Sulfuric acid calculation

Both cis and tran -cyclohexene have been synthesized, but only one of them can be isolated. Electrophilic addition of ROH to one isomer occurs spontaneously, while addition to the other isomer occurs only in the presence of a strong acid, such as sulfuric acid. Calculate the energy of protonation for each isomer cyclohexene protonated cyclohexene, trans-cyclohexene protonated trans-cyclohexene), and identify the more reactive isomer. Also examine electrostatic potential maps. Suggest an explanation to account for both the reactivity difference and the structural changes. (See also Chapter 7, Problem 5.)... 

Sulfur trioxide reacts (violently) with water to produce sulfuric acid. Calculate the number of grams of sulfur trioxide necessary to produce 1.00 kg of sulfuric acid. 

The industrial processing of copper(l) sulfide to produce copper metal involves roasting (heating) the solid ore in the presence of oxygen gas to produce the metal and sulfur dioxide gas. (The sulfur dioxide is used to make sulfuric acid.) Calculate the mass of copper(l) sulfide needed to produce 70.0 metric tons (1 metric ton = 1 X 10 g) of copper by roasting. 

The formula of a hydrate of barium chloride is BaCl2 XH2O. If 1.936 g of the compound gives 1.864 g of anhydrous BaS04 upon treatment with sulfuric acid, calculate the value of x... 

The resulting sulfuric acid is then titrated with a standard NaOH solution. A 1.325-g sample of coal is burned and the SO2 collected in a solution of hydrogen peroxide. It took 28.44 mL of 0.1000 A/NaOH to neutralize the resulting sulfuric acid. Calculate the mass percent of sulfur in the coal sample. Sulfuric acid has two acidic hydrogens. 

A 2.0 M solution of styrene in ethylene dichloride is polymerized at 25°C using 4.0 X 10 M sulfuric acid. Calculate the initial degree of polymerization. What would be the degree of polymerization if the monomer solution contains isopropylbenzene at a concentration of 8.0 x 10 Ml Use the following data as needed kp = 7.6 L mol ... 

Production level 1,200 tpd of 93%-96% sulfuric acid calculated on 100% H2SO4 (sulfur burnir ). Production level 1,050 tpd of 93%-96% sulfuric acid calculated on 100% H2SO4 (pyrite gas treatment). 

At present all licensers offer very high rates of S02-conversion, up to 99.8%, and heat recovery as much as 90%. Production-scale capacities are usually between 1,000 tpd and 3,000 tpd. At the normal operating time of about 330 days per year this amounts to 330,000-990,000 tpy of sulfuric acid calculated as 100% H2SO4. 

Due to capillary condensation, salts may form on the catalyst up to 350 °C [8]. For exact calculations, the local gas-phase concentration of SO3, NH3 and HjO along the catalyst and the pore distribution of the catalyst are necessary [11]. The dew-point of sulfuric acid calculated according to [12] is shown in Fig. 2.14. 

Cold, dilute sulfuric acid is capable of oxidizing metals above in the table of standard reduction potentials, but the oxidation state of sulfur does not necessarily change in such reactions. Write an equation representing the oxidation of Mn to the manganous ion by sulfuric acid. Calculate a value for E° for this reaction. 

The purity of a pharmaceutical preparation of sulfanilamide, C6H4N2O2S, can be determined by oxidizing the sulfur to SO2 and bubbling the SO2 through H2O2 to produce H2SO4. The acid is then titrated with a standard solution of NaOH to the bromothymol blue end point, where both of sulfuric acid s acidic protons have been neutralized. Calculate the purity of the preparation, given that a 0.5136-g sample required 48.13 mL of 0.1251 M NaOH. 

Sulfuric Acid. Sulfuric acid is a dense, colorless Hquid at room temperature, having specific gravity as shown in Figure 3 (50). Historically, the concentration of sulfuric acid has been reported as specific gravity (sp gr) in degrees Baumn. In the United States, the Baumn scale is calculated by the following formula ... 

In Germany and France the Baumii scale is calculated using 144.3 as the constant. The Baumii scale only includes the sulfuric acid concentration range of 0—93.19% H2SO. Higher concentrations are not included in the Baumh scale because density is not a unique function of concentration between 93% and 100% acid. The density of sulfuric acid versus temperature and concentration is shown in Figure 4 (50). 

In the early 1970s, air pollution requirements led to the adoption of the double contact or double absorption process, which provides overall conversions of better than 99.7%. The double absorption process employs the principle of intermediate removal of the reaction product, ie, SO, to obtain favorable equiUbria and kinetics in later stages of the reaction. A few single absorption plants are stiU being built in some areas of the world, or where special circumstances exist, but most industriali2ed nations have emission standards that cannot be achieved without utili2ing double absorption or tad-gas scmbbers. A discussion of sulfuric acid plant air emissions, control measures, and emissions calculations can be found in Reference 98. 

