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2 FeS 2 (s) + 7 O 2 + 2 H 2 O → 2 Fe 2+ + 4 SO 2− 4 + 4 H + The resulting highly acidic water is called acid mine drainage (AMD) or acid rock drainage (ARD). The Fe 2+ can be further oxidized to Fe 3+: 4 Fe 2+ + O 2 + 4 H + → 4 Fe 3+ + 2 H 2 O. The Fe 3+ produced can be precipitated as the hydroxide or hydrous iron oxide: Fe 3+ + 3 H 2 O ...
Hot sulfur trioxide passes through the heat exchanger and is dissolved in concentrated H 2 SO 4 in the absorption tower to form oleum. H 2 SO 4 + SO 3 → H 2 S 2 O 7. Note that directly dissolving SO 3 in water is impractical due to the highly exothermic nature of the reaction. Acidic vapor or mists are formed instead of a liquid. Oleum is ...
The lead chamber process was an industrial method used to produce sulfuric acid in large quantities. It has been largely supplanted by the contact process.. In 1746 in Birmingham, England, John Roebuck began producing sulfuric acid in lead-lined chambers, which were stronger and less expensive and could be made much larger than the glass containers that had been used previously.
Sulfurous acid is commonly known to not exist in its free state, and due to this, it is stated in textbooks that it cannot be isolated in the water-free form. [4] However, the molecule has been detected in the gas phase in 1988 by the dissociative ionization of diethyl sulfite. [5]
In chemistry, the oxygen reduction reaction refers to the reduction half reaction whereby O 2 is reduced to water or hydrogen peroxide. In fuel cells, the reduction to water is preferred because the current is higher. The oxygen reduction reaction is well demonstrated and highly efficient in nature. [1] [2]
For example, 10% oleum can also be expressed as H 2 SO 4 ·0.13611SO 3, 1.13611SO 3 ·H 2 O or 102.25% sulfuric acid. The conversion between % acid and % oleum is: % = + % For x = 1 and y = 2 the empirical formula H 2 S 2 O 7 for disulfuric (pyrosulfuric) acid is obtained. Pure disulfuric acid is a solid at room temperature, melting at 36 °C ...
2 CaSO 3 + H 2 O + O 2 → 2 CaSO 4 ·2H 2 O. A natural alkaline usable to absorb SO 2 is seawater. The SO 2 is absorbed in the water, and when oxygen is added reacts to form sulfate ions SO 2− 4 and free H +. The surplus of H + is offset by the carbonates in seawater pushing the carbonate equilibrium to release CO 2 gas: SO 2 + H 2 O + O → ...
Beaumont St. Louis and San Francisco Railroad Water Tank (1875, restored 2012), Beaumont, Kansas, US. Although the use of elevated water storage tanks has existed since ancient times in various forms, the modern use of water towers for pressurized public water systems developed during the mid-19th century, as steam-pumping became more common, and better pipes that could handle higher pressures ...