Sulfuric acid H2SO4 making

Anhydride. A chemical compound derived from an acid by elimination of the atoms that make up water. Example SO3, sulfur trioxide, is the anhydride of sulfuric acid, H2SO4. Anhydrides are a class of organic compounds derived from the combination of two carboxylic acids (R-COOH) by. elimination of a molecule of water. For example, acetic acid (CH3COOH) minus water gives acetic anhydride. 

The important point is that, at any one particular temperature, the equilibrium constant is just that—constant. This gives us a means of forcing the equilibrium to favour the products (or reactants) since the ratio of the two must remain constant. Therefore, if we increase the concentration of the reactants (or even that of just one of the reactants), more products must be produced to keep the equilibrium constant. One way to make esters in the laboratory is to use a large excess of the alcohol and remove water continually from the system as it is formed, for example by distilling it out. This means that in the equilibrium mixture there is a tiny quantity of water, lots of the ester, lots of the alcohol, and very little of the carboxylic acid in other words, we have converted the carboxylic acid into the ester. We must still use an acid catalyst, but the acid must be anhydrous since we do not want any water present—commonly used acids are toluene sulfonic acid (tosic acid, TsOH), concentrated sulfuric acid (H2SO4), or gaseous HC1. The acid catalyst does not alter the position of the equilibrium it simply speeds up the rate of the reaction, allowing equilibrium to be reached more quickly. 

Palladium has two primary uses as a catalyst and in making jewelry and specialized alloys. A catalyst is a substance used to speed up a chemical reaction without undergoing any change itself. Palladium catalysts are used in breaking down petroleum to make high quality gasoline and other products. It is also used in the production of some essential chemicals, such as sulfuric acid (H2SO4), which is used in paper and fabric production. The catalytic converters used in automobiles today may also contain a palladium catalyst. A catalytic converter is a device added to a car s exhaust system. It helps the fuel used in the car burn more efficiently. 

Some powdered sulfur is also used as an insecticide. It can be spread on plants to kill or drive away insects that feed on the plants. By far the majority of sulfur is used, however, to make sulfur compounds. The most important of these is sulfuric acid (H2SO4). 

Similarly, tin is attacked only slowly by dilute acids such as hydrochloric acid (HCl) and sulfuric acid (H2SO4). Dilute acids are mixtures that contain small amounts of acid dissolved in large amounts of water. This property also makes tin a good protective covering. It does not react with acids as rapidly as do many other kinds of metals, such as iron, and can be used, therefore, as a covering for those metals. 

LAB that in order to compete, manufacturers must reduce the cost of making their products to the lowest level possible. Percent yield is important in the calculation of overall cost effectiveness in industrial processes. For example, sulfuric acid (H2SO4) is made using mined sulfur. Figure 12-8. Sulfuric acid is an important chemical because it is a raw material for products such as fertilizers, detergents, pigments, and textiles. The cost of sulfuric acid affects the cost of many of the consumer items you use every day. 

Describe how the strong diprotic acid sulfuric acid, H2SO4 (used to make industrial explosives) acts when it is added to water, including a description of the nature of the particles in solution before and after the reaction with water. If there is a reversible reaction with water, describe the forward and the reverse reactions. 

An impure sample of zinc (Zn) is treated with an excess of sulfuric acid (H2SO4) to form zinc sulfate (ZnS04) and molecular hydrogen (H2). (a) Write a balanced equation for the reaction, (b) If 0.0764 g of H2 is obtained from 3.86 g of the sample, calculate the percent purity of the sample, (c) What assumptions must you make in (b) ... 

Fig. 23.1. Simplified single contact sulfuric acid production flowsheet. Its inputs are moist feed gas and water. Its outputs are 98 mass% H2SO4, 2 mass% H2O sulfuric acid and dilute SO2, O2, N2 gas. The acid output combines gas dehydration tower acid, H2SO4 making tower acid and liquid water. The equivalent sulfur burning acid plant sends moist air (rather than moist feed gas) to dehydration. Appendix V gives an example sulfur burning calculation.

C.2.3 100 mL sulfuric acid (H2SO4, sp gr 1.84) Reagent water to make 1000 mL 1 to 3 min 20 to 25°C Remove bulky corrosion products before treatment to minimize copper redeposition on specimen surface. 

DeteiTnine how many grams of each of the following solutes would be needed to make 2.50 X 10" mL of a 0.100 M solution (a) cesium iodide (Csl), (b) sulfuric acid (H2SO4), (c) sodium carbonate (Na2C03), (d) potassium dichromate (K2Cr207),... 

Sulfur is a yellow solid that exists as several allotropes that form when sulfur is heated to different temperatures. Elemental sulfur is found in nature in underground deposits and is mined by the Erasch Process, which uses hot water to melt the sulfur so that is can be forced to the surface with compressed air. Most of the mined sulfur is used to make sulfur dioxide (SOj). The most important compound of sulfur is sulfuric acid (H2SO4). This compound is made by converting SO2 to SO3 and then reacting the SO3 with water. Sulfuric acid is the largest volume chemical produced in this United States. 

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