Also Haber process

H+], calculation of, 192, see also Hydrogen ion Haber, Fritz, 151 Haber process, 140, 150 Hafnium, oxidation number, 414 Haldane, J. B. S., 436 Half-cell potentials effect of concentration, 213 measuring, 210 standard, 210 table of, 211, 452 Half-cell reactions, 201 Half-life, 416 Half-reaction, 201 balancing, 218 potentials, 452 Halides... 

In this chapter, we present basic features of chemical equilibrium. We explain why reactions such as the Haber process cannot go to completion. We also show why using catalysts and elevated temperatures can accelerate the rate of this reaction but cannot shift Its equilibrium position in favor of ammonia and why elevated temperature shifts the equilibrium In the wrong direction. In Chapters 17 and 18, we turn our attention specifically to applications of equilibria. Including acid-base chemistry. 

Bosch also helped develop Haber s process into an industrial process. In 1913, Haber and Bosch opened an ammonia manufacturing plant in Germany. A year later, World War I started. Saltpeter had another use besides making fertilizer. It was also necessary to make nitric acid that was used to make explosives. When the war started, the British Navy quickly cut off Germany s supply of Chilean saltpeter. If not for the Haber process, some historians estimate that Germany would have run out of nitrates to make explosives by 1916. The war lasted another two years, however, because Germany did not need to rely on outside sources of nitrates for fertilizers or explosives. 

Haber process, 22 792 Hackling, 77 292 Hackmanite, color, 7 338 Haemanthamine, 2 87 Hafnium (Hf), 73 78-97 26 637. See also Hafnium compounds analytical methods for, 73 87-88 chemical properties of, 73 80 economic aspects of, 73 86-87 health and safety factors related to, 73 88... 

As we have discussed previously, the balanced chemical equation not only indicates which chemical species are the reactants and the products, but also indicates the relative ratio of reactants and products. Consider the balanced equation of the Haber process for the production of ammonia ... 

SCFs will find applications in high cost areas such as fine chemical production. Having said that, marketing can also be an issue. For example, whilst decaffeina-tion of coffee with dichloromethane is possible, the use of scCC>2 can be said to be natural Industrial applications of SCFs have been around for a long time. Decaffeination of coffee is perhaps the use that is best known [16], but of course the Born-Haber process for ammonia synthesis operates under supercritical conditions as does low density polyethylene (LDPE) synthesis which is carried out in supercritical ethene [17]. 

Carl Bosch developed the industrial stages for the Haber Process. The perfection of the Haber-Bosch process was used by Germany during World War I. Haber also worked on the thermodynamics of gaseous reactions, the electrochemistry and the explosion of gases. 

The reactant adsorbs, or attaches, to the catalyst s surface. As a reactant molecule adsorbs, its bonds are weakened and the reaction can proceed more quickly because the bonds are more easily broken (Fig. 13.31). One important step in the mechanism of the Haber process is the adsorption of N2 molecules on the iron and the weakening of the strong N=N triple bond. As mentioned at the beginning of this chapter, adsorption onto a metal such as platinum is also used to dissociate the bond in H2 to accelerate the electrolysis of water. 

Nitrogen In the production of ammonia by the Haber process (see p. 176) the ammonia is then used to make nitric acid, which is used in the manufacture of dyes, explosives and fertilisers In liquid form, as a refrigerant As an inert atmosphere for some processes and chemical reactions, because of its unreactive nature for example, empty oil tankers are filled with nitrogen to prevent fires In food packaging to keep the food fresh, for example in crisp packets where it also prevents the crisps being crushed (Figure 11.10)... 

Man has also found a way of converting nitrogen present in the air to ammonia. The process for preparing ammonia is known as the Haber process. 

Haber process also known as the Haber-Bosch process, this industrial process uses nitrogen (N2) and hydrogen (H2) to produce NH3. 

A catalyst is a substance that speeds up a reaction without being consumed itself. Just as virtually all vital biological reactions are assisted by enzymes (biological catalysts), almost all industrial processes also benefit from the use of catalysts. For example, the production of sulfuric acid uses vana-dium(V) oxide, and the Haber process uses a mixture of iron and iron oxide. 

Explain the dependence of the yield of ammonia upon temperature and pressure in the Haber process, and also explain the role of the catalyst. 

Much of the ammonia made by the Haber Process is used directly in the manufacture of fertilisers, but large quantities are also converted to nitric acid which is used in the ... 

Nitrogen combines directly with uranium at a temperature of 1000° 1 nitrogen or ammonia reacts with the carbide, yielding a nitride dry ammonia also produces a nitride when it reacts with uranium tetrachloride. The formula of the nitride is usually U N . The catalytic influence of uranium carbide in the manufacture of ammonia by the Haber process is attributed to the formation of the nitride. 

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