Sulfur can be recovered from the hydrogen sulfide removed from crude oil deposits, a process known as sweetening, by roasting in air and using the sulfur dioxide initially formed to push the reaction to the final product: H2S(g) + O2(g) --> H2O(g) + SO2(g) H2S(g) + SO2(g) --> H2O(g) + S(s) The maximum number of kilograms of sulfur that can be isolated per kilogram of hydrogen sulfide entering the process is __________.

Sulfur can be recovered from the hydrogen sulfide removed from crude oil deposits, a process known as sweetening, by roasting in air and using the sulfur dioxide initially formed to push the reaction to the final product: H2S(g) + O2(g) --> H2O(g) + SO2(g) H2S(g) + SO2(g) --> H2O(g) + S(s) The maximum number of kilograms of sulfur that can be isolated per kilogram of hydrogen sulfide entering the process is __________.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 80AP

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42. The primary use of 1,2‐dichloroethane, ClCH2CH2Cl, is to make vinyl chloride, which is then converted into polyvinyl chloride (PVC) for many purposes, including plastic pipes. Balance the following equation, which describes the industrial reaction for producing 1,2‐dichloroethane. C2H4 + HCl + O2 → ClCH2CH2Cl + H2O 50. Gaseous propane and liquid diethyl ether mix to form a solution. Which of thesesubstances is the solute and which is the solvent? 51. Consider a solution of 10% liquid acetone and 90% liquid chloroform. Which of these substances is the solute and which is the solvent?
A secondary step in the process to produce ultra-pure silicon forelectronic applications involves silicon tetrachloride with magnesium in a redox reaction:__SiCl + __Mg→ __Si + __MgClBalance the equation above and assign the oxidation numbers (O.N.) of the atoms in the reactants and products. REACTANTS SIDEO.N. of Si in SiCl : ______O.N. of Cl in SiCl : ______O.N. of Mg: ______PRODUCTS SIDEO.N. of Si: ______O.N. of Mg in MgCl : _______O.N. of Cl in MgCl : ______
Fe2O3 is produced from a pyrite concentrate containing 65% by weight of pyrite (FeS2) by total oxidizing roasting according to the following reaction. 5 tons of pyrite concentrate is roasted daily (MA, g / mol; Fe: 56; S: 32; 0: 16; H: 1). 2FeS2 + 11 / 2O2 → Fe2O3 + 4SO2 How much Fe2O3 is produced in 1 day?
Aircraft de-icing agents, such as propylene glycol [1,2-propanediol; CH₃CH(OH)CH₂OH; d=1.036 g/mL], are used toremove ice and snow prior to winter flights, but their presence inrunoff depletes O₂ in natural waters. (a) Write a balanced equa-tion for the complete oxidation of propylene glycol by O₂.(b) What is the “theoretical oxygen demand,” in grams of O₂ required per gram of propylene glycol oxidized? (c) What is thetheoretical oxygen demand, in grams of O₂ required per liter ofsolution, of 90.0% by volume aqueous propylene glycol?
A typical formulation for window glass is 75% SiO₂, 15% Na₂O, and 10.% CaO by mass. What masses of sand (SiO₂),sodium carbonate, and calcium carbonate must be combined toproduce 1.00 kg of glass after carbon dioxide is driven off bythermal decomposition of the carbonates?
Pure CO2 may be prepared by treating limestone with sulfuric acid. The limestone used in the process contains CaCO3, MgCO3 and inert. The acid used contains 12% H2SO4 by weight The residue from the process had the following composition. CaSO4 – 8.56%; MgSO4 – 5.23%; H2SO4 – 1.05%; Inert – 0.53%; CO2 – 0.12%; H2O – 84.51%; During the process, the mass was warmed where CO2 and H2O were removed. Calculate the following.a) The analysis of lime stone and b) The % excess acid used.
A commercial 737 jet transporting 143 passengers and 5 crew members from Kansas city (MCI) to Baltimore (BWI) burned 11800 lb. of Jet A fuel. Jet A fuel is kerosene based, consisting primarily of CnH2n+2 hydrocarbons, with n = 6 to 16, so the Carbon:Hydrogen ratio is close to 1:2. During this flight , how much CO2 (in kg) was released into the atmosphere? (assume the combustion of fuel was complete, so all fuel was converted into H2O and CO2).
An ore containing Fe3O4 was analyzed by dissolving a 1.5419-g sample in concentrated HCl. HNO3 was then added to oxidize any Fe2+ to Fe3+. The Fe3+ was precipitated as Fe(OH)3 by adding NH3. The precipitate was collected by filtration and was finally heated yielding 0.8525 g of Fe2O3. Report the concentration of Fe3O4 in the sample as %(w/w). (Note: the final answer is said to be 53.4%)
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Farmers use ammonium sulfate as a fertilizer. In the soil, ni-trifying bacteria oxidize NH4+to NO3-, a groundwater contam-inant that causes methemoglobinemia (“blue baby” syndrome).The World Health Organization standard for maximum [NO3-]in groundwater is 45 mg/L. A farmer adds 210. kg of (NH4)2SO4 to a field and 37% is oxidized to NO3-. What is the groundwa-ter [NO3-] (in mg/L) if 1000. m3of the water is contaminated?