Here is everything to know about electrochemistry, with tips and tricks!!

“Every man who receives a liberal education now counts chemistry among the most indispensable objects of his studies.”

-Antoine Francois Fourcroy.

Let’s start with what electrochemistry actually is? But, a question may arise in the mind of every student at some point: how should we deal with all the reactions of chemistry? And how can they be remembered? Most importantly, how do we retain them? In all of this, we would like to recommend you not to become worried, because here at DoubtConnect, we, the whole team, are there to assist you with all your issues.

Let’s begin by stating what will be the main topics discussed today. Thereafter, we will discuss the various reference books through which you can study more effectively. And last but not least, we’ll discuss tricks and tips.

• Electrochemical Cell
• Types of Electrochemical cells
• EMF of a cell

So, the study of electrical energy and chemical change is called electrochemistry, a subfield of chemistry. Those chemical reactions that involve the generation or input of electric currents are referred to as electrochemical reactions.

Two broad categories of reactions can be distinguished:

1. Electrical energy is used to cause a chemical change, which is known as electrolysis.
2. The process of transforming chemical energy into electrical power. This refers to spontaneous redox reactions that produce electricity.

• Electrochemical Cell-

An electrochemical cell is a device that can create electricity by utilizing chemical reactions, or it can generate electricity by supplying it with electrical energy so that it can facilitate chemical reactions. In these devices, chemical energy can be converted into electrical energy or the other way around. Example: Electric appliances such as TV remotes and clocks are powered using electrochemical cells such as standard 1.5-volt cells.

• Electrochemical cells can be classified into two types:

The first is galvanic cells, while the second is electrolytic cells. These are fundamentally different types of electrochemical cells.

Galvanic cell — In a galvanic cell, chemical energy is transformed into electrical energy through spontaneous redox reactions. Alternatively, the cell is called a voltaic cell or Daniel cell.

Electrochemical cells such as galvanic cells play an imperative role in our society. Two metal rods, known as electrodes, are combined in a galvanic cell. An electrode is immersed in both electrode solutions, and the electrodes form a half cell when the solutions contain a combination of ions.

Salt bridges connect the half-cells, and the electrolyte is the solution in which both electrodes are dipped. Those occurring inside this cell are undergoing a redox reaction. On the electrode that functions as an anode, oxidation occurs, while on the electrode that functions as a cathode, reduction occurs.

Electrolytic cells- Cells that perform nonspontaneous redox reactions using electric energy include electrolytic cells. An electric energy conversion device or device that converts chemical energy into electricity. In such a cell, two metals or electronic conductors (electrodes) are separated from one another and connected to an electrolyte, usually a dissolved or fused ionic compound.

By taking the difference between the standard potentials of the anode and cathode, we can calculate the standard potential of the cell.

• EMF — what is it?

Electromotive force (EMF), which is the maximum potential difference between two electrodes of a galvanic or voltaic cell, is described by the electromotive force abbreviation.

The following is a description of its structure:
A cell’s electromotive force can be calculated as half-cell potential at the cathode (right) and half-cell potential at the anode (left).

❖ Reference books for better comprehension

1. Pradeep’s New Course Chemistry for Class XII (Vol I and II)
2. Modern’s ABC of Chemistry Class — 12th (Part 1 & 2)
3. Concise Inorganic Chemistry
4. Modern Approach to Chemical Calculations

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