February 2024

The following are some examples for corrosion that we experience in our day to day life. (i) Rusting of iron : Iron exposed to the environment forms a brown rust film on its surface. (ii) Water stored in aluminium vessel : If water is stored for a long time in an aluminium vessel, white spots

Here are a few simple electrochemistry solved problems along with their solutions: 1. Calculate the single electrode potential of copper metal immersed in 0.15°MCu2+ solution. E° for copper is +0.34 V at 25°C. Solution: By Nernst equation [latex] \mathrm{E}=\mathrm{E}^{\circ}+\frac{0.0592}{\mathrm{n}}\left[\log \mathrm{M}^{\mathrm{n}+}\right] at 25^{\circ} \mathrm{C} [/latex] [latex] \begin{aligned} & =0.34+\frac{0.0592}{2} \log [0.15] \\ & =0.34+\frac{0.0592}{2}(-0.8239)=0.3156 \mathrm{~V} \end{aligned} [/latex] 2. Calculate the electrode potential of

Definition : When elements are arranged in increasing order of their standard reduction electrode potentials, the series so obtained is known as electrochemical (or) electromotive series. or A series in which standard reduction potentials of various electrodes are arranged in the order of increasing reduction potentials (largest reduction potential at the top) or decreasing oxidation

Nernst equation can be used to calculate the emf of the cells when the concentration of reactants and products are known. Let us consider a general redox reaction Mn+ + ne– [latex] \rightleftharpoons [/latex] M. For any reversible reaction, the change in free energy ΔG and equilibrium constant K can be related using van’t Hoff’s isotherm as

It is impossible to know the absolute values of the single electrode potential. It is because a single electrode constitutes only a half- cell. A half-cell would not lose or gain electrons by itself. The loss or gain of electrons can take place only in a complete circuit containing two half- cells connected to each

Definition : Measure of tendency of a metallic electrode to lose or gain electrons when it is in contact with its own ions in solution is called electrode potential. When an electrode, say a metal, is immersed in a solution of its ions, then there can be two possibilities: (i) Mn+ ions may collide with

The cells used for electrolysis are called electrolytic cells while those used for generation of electrical energy from chemical reactions are called galvanic or voltaic cells. The practical application of a galvanic cell is Daniel cell. The electrode where oxidation occurs is called anode and the electrode where reduction occurs is called cathode. John Daniell

The chemical reactions in which both oxidation and reduction occur simultaneously are called redox reaction. Oxidation is the process where electrons are lost from a species and reduction is the process where electrons are gained by a species. On the other hand, the species which reduces other species and itself undergoes oxidation by donating electrons

Sodium-potassium pumps, also known as Na+/K+-ATPases, are integral membrane proteins responsible for maintaining the electrochemical gradient across cell membranes. This gradient is vital for numerous cellular functions, including nerve signal transmission, muscle contraction, and nutrient uptake. Structure of Sodium-Potassium Pumps At the structural level, sodium-potassium pumps consist of several subunits, including alpha and beta subunits.

A cell is a device for the conversion of electrical energy into chemical change or vice versa. It is a system containing two metallic electrodes, dipped into the same or different electrolytes, connected by an external metallic conductor. Types of cells The cells are classified into two types: Electrolytic cells. Electrochemical cells. Electrolytic cells These