Electrochemistry creates electricity by moving electrons between elements. This is an oxidation-reduction process. The procedure is also used in daily life. According to the NCERT for electrochemistry class 12, here are some explanations of its applications.
There are two kinds of reactions. Read the article on electrochemistry class 12 NCERT solutions below to understand how it works. It will help you know some of its applications.
The phrase 'electrochemical cell' refers to the interconversion in equipment. To comprehend electrochemical cells, it is necessary to understand what they are. An anode and a cathode are the two electrodes of an electrochemical cell. The anode is oxidised, while the cathode is reduced. When the metal on the anode gets an electron and becomes an ion, this is referred to as oxidation. Metal ions in the solution absorb electrons from the cathode and decrease to zero, resulting in a solid metal on the opposite side.
There are two main types of electrochemical cells:
E.g.:- Daniell cells and Redox cells. Both are composed of two electrodes connected by an ionic conductor. An electrolyte separates the two electrodes and serves as the fluid that transfers electrons. The two half-cells are separated by a metal wire called the anode. The electron conductor that links the two electrodes is often metal wire.
The Nernst Equation describes the relationship between the cell potential and the concentrations of electrically active species. It is also used to calculate the cell potential at any point during a reaction.
Electrolysis is a process in which chemicals are changed. In particular, it is a decomposition process. In this process, the ions of the electrolyte move towards the electrodes. The negative ions move toward the anode and lose an electron, becoming neutral. The positive ions move toward the cathode and gain an electron. The resulting reaction is called oxidation. This method is used to extract metals, such as gold and silver.
Batteries come in many shapes and sizes, from small cells for wristwatches and hearing aids to massive battery banks that provide standby power to computer data centres and telephone exchanges. Despite the differences in size and shape, batteries are fundamentally the same.
There are two different types of commercial cells. While the fundamental laws of electrochemistry apply to all of them, commercial batteries differ primarily by the type of reactant they use.
A fuel cell is an electrochemical cell that uses an electrochemical technique to produce electricity from fuels. Fuel cells are similar to electrochemical cells.
One of the essential factors in determining the overall market size for Fuel Cells is the fuel cells used. This cell type is best suited for stationary power generation and runs at high temperatures. These systems can be degraded by repeated cycling on and off, but their long-term stability makes them a good choice for continuous use. Solid oxide cells also produce steam, channelled into turbines to produce more electricity.
Working of a Fuel Cell
The working of a Fuel Cell involves three different steps.
There are several examples of Fuel Cells and their workings.
Corrosion is the natural process by which metals revert to their oxidation state. It is a spontaneous, electrochemical reaction that produces various products, including rusting, a visible orange colouration. However, corrosion can also occur in materials other than metals, more commonly referred to as degradation. The material loses many valuable properties in this process, including its strength, appearance, and permeability to liquids. Copper rusting, silver corrosion, and rusting are just a few instances of what might happen.
Types of Corrosion
Understanding the different types of corrosion can help you prevent or mitigate problems. The most common form of corrosion is uniform corrosion. This type of corrosion is characterised by an even attack on the surface of a metal. It is prevalent, as its impact is easy to judge and evaluate. The main difference between uniform and other forms of erosion is that the former occurs on a larger area of the material's surface. This type of corrosion occurs on many materials, including aluminium.
The conductivity of electrolytic solutions increases as the concentration of the electrolyte increases. As the concentration of the electrolyte increases, the ionic forces of attraction between like ions decrease. The change in equilibrium is caused by an increase in the number of ions. As the solution dries, the ionic forces of attraction decrease, and the electrolyte undergoes further ionisation.
Factors affecting Electrolytic Conductance
Keep these electrochemistry class 12 NCERT solutions handy if you're worried about the exam. This NCERT for electrochemistry class 12 revision guides is easy to read and give you the best chance of getting a good grade. You'll be glad you did when you see how useful they are! You'll also find them helpful for CBSE students taking the same course. This guide is a must-have for your studies.
Q: Can AgCl be stored in a Zinc pot?
A: Yes, but you shouldn't. The reason is simple: zinc reacts with silver and forms zinc chloride. The silver is replaced by zinc. This is called a single replacement reaction. Therefore, you should keep your AgCl solution in a plastic container, like a glass jar. This will prevent it from oxidising.
Q: What is the definition of Standard electrode potential?
A: This is the electrical potential of a reaction at an electrode. This happens when all substances involved in the reaction are normal. This means all gases and solutions have a concentration of 1M and are at 25C. Lithium, on the other hand, has a negative electrode reduction potential. Hence, lithium is the most potent reducing agent.
Q: What is cell electromotive force?
A: The electric potential difference between two oppositely charged metals in a cell is the electromotive force. This force is created when electrons move from one metal with higher free energy to another with lower free energy. The voltage produced depends on the size of the load. The electromotive forces produced in the battery and a generator are different. For this reason, it is essential to understand the chemistry of batteries.
Q: Can an electrochemical cell become electrolytic? How?
A: When an electrochemical cell becomes electrolytic, it switches from chemical to electrical. The two electrodes must be connected electrically, and the ions of the anode must move from the right to the left to balance the flow of electrons. An external electrical potential produces an electric current. The electrons from the oxidation will transfer to the reduction of the negative ions in the cell and vice versa.
Q: What Is An Electrochemical Series?
A: An electrochemical series is a table presenting the order of elements in a reaction based on their standard electrode potential. The element with the lowest potential, or the electrode with which the reaction takes place, is called a standard electrode, and the elements above and below it have different potentials. Higher-ranking elements are considered good oxidising agents, and lower-ranking ones are considered better reducing agents.