Application of electrochemical series. Electrochemical Series: The concept and its applications 2022-12-21

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The electrochemical series is a list of elements arranged in order of their standard reduction potentials. It is a useful tool for predicting the feasibility of a redox reaction, as well as the direction of electron flow in a galvanic cell.

One common application of the electrochemical series is in the design of galvanic cells, which are devices that use a chemical reaction to generate an electrical current. By arranging the anode and cathode of a galvanic cell based on the relative positions of their constituent elements in the electrochemical series, it is possible to predict the direction of electron flow and the potential difference between the two electrodes.

For example, consider a galvanic cell consisting of a zinc anode and a copper cathode. Since zinc has a more negative reduction potential than copper, it is more likely to be oxidized, releasing electrons to the cathode. This creates a flow of electrons from the anode to the cathode, which can be harnessed to do work, such as powering an electrical circuit.

Another application of the electrochemical series is in the prediction of the feasibility of redox reactions. When two elements are placed in contact with each other, a redox reaction may occur if the reduction potential of one element is more positive than the other. If the difference in reduction potentials is large enough, the reaction will be highly exothermic and proceed spontaneously. If the difference is small, however, the reaction may not occur at all, or may require the input of energy to drive it forward.

One practical example of this is the use of the electrochemical series to predict the corrosion of metals. Corrosion occurs when a metal is oxidized by its surroundings, and the rate at which it occurs is determined by the relative positions of the metal and its oxidizing agents in the electrochemical series. If a metal is located lower in the series than the species that can oxidize it, it will be prone to corrosion. Conversely, if it is higher in the series, it will be more resistant to corrosion.

In summary, the electrochemical series is a valuable tool for predicting the direction of electron flow in a galvanic cell, as well as the feasibility of redox reactions. It is widely used in a variety of fields, including chemistry, electrochemistry, and materials science, to understand and predict the behavior of different elements and their reactions with one another.

Write two applications of electrochemical series.

application of electrochemical series

A redox reaction is feasible only if the species which has higher potential is reduced i. Metals near the top with large negative standard reduction potential values quickly lose electrons. Step II The number of electrons in the two equations are made equal by multiplying one of the equations if necessary by a suitable number. The electrodes above hydrogen have negative reduction potential while those place below it have positive reduction potential and vice-versa. To Find Thermal Stability of Metallic Oxides: The thermal stability of the metal oxide depends on its electropositive nature.


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Electrochemical Series: Explanation & Table

application of electrochemical series

Therefore, I- will be oxidized to I2 and this reaction should be written as oxidation. While those having lower -ve reduction potential are placed at the bottom. They are arranged in decreasing strength of reducing agent to form a series known as Electrochemical Series. Hydrogen and oxygen are bubbled through the electrodes into electrolyte which is an aqueous solution of NaOH or KOH. Cadmium is a toxic heavy metal so NiCd batteries should never be opened or put into the regular trash. In galvanic cell, electrical Electrolytic Cell1. So, the electrochemical series imply that Li is more reactive than Cu.

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Electrochemical Series: The concept and its applications

application of electrochemical series

The elements present at the top of the electrochemical series are considered as good oxidizing agents and those which are present below the electrochemical series are considered as good reducing agents. It assesses the impulsiveness of the complete intracellular response. The series of elements or ions in the increasing order of reduction potential or decreasing order of oxidation potential is known as the electrochemical series. Predicting the Electrolysis Product In the presence of two or more types of positive and negative ions in solution, certain metal ions are discharged or freed at the electrodes in preference to others during electrolysis. In a mixture of copper and silver ions, silver will be deposited first because the reduction potential of silver is higher than copper. It forces the electrons to flow in opposite directions resulting in the deposition of Pb on the anode and Pb02 on the cathode.

