its ore: [pic] Because both reduction and oxidation are going on side-by-side‚ this is known as a redox reaction. Oxidising and reducing agents An oxidising agent is substance which oxidises something else. In the above example‚ the iron(III) oxide is the oxidising agent. A reducing agent reduces something else. In the equation‚ the carbon monoxide is the reducing agent. • Oxidising agents give oxygen to another substance. • Reducing agents remove oxygen from another substance. Oxidation
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FD & C Blue #1 aluminum lake (in 25 mg tablet)‚ FD & C Red #40 aluminum lake (in 25 mg tablet)‚ FD & C Blue #2 aluminum lake (in 50 mg tablet)‚ hydroxypropyl cellulose‚ hypromellose‚ magnesium stearate‚ microcrystalline cellulose‚ polyethylene glycol‚ polysorbate 80‚ sodium starch glycolate‚ synthetic yellow iron oxide (in 100 mg tablet)‚ and titanium dioxide. Zoloft ZOLOFT is supplied for oral administration as scored tablets containing sertraline hydrochloride equivalent to 25‚ 50 and 100 mg
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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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each bottle would most readily enable the bottles to be correctly relabelled? A B C D ammonia hydrochloric acid lead(II) nitrate sodium hydroxide © UCLES 2011 5070/11/O/N/11 3 3 Oxygen was prepared from hydrogen peroxide‚ with manganese(IV) oxide as
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Color:- Most of the metals are grey in color. But gold and copper are exceptions. Chemical Properties of Metals: Part-I Reaction with oxygen:- Most of the metals form respective metal oxides when react with oxygen. Examples: (1) Reaction of potassium with oxygen:- Potassium metal forms potassium oxide when reacts with oxygen. (2) Reaction of sodium with oxygen:- Sodium metal forms sodium
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causes nausea and vomiting Uses: • gastric antacid for hyperchlorhydria • for intestinal toxemia CALCIUM-CONTAINING ANTACIDS • dependent upon their basic properties • raise stomach pH to 7 • constipating • found in combinations with magnesium antacids 1. CALCIUM CARBONATE • precipitated chalk • fast action • found in combinations with Mg antacids • in Lozenges and Oral suspension 2. TRIBASIC CALCIUM PHOSPHATE • Precipitated Calcium Phosphate‚ Tertiary Calcium
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THE CHEMICAL EARTH: 1. The living and nonliving components of the Earth contain mixtures ● Construct word and balanced formulae equations of chemical reactions as they are encountered Reactants → products Chemical reaction: the way atoms are joined changes‚ atoms are not created nor destroyed‚ but are rearranged Indicators: emission of light or heat‚ odour formation of a gas formation of a precipitate colour change change in state aqueous = dissolved in water‚ an aqueous solution
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atmospheric condition i.e.‚ moist air‚ carbon dioxide form undesirable compounds on the surface is known as corrosion‚ The compounds formed are usually oxides . Rusting is also a type of corrosion but the term is restricted to iron or products made from it .Iron is easily prone to rusting making its surface rough. Chemically‚ rust is a hydrated ferric oxide. Titanic‘s bow exhibiting microbial corrosion damage in the form of ‘rusticles’ Rusting an Electrochemical Mechanism ; Rusting may be explained
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COMPOUNDS “Analytical chemistry -I” http://foricseandbeyond.blogspot.in/ metal oxide “Oxides of metals are generally stable to heat and they are considered to be most stable form of compound found in nature.” Oxides of potassium‚sodium‚calcium‚magnesium‚ aluminum ‚ zinc‚iron‚lead and copper are stable to heat uO C PbO Zn O http://foricseandbeyond.blogspot.in/ MERCURIC OXIDE “Mercury(II)oxide” “orange red” 2HgO 2Hg + O2 1.The amorphous powder changes to dark red and
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spontaneous (∆G < 0). The second reaction involved magnesium ribbon. Two slabs of dry ice were set-up‚ with holes carved on both of them. When the magnesium ribbon was lighted on the first slab of ice‚ it produced a bright‚ white light‚ and was quickly covered with the second slab of dry ice. The reaction produced very bright light (which may cause blindness) and some sparks (exothermic reaction took place)‚ which signified that the reaction between magnesium solid and carbon dioxide gas had been proceeding
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