Δ(Product) Δ(Time) http://www.one-school.net/notes.html Rate of Reaction = 1 Δ(Product) Δ(Time) ONE-SCHOOL.NET Chemical Reaction Precipitation of Sulphur 2HCl(aq) + Na2S2O3(aq) ⎯→ 2NaCl(aq) + S(s) + SO2(g) + H2O(l) Na2S2O3: Sodium thiosulphate Notes: 1. Yellow precipitate (sulphur) is formed. 2. The reaction is slow. Potassium Dichromate (VI) with Ethanedioic Acid Cr2O72- + 14H+ + 3C2O42- ⎯→ 6CO2 + 7H2O + 2Cr3+ Notes: 1. In the reaction‚ the orange colour of the
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sulphur oxygen sulphur trioxide 2 Fe + O2 ---------> 2 FeO iron oxygen iron (II) oxide Decomposition
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the benzene and the benzene reacted with the explosives resulting in that huge explosion. f) Try to make the reaction endothermic instead of exothermic. g) Reaction 1: decomposition Reaction 2: single displacement Reaction 3: Synthesis h) It is incorporated because it reacts very quickly with sodium and releases sodium oxide. 1. It must produce heat when it reacts‚ it must produce gases as products‚ it must react very quickly‚ and it must be stable enough so that it can be exploded in controlled
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page) Group I II III IV V VI VII 0 1 4 H He Hydrogen Helium 1 7 9 11 12 14 16 19 2 20 Li Be B C N O F Ne Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon 3 23 4 24 5 27 6 28 7 31 8 32 9 35.5 10 40 Na Mg Al Si P S Cl Ar Sodium Magnesium Aluminium Silicon Phosphorus Sulphur Chlorine Argon
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sulfur dioxide gas” i. CuS + O2 Cu + SO2(g) b. When heated‚ baking soda (sodium hydrogen carbonate) decomposes to form the products sodium carbonate‚ carbon dioxide‚ and water.” i. NaHCO3 Na2CO3 + CO2 + H2O 11. Write and balance equations for the following reactions. a. “Iron metal and chlorine gas react to form solid iron(III) chloride” i. 2FeCl3(s) b. “Solid aluminum carbonate decomposes to form solid aluminum oxide and carbon dioxide gas” i. Al2O3(s) + CO2(g)
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concentration of H+(aq) ions by titrimetric analysis. 9 F The hydrogen gas formed in the reaction between zinc and dilute hydrochloric acid CANNOT escape from a closed reaction vessel. Thus‚ the mass of the reaction mixture would NOT decrease as the reaction proceeds. 10 F It is difficult to measure the volume of water produced from the reaction between oxalate ions and permanganate ions in aqueous solution. 1 11 T During the decomposition of hydrogen peroxide solution‚ oxygen gas is formed. 2H2O2(aq)
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acid H2S2O7 (l) + H2O (l) 2H2SO4 (l) ELECTROLYSIS of Sodium Chloride: Molten NaCl: Overall reaction: 2NaCl (l) 2Na (l) + Cl2 (g) Half-equations: 2Cl− (l) Cl2 (g) + 2e− Na+ (l) + e− Na (s) Concentrated NaCl: Half-equations: 2Cl− (aq) Cl2 (g) + 2e− 2H2O (l) + 2e− H2 (g) + 2OH− (aq) Dilute NaCl: Half-equations: 2H2O (l) O2 (g) + 4H+ (aq) + 4e− 2H2O (l) + 2e− H2 (g) + 2OH− (aq) Overall reaction: 2H2O (l) 2H2 (g) + O2 (g) Production of SODIUM HYDROXIDE: Mercury Cell: Electrolytic half-equations:
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IGSCE Chemistry Notes Oxides Oxides are used to determine whether an element is a metal or a non-metal. Most non-metals are classed as acidic oxides. While most metals are classed as basicoxides. Acidic Oxides * Reacts with water to form acids * Neutralises alkaline solution to form salt + water Basic Oxides * Neutralises acidic solutions to form salt + water Amphoeteric Oxides * These are non-metals which display both acidic and basic properties Alkaline Oxides * Reacts
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chalk + limestone (from calcium carbonate) - metamorphic rock has crystals - formed by heat + pressure on sedimentary rock - contains interlocking crystals - eg marble (from limestone or chalk) quarrying limestone - produces local jobs in rural areas + improves economy - quarries can be landscaped after - used 4 making cement (heated w powdered clay) - used 4 making concrete (mix cement + sand + gravel + water) - used 4 making glass (heated w sodium carbonate + sand) - all used to construct
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The goal for this experiment is to determine which out of the four balanced chemical equations best represent the thermal decomposition of sodium bicarbonate. The guiding question will be answered with the outcome of the sodium bicarbonates thermal decomposition and it being plugged in into the four balanced chemical equations. John Dalton atomic theory explains two fundamental laws of chemistry which are the law of conservation of mass and the law of definite proportions. The atomic theory states
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