H2s acts as reducing agent
WebFollow. Sulfuric acid is an oxidising acid. Sulfur in sulfuric acid has an oxidation state of +6 (the four oxygens are each -2, the hydrogens are +1 and the sum of oxidation numbers for a neutral substance is 0). This is the highest oxidation state that sulfur can have; it can be reduced to +4 (e.g in SO2), 0 (e.g. S) or even -2 (e.g. H2S).
H2s acts as reducing agent
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WebProperties. Hydrogen sulfide is slightly denser than air. A mixture of H 2 S and air can be explosive. In general, hydrogen sulfide acts as a reducing agent, although in the presence of a base, it can act as an acid by … WebThis problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Question: Which of the following is most likely to act as a reducing agent? A) H2S B) H2S05 C) SO3 D) H2504 E) H25208 A o B D OE.
WebSep 23, 2024 · The reducing agent is a substance that causes reduction by losing electrons; therefore its oxidation state increases. The simplest way to think of this is that … Web6 rows · Sep 13, 2024 · A reducing agent is oxidized, because it loses electrons in the redox reaction. Examples of ...
WebSolution. Verified by Toppr. In SO 2, sulphur having oxidation state +4 so it can lose its two more electrons to attain +6 oxidation state. Therefore it can lose and gain electron therefore it acts as oxidising as well as reducing agent. Was this answer helpful? WebMar 30, 2024 · explanation : we know , reducing agent oxidizes itself and reduces other. in option (c) ; here, oxidation number or O.N of Fe in FeCl3 = +3. O.N of S in H2S = -2 . O.N kf Fe in FeCl2 = +2 . Oxidation number of S = 0. it is clear that, Fe is reduced from +3 to +2 whereas S is oxidised from -2 to O. hence, this reaction shows that H2S is strong ...
WebReducing agent. In chemistry, a reducing agent (also known as a reductant, reducer, or electron donor) is a chemical species that "donates" an electron to an electron recipient …
WebH 2 S act as only a reducing agent: In H 2 S, S is in its lowest oxidation state that is − 2. Hence, it can only act as a reducing agent only. bodybuilding reddit traveling supplementsWebJul 20, 2024 · In the world of redox chemistry there exist substances that can act as both a reducing agent and oxidizing and a couple of examples are given below. Water. We have seen that some oxidizing agents, such as fluorine, can oxidize water to oxygen. There are also some reducing agents, such as lithium, which can reduce water to hydrogen. bodybuilding recovery tipsWeb5 years ago. H2S act as only reducing agent because in h2s sulphur is in its minimum oxidation state (-2 ) so it cannot reduce itself to act as oxidising agent but in so2 sulphur … bodybuilding recovery weekWeb36 rows · May 7, 2024 · Solution. We can solve the problem in one of two … bodybuilding recovery assesoriesWebApr 8, 2024 · Reaction of Hydrogen Sulfide with Chlorine – Image will be uploaded soon. As oxidation state of sulfur is increasing (-2 🡪 0) so it is working as reducing agent in the … bodybuilding redditWebH 2O 2−1 H 2O−2 + O 20. H 2O 2 can be reduced to H 2O as well as it can be oxidised to O 2. Hence, it can act as an oxidizing agent by itself getting reduced to H 2O as well as it can act as a reducing agenct by getting oxidized to O 2. Therefore, it can act as oxidizing as well as reducing agent. Solve any question of Redox Reactions with:-. close brewery rentals ltdWebApr 11, 2024 · Complete step by step answer: Sulfur is the element of group 16 and forms a dioxide. It is called sulfur dioxide and has a formula S O 2. The sulfur dioxide acts as a reducing agent as well as an oxidizing agent. First, let us study the reducing property of S O 2 (sulfur dioxide). In the presence of moisture, S O 2 acts as a good reducing agent. close brewery