cell named Downs cell. The cell is connected to an electrical power supply, allowing electrons to migrate from the power supply to the electrolytic cell. [28] Reactions that take place in a Downs cell are the following: [28] Anode (oxidation): 2 Cl − (l) → Cl 2 (g) + 2 e −
The potential of the whole cell is obtained as the difference between the potentials for the two half-cells, so it depends on the concentrations of both dissolved metal ions. If the concentrations are the same the Nernst equation is not needed, and E c e l l = E c e l l o {\displaystyle ~E_{\mathsf {cell}}~=~E_{\mathsf {cell}}^{\mathsf {\;\!o ...
An electrolytic cell is an electrochemical cell that utilizes an external source of electrical energy to force a chemical reaction that would otherwise not occur. [ 1 ] : 64, 89 [ 2 ] : GL7 The external energy source is a voltage applied between the cell's two electrodes ; an anode (positively charged electrode) and a cathode (negatively ...
The difference can be measured as a difference in voltage potential: the less noble metal is the one with a lower (that is, more negative) electrode potential than the nobler one, and will function as the anode (electron or anion attractor) within the electrolyte device functioning as described above (a galvanic cell).
The term is directly related to a cell's voltage efficiency. In an electrolytic cell the existence of overpotential implies that the cell requires more energy than thermodynamically expected to drive a reaction. In a galvanic cell the existence of overpotential means less energy is recovered than thermodynamics predicts.
In electrochemistry, a thermogalvanic cell is a kind of galvanic cell in which heat is employed to provide electrical power directly. [1] [2] These cells are electrochemical cells in which the two electrodes are deliberately maintained at different temperatures. This temperature difference generates a potential difference between the electrodes.
It may also be defined as the potential difference between the charged metallic rods and salt solution. The electrode potential has its origin in the potential difference developed at the interface between the electrode and the electrolyte. It is common, for instance, to speak of the electrode potential of the M + /M redox couple.