To calculate the open circuit voltage of the lead—acid battery, an accurate value for the standard cell potential, which is consistent with the activity coefficients of sulfuric acid, must also be known. The standard cell potential for the double sulfate reaction is 2.048 V at 25 °C. This value is calculated from the standard electrode potentials for the (Pt)H2 H2S04(yw) PbS04 Pb02(Pt) electrode 1.690 V (14), for the Pb(Hg) PbS04 H2S04(yw) H2(Pt) electrode 0.3526 V (19), and for the Pb Pb2+ Pb(Hg) 0.0057 V (21). 

Table 1 gives the calculated open circuit voltages of the lead—acid cell at 25°C at the sulfuric acid molalities shown. The corrected activities of sulfuric acid from vapor pressure data (20) are also given. 

The temperature dependence of the open circuit voltage has been accurately determined (22) from heat capacity measurements (23). The temperature coefficients are given in Table 2. The accuracy of these temperature coefficients does not depend on the accuracy of the open circuit voltages at 25°C shown in Table 1. Using the data in Tables 1 and 2, the open circuit voltage can be calculated from 0 to 60°C at concentrations of sulfuric acid from 0.1 to 13.877 m. 

Assay of beryUium metal and beryUium compounds is usuaUy accompHshed by titration. The sample is dissolved in sulfuric acid. Solution pH is adjusted to 8.5 using sodium hydroxide. The beryUium hydroxide precipitate is redissolved by addition of excess sodium fluoride. Liberated hydroxide is titrated with sulfuric acid. The beryUium content of the sample is calculated from the titration volume. Standards containing known beryUium concentrations must be analyzed along with the samples, as complexation of beryUium by fluoride is not quantitative. Titration rate and hold times ate critical therefore use of an automatic titrator is recommended. Other fluotide-complexing elements such as aluminum, sUicon, zirconium, hafnium, uranium, thorium, and rate earth elements must be absent, or must be corrected for if present in smaU amounts. Copper-beryUium and nickel—beryUium aUoys can be analyzed by titration if the beryUium is first separated from copper, nickel, and cobalt by ammonium hydroxide precipitation (15,16). 

Continuous esterification of acetic acid in an excess of -butyl alcohol with sulfuric acid catalyst using a four-plate single bubblecap column with reboiler has been studied (55). The rate constant and the theoretical extent of reaction were calculated for each plate, based on plate composition and on the total incoming material to the plate. Good agreement with the analytical data was obtained. 

MO calculations of the cinnoline ring system show that the relative order of reactivities for electrophilic substitution is 5=8>6 = 7>3 4. This is confirmed experimentally, as nitration of cinnoline with a mixture of nitric and sulfuric acids affords 5-nitrocinnoline (33%) and 8-nitrocinnoline (28%). Similarly, 4-methylcinnoline gives a mixture of 4-methyl-8-nitrocinnoline (28%) and 4-methyl-5-nitrocinnoline (13%). 

The calcium salt of the principal product, d/-tartaric acid, crystallizes with four molecules of water, while the secondary product, meso-tartaric acid, forms a calcium salt which crystallizes with three molecules of water. The amount of sulfuric acid actually required may readily be calculated from the percentage of calcium found on analysis in the regular way or it may be estimated by igniting a sample, and titrating the residue with standard acid. 

Experimental observations indicate that acid strength significantly affects the reaction rate. For example, sulfuric acid promotes nucleophilic substitution of alcohols by bromide, but acetic acid does not. How would a change in acid strength affect your calculated reaction energies ... 

The sole known example of electrophilic substitution in quinazoline is nitration. Quinazoline gives 6-nitroquinazoline with fuming nitric acid in concentrated sulfuric acid. No oxidation of the heterocyclic ring can occur under these conditions because the hydrated cation (see Section IIA>4) is not present. This substitution is in agreement with theoretical calculation [see (2) and reference 36]. 

In Table 38 the autoprotolysis constant of sulfuric acid is given by — log K = 3.1, from which we calculate... 

Suppose you wish to calculate the mass of sulfuric acid that can be obtained from an underground deposit of sulfur 1.00 km2 in area. What additional information do you need to make this calculation ... 

Hibbert and Burt dissolved the benzoylperoxide in dry ether, cooled to — 50 and added the calculated amount of a 10 per cent sodium ethylate solution, maintaining the low temperature during the procedure. Sufficient ice water was added to give a clear solution, the ether containing the ethyl benzoate separated and the aqueous sodium benzoylperoxide solution added slowly with stirring to twice the necessary amount of cold 20 per cent sulfuric acid (reaction mixture always at o°). The oily layer of benzoylhydroperoxide was then extracted three times with chloroform and the extract dried over anhydrous sodium sulfate. 

Cyclohexylcarbinol (6, 22), In the preparation of cyclohexylcarbinol as described in Vol. 6, 22, a high-boiling by-product, the cyclohexylcarbinol acetal of formaldehyde, is sometimes obtained. The by-product becomes the main product if the steam distillation of the reaction mixture is omitted. The by-product can usually be avoided if twice the calculated amount to decompose the Grignard reagent of io per cent sulfuric acid is added to the reaction mixture before steam distillation is earned out. The acetal which may be present is thus hydrolyzed. 

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