It can have harmful effects on plants‚ aquatic animals and infrastructure. Acid rain is caused by emissions of sulfur dioxide and nitrogen oxide‚ which react with the water molecules in the atmosphere to produce acids. Governments have made efforts since the 1970s to reduce the release of sulfur dioxide into the atmosphere with positive results. Nitrogen oxides can also be produced naturally by lightningstrikes and sulfur dioxide is produced by volcanic eruptions. The chemicals in acid rain can cause
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AgNO3 silver nitrate 7761-88-8 Ag2O silver oxide 1301-96-8 AgONC silver fulminate 5610-59-3 AgSNC silver thiocyanate 14104-20-2 Ag2C2 silver acetylide 7659-31-6 Ag2CO3 silver(I) carbonate 534-16-7 Ag2C2O4 silver oxalate 533-51-7 Ag2Cl2 silver(II) dichloride 75763-82-5 Ag2CrO4 silver chromate 7784-01-2 Ag2Cr2O7 silver dichromate Ag2F silver subfluoride 1302-01-8 Ag2MoO4 silver molybdate 13765-74-7 Ag2O silver(I) oxide 20667-12-3 Ag2S silver sulfide 21548-73-2
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Mg(OH)3 | 25 | Methane formula | CH4 | 26 | Nitrogen monoxide formula | NO | 27 | Potassium hydroxide formula | KOH | 28 | Sodium nitrate formula | NaNO3 | 29 | Sulfurous acid formula | H2SO3 | 30 | Phosphate formula | PO4- | 31 | Aluminum oxide formula | Al2O3 | 32 | Ammonia chemical formula | NH4 | 33 | Ammonium nitrate formula | NH4NO3 | 34 | Ammonium phosphate formula | (NH4)3PO4 | 35 |
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water; soluble in fuming sulfuric acid. Thermochemical Properties ∆Ηƒ° ∆Gƒ° S° Cρ ∆Hvap 12.37 kcal/mol 15.81 kcal/mol 62.55 cal/degree mol 10.68 cal/degree mol 6.16 kcal/mol Preparation Nitrosyl chloride can be prepared by the reaction of nitric oxide with chlorine: 2NO + Cl2