40 – 60 % propene is used for the manufacture of 2-propanol. A large number of catalysts for 2-propanol dehydrogenation have been studied‚ including copper‚ zinc‚ and lead metals‚ as well as metal oxides‚ e.g.‚ zinc oxide‚ copper oxide‚ chromium-activated copper oxide‚ manganese oxide‚ and magnesium oxide. Inert supports‚ such as pumice‚ may be used. CH3CH=CH2 CH3CH(OH)CH3 CH3COCH3 +H2 (3) By catalytic oxidation of Propene (Wacker-Hoechst). The process is analogous
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acidic presents two different problems for crops. First‚ the amount of necessary minerals in the soil such as potassium and calcium decreases. Second‚ aluminum and manganese levels increase to potentially toxic levels below a pH of roughly 5.5.Calcium oxide‚ addresses the problem. It reacts in water to release calcium ions and hydroxide ions‚ which raise the pH of the soil.The soil which is too acidic will be neutralised by the lime which is alkaline. H2O + CO2 -> H2CO3 2SO2 + H2O + O2 -> 2H2SO4
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Compound and Its Parent Elements Hypothesis The hypothesis of this experiment is magnesium oxide can be synthesized by combining (burning) the magnesium with oxygen. The chemical and physical properties of each element (magnesium‚ oxygen‚ and magnesium oxide) might be different‚ from the state‚ color‚ electrical conductivity‚ and pH. Aim This experiment was performed to synthesize magnesium oxide by direct combination of magnesium and oxygen and to compare the properties of the elements (magnesium
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explode. It reacts with non-metallic elements except for nitrogen‚ oxygen‚ noble gases‚ silicon and halogens. It oxides them to their highest oxidation states(3) as acids with the formation of nitrogen dioxide for concentrated acid and nitric oxide for dilute acid. Chromium (Cr)‚ iron (Fe) and aluminium (Al) dissolve in dilute nitric acid‚ which the concentrated acid forms a metal oxide layer that protects the metal from further oxidation‚ and it is called passivation. Nitric acid can be made
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experiment. Keeping that in mind‚ I checked the information of each reactants and products on online resources. Not only did that help me realize the Aluminum was oxidized‚ it helped me understood that the product was the gray Copper (II) Oxide instead of the red Copper (I) Oxide. This was one of the problems that I was able to solve by careful observation and checking additional
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BALANCE EACH EQUATION BEFORE SOLVING ANY PROBLEMS. SHOW ALL WORK. 1. ___Cu + ___O2 ___CuO a. If 101 grams of copper is used‚ how many moles of copper (II) oxide will be formed? b. If 5.25 moles of copper are used‚ how many moles of oxygen must also be used? c. If 78.2 grams of oxygen react with copper‚ how many moles of copper (II) oxide will be produced? 2. ___C4H10 + ___O2 ___CO2 + ___H2O a. How many moles of butane‚ C4H10‚ are needed to react with 5.5 moles of oxygen? b. How many
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furnace is a huge‚ steel stack lined with refractory brick. The purpose of the blast furnace is to chemically reduce and physically convert the iron oxide in to liquid iron called “hot metal” Three substances are needed for this extraction and the combined mixture of them is called the “charge”: Haematite (iron ore): contains sand with iron oxide (Fe2O3) Limestone: calcium carbonate Coke: mainly carbon They are put
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Q. 7. Ammonium salts decomposes on heating. What other property do ammonium salts have in common ? Q. 8. The following reactions are carried out : A: Nitrogen + metal → compound X B: X + water → ammonia + another compound C: Ammonia + metal oxide → metal + water + N2. (1) One metal that can be used for reaction A is magnesium. i. Write the formula of the compound X formed. ii. Write the correctly balanced equation for reaction B where X is the compound formed. iii. What property of ammonia
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oxygen: Burns brightly when heated in air to form a white powder of ionic magnesium oxide Mg2+O2- when heated strongly in air. 2Mg(s) + O2(g) ==> 2MgO(s) Reaction of oxide with water: It is slightly soluble in water‚ and is a basic oxide forming an alkaline solution of magnesium hydroxide Mg2+(OH-)2‚ of about pH12. MgO(s) + H2O(l) ==> Mg(OH)2(aq) Reaction of oxide with acids: Behaves as a basic oxide dissolving to form the chloride‚ sulphate and nitrate salt in the relevant dilute acid
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hydrogen ions. The metal is‚ of course‚ oxidised to positive metal ions because it loses electrons. But nitrate ions are also easily reduced to products like nitrogen monoxide and nitrogen dioxide. So metals reacting with nitric acid tend to give oxides of nitrogen rather than hydrogen. If the acid is relatively dilute‚ you tend to get nitrogen monoxide‚ although this immediately reacts with oxygen in the air to make brown nitrogen dioxide. Concentrated nitric acid gives
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