Of magnesium metal

Alagnesium Fluoroborate. Treatment of magnesium metal, magnesium oxide, or magnesium carbonate with HBF gives magnesium fluoroborate [14708-13-5]. The MgF2 is filtered and the product is sold as a 30% solution. 

The abihty of magnesium metal to reduce oxides of other metals can be exploited to produce metals such as zirconium, titanium [7440-32-6] and uranium [7440-61-1] (see ZiRCONiUMAND ZIRCONIUM COMPOUNDS Titaniumand titanium alloys Uraniumand uranium compounds). These reactions are... 

When magnesium oxide is chlorinated in the presence of powdered coke or coal (qv), anhydrous magnesium chloride is formed. In the production of magnesium metal, briquettes containing CaCl2, KCl, NaCl, MgO, and carbon are chlorinated at a temperature such that the electrolyte or cell melt collects at the bottom of the chlorinator, enabling the Hquid to be transferred directly to the electrolytic cells. 

Economic Aspects and Uses. Magnesium hydroxide and magnesium chloride are used as a basic feedstock to make elemental magnesium, MgO refractories, and reactive chemicals. One hundred and sixty thousand tons of magnesium metal were produced ia the United States in 1989 in addition to 1,013,000 tons of MgO equivalent in magnesium compounds (qv) (54). 

The Alcan process has been used commercially by Osaka Titanium Co. ia Amagasaki, Japan. Multipolar ceUs of 1000 t/yr capacity are ia operation. Energy consumption is about 9.5—10 kWh/kg of magnesium metal (111). 

At the metal surface, the radical species R and MgX combine to form the Grignard reagent 2, which subsequently desorbs from the surface into solution. Macroscopically, the overall process is observed as a continuous decrease of the amount of magnesium metal. 

Two moles of magnesium oxide require two moles of magnesium metal. Thus,... 

We could have decided to begin by choosing one mole of magnesium metal as the amount of reactant consumed in (a) ... 

Sf.lf-Tksi 12.15A Determine the mass (in grams) of magnesium metal that can be obtained from molten magnesium chloride, by using a current of 7.30 A for 2.11 h. What volume of chlorine gas at 25°C and 1.00 atm will be produced at the anode ... 

Write the chemical equation for (a) the industrial preparation of magnesium metal from the magnesium chloride in seawater (b) the action of water on calcium metal. 

In 2009, Ritter and coworkers reported a stereo- and regio-selective 1,4-addition of a-olefins to 1,3-dienes catalyzed by the mixmre of FeCl2, the iminopyridine ligand (LI or L2), in the presence of magnesium metal (Scheme 30) [108]. This combination is also adaptable to the 1,4-hydroboration of 1,3-dienes (see 3.2). 

C02-0031. When a strip of magnesium metal bums in air, the mass of the resulting residue is greater than the mass of the original strip of metal. Explain this observation in terms of conservation of mass. 

The reaction of magnesium metal with aqueous strong acid, which appears in Figure 4-12. illustrates the fundamental principles of oxidation-reduction. When a piece of magnesium is dropped into a solution of hydrochloric acid, a reaction starts almost Immediately. The metal dissolves, and gas bubbles from the solution. The gas is H2, and analysis of the solution reveals the presence of ions. A list of chemical species before and after the reaction... 

Redox reactions of metals with acids are described in Chapter 4. Oxidation of the metal generates hydrogen gas and an aqueous solution of ions. Suppose that 3.50 g of magnesium metal is dropped into 0.150 L of 6.00 M HCl in a 5.00-L cylinder at 25.0 °C whose initial gas pressure is 1.00 atm, and the cylinder is immediately sealed. Find the final partial pressure of hydrogen, the total pressure in the container, and the concentrations of all ions in solution. 

A simple example of a redox reaction Is the violent reaction of magnesium metal with molecular oxygen to generate magnesium oxide, shown in Figure 19-1 2 Mg( ) + 02(g) 2 MgO(5 ) In magnesium metal, each atom is... 

A starting material loses electrons in an oxidation, so electrons appear among the products of the oxidation half-reaction. A starting material gains electrons in a reduction, so electrons appear among the reactants of the reduction half-reaction. The reaction of magnesium metal with hydronium ions to produce hydrogen gas provides an example Mg(.y) -I- 2H3 0 ((2 q) q) H2(g) + 2H2 0(/) Here are the half-reactions for this... 

The reaction of magnesium metal with an alkyl or aryl halide in diethyl ether is the standard method for synthesis of Grignard reagents. The order of reactivity of the halides is RI > RBr > RC1. 

That day fifty tons of magnesium metals and alloys were made at Bitterfeld and Aken — a 65 per cent increase over the 1932 rate. Krauch s plans called for another 65 per cent increase by 1943. And Farben made fifty tons of aluminum, with similar increases called for. 

Calculate the mass of magnesium chloride that would be obtained when 48 g of magnesium metal is reacted completely with chlorine (Mg = 24, Cl = 35.5). 

Dow seawater A process for extracting magnesium from seawater. Calcined dolomite (CaO-MgO, dololime), or calcined oyster shell, is added to seawater, precipitating magnesium hydroxide. This is flocculated, sedimented, and filtered off. For use as a refractory it is calcined for the manufacture of magnesium chloride for the manufacture of magnesium metal, it is dissolved in hydrochloric acid. Developed by the Dow Chemical Company and later operated by the Steetly Company in West Hartlepool, UK, and Sardinia. 

We can explain this in terms of a rate expression, as follows. First, consider the case where 1 mol of magnesium is reacted with 1 mol of sulphuric acid (we will also say that the overall volume of the solution is 1 dm3). Initially there is no product, but at the end of reaction there will be 1 mol of MgS04 and 0 mol of magnesium metal or sulphuric acid. Therefore, the amount of product in creases while the amounts of the two reactants will both decrease as the reaction proceeds. The amounts of material change and, as the volume of solution is constant, the concentrations change. 

Magnesium, the alkaline earth metal next to sodium in the periodic table, has a relatively strong tendency to give up its two outermost electrons, but this tendency is much less than that of sodium. When a fresh surface of magnesium metal is exposed to water, the reaction occurs very slowly ... 

A sample of magnesium metal is heated in the presence of nitrogen gas. After the sample was heated, some water was added to it. Which of the following statements is false ... 

For the reaction of magnesium metal with aluminum ions, the two balanced half-reactions include different numbers of electrons, 2 and 3. The least common multiple of 2 and 3 is 6. To combine the half-reactions and give a balanced net ionic equation, multiply the balanced halfreactions by different numbers so that the results both include six electrons, as shown below. 

K.S. Jung, E.Y. Lee, K.S. Lee, Catalytic effects of metal oxide on hydrogen absorption of magnesium metal hydride, J. Alloys Compd. 421 (2006) 179-184. 

Magnesium chloride ((MgCy is mostly obtained from saltwater and has many uses, including as the source of magnesium metal during electrolysis, as a catalyst, and in the making of ceramics, lubricants, paper and textiles, and disinfectants. 

In a balanced chemical equation, the number of atoms of each element on the left-hand, or reactant, side will equal the number of atoms of eaeh element on the right-hand, or product, side. The above equation states that one mole of potassium perchlorate (KCIO 4, a reactant) will react with 4 moles of magnesium metal to produce one mole of potassinm chloride (KCl) and 4 moles of magnesinm oxide (MgO). 

---