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Electrochemical Series: Definitions, 12th Notes, Characteristics, Applications, Chart, Examples

application of electrochemical series

The third and final class is weak electropositive metals which have positive standard electrode potential and placed below hydrogen. Elements having positive or greater reduction potentials do not lose electrons quickly, but they do rapidly gain electrons. The electrochemical series is the basis behind all kinds of modern fuel cells and batteries. Weakly electropositive metals: The metals which are above hydrogen and possess positive values of standard reduction potentials are weakly electropositive metals. Element Li having the bottom-most position has the lowest reduction potential hence it is the strongest reducing agent.

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Electrochemical series and its applications

application of electrochemical series

The discharging and recharging of lead storage battery has been shown in Figs. What are the applications of electrochemical cells. C Almost an equal amount of gas is evolved. Electrochemical Series or EMF Series :- The standard electrode potential Eo cell of a large number of electrodes are determined with respect to the standard hydrogen electrode acting as a reference electrode. Discharging and recharging of lead storage cell b Nickel-cadmium Storage Cell. But if there is a scratch on the tin-plated iron, iron gets rusted because in e. The metals which are above hydrogen in electrochemical series like Cu, Hg, Au, Pt, etc.

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Define Electrochemical Series. Write Its Applications

application of electrochemical series

Cu, Hg, Ag, etc. In general, species with a negative electrode potential are good reducing agents and tend to lose electrons themselves. It means the metal placed above the electrochemical series can displaced the metal from its solution which is placed below it. Above hydrogen, the reducing agent with a positive standard reduction potential is determined. So it is difficult to calculate the electrode potential of an element from half-cell. To predict oxidizing and reducing agent The metals or ions having lower values of reduction potential act as reducing agents whereas the metals or ions having higher values of reduction potential act as oxidizing agents. So, if the voltmeter deflect towards the metal electrode it means that electron moves towards the hydrogen electrode and the metal acts s anode while hydrogen electrode is cathode.

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Importance of Electrochemical Series

application of electrochemical series

This half-cell is completed by adding platinum hydrogen electrode and a salt bridge, while the electrode potential is measured by voltmeter. Thus, the metals placed at the top in the electrochemical series are more active than those placed lower in the electrochemical series. Introduction Electrochemical series is defined as the arrangement of the elements or their ions in increasing or decreasing order of their standard electrode potential under standard conditions. You eventually form an equilibrium, in which some of the zinc atoms give up their electrons to form zinc ions. Thus as we move down the group strength of reducing agent increases while the strength of the oxidizing agent decreases. If it is negative, the cell reaction is not feasible in the given direction and the cell is wrongly represented.


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Application of electrochemical cells Chemistry

application of electrochemical series

F 2 is the strongest oxidizing agent. To solve the problem,a reference electrode is needed and an arbitrary electrode potential must be assigned to it. Elements are arranged in an order in which their strength as reducing agent is decreasing from top to bottom, whereas strength of oxidizing agent increasing from bottom to top. There are two basic types of batteries: primary and secondary. If it is -ve, the cell reaction is not feasible in the given direction and the cell is wrongly represented.


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Applications of electrochemical series?

application of electrochemical series

Commonly used mercury cell. If the electromotive force of the cell is negative, the reaction is not spontaneous. Hence, it can be concluded that metals which lie above hydrogen in the electromotive series can reduce H+ ions to hydrogen and hence, liberate hydrogen gas on reaction with dil acids. For Choosing Elements as Reducing Agents: The elements which have more electron losing tendency are reducing agents. In such a competition, the ion with the higher oxidizing potential high standard reduction potential is discharged first at the cathode.


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Application of Electrochemical Series

application of electrochemical series

A few batteries of each type are described next. The species which lose electrons during oxidation are called Reducing agents. In such a case, hydrogen electrode will act as anode and the metal electrode as the cathode. The electron realeasing or accepting tendency of an electrode is only relative tendency and not absolute tendency. As mentioned above hydrogen is considered as standard and a system which consisted of two hydrogen electrodes have zero reduction potential Eo.

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