In ICSE Class 10 Chemistry Sulphuric Acid the Sulphuric acid, or as we write, H2SO4, is a very corrosive odourless, colourless, oily liquid. People called it Vitriol's Oil. It has alluded as the' King of Chemicals' because of its wide applications. We can find it in both free and combined condition. Get the ICSE Class 10 Chemistry Sulphuric Acid explanation on the Extramarks website. Get the ICSE Class 10 Chemistry Sulphuric Acid study matter is on the Extramarks website.

Sulfur dioxide, SO2, is a dense, colourless gas formed by the burning of many sulfur compounds in the air. It's very toxic and smells asphyxiating. It occurs naturally as one of the plants and animal degradation products, as well as one of the gasses emitted from volcanoes (along with CO2 and H2S).

Because SO2 is produced when some of the sulfur-containing oil and coal components are burned, our power plants and factories release huge volumes of this toxic gas into the atmosphere. It is estimated that this releases approximately 200 million tons of sulfur annually compared to 300 million tons from natural sources. This has serious environmental effects as the SO2 can dissolve in cloud water vapour to form dilute sulphuric acid (H2SO3) and sulphuric acid (H2SO4). This, together with nitric and nitrous acids produced from nitrogen oxides in the same way, forms the basis for' acid rain,' which then falls back to Earth killing and damaging forests and forests, polluting lakes, and corroding buildings and statues.

Simply explained, under the influence of an electric current, the electrolysis process refers to the decomposition of a given element. Sir Humphrey Davey performed the first electrolysis in 1808. This experiment revealed new understandings of how certain elements behave and how compounds and ions differ from each other. The ICSE Class 10 Chemistry Electrolysis study matter is on the Extramarks website. The ICSE Class 10 Chemistry Electrolysis explanation is also available on the Extramarks app.

As for an electrolytic cell, we can say that it is much the same in many respects as a galvanic cell because it requires a salt bridge, two electrodes and the flow of electrons from the anode to the cathode. However, in many respects, the two still manage to be different from each other. For one, electrical energy is converted into chemical energy by an electrolytic cell and not the other way around.

The resulting redox reaction in the process is not spontaneous, and electrical energy must be inserted into the apparatus for the reaction to begin. Unlike a galvanic cell, both metals must be placed in the same container by an electrolytic cell. In this case, the positive electrode is called the anode and the cathode is called the negative electrode. An external battery is used for the supply of electrons.