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Sulfuric acid (American spelling and the preferred IUPAC name) or sulphuric acid (Commonwealth spelling), known in antiquity as oil of vitriol, is a mineral acid composed of the elements sulfur, oxygen, and hydrogen, with the molecular formula H 2 SO 4. It is a colorless, odorless, and viscous liquid that is miscible with water. [6] Structure ...
Some water-reactive substances are also pyrophoric, like organometallics and sulfuric acid. The use of acid-resistant gloves and face shield is recommended for safe handling; fume hoods are another effective control of such substances. [4]
The first and faster [citation needed] process is the removal of hydrogen and oxygen as units of water by the concentrated sulfuric acid. This occurs because hydration of concentrated sulfuric acid is strongly thermodynamically favorable, with a standard enthalpy of reaction of −880 kJ/mol.
The most reactive metals, such as sodium, will react with cold water to produce hydrogen and the metal hydroxide: 2 Na (s) + 2 H 2 O (l) →2 NaOH (aq) + H 2 (g) Metals in the middle of the reactivity series, such as iron , will react with acids such as sulfuric acid (but not water at normal temperatures) to give hydrogen and a metal salt ...
Sulfamic acid melts at 205 °C before decomposing at higher temperatures to water, sulfur trioxide, sulfur dioxide and nitrogen. [2] Sulfamic acid (H 3 NSO 3) may be considered an intermediate compound between sulfuric acid (H 2 SO 4), and sulfamide (H 4 N 2 SO 2), effectively replacing a hydroxyl (–OH) group with an amine (–NH 2) group at
Sulfur dioxide reacts with water to form the weak acid, sulfurous acid: SO 2 + H 2 O → H 2 SO 3. Sulfur trioxide forms the strong acid sulfuric acid with water: SO 3 + H 2 O → H 2 SO 4. This reaction is important in the manufacturing of sulfuric acid.
The contact process is a method of producing sulfuric acid in the high concentrations needed for industrial processes. Platinum was originally used as the catalyst for this reaction; however, because it is susceptible to reacting with arsenic impurities in the sulfur feedstock, vanadium(V) oxide (V 2 O 5) has since been preferred.
Sulfuryl chloride reacts with water, releasing hydrogen chloride gas and sulfuric acid: . 2 H 2 O + SO 2 Cl 2 → 2 HCl + H 2 SO 4. For sulfuryl chloride, this happens at room temperature, but the related sulfuryl fluoride does not hydrolyse at temperatures up to 150 °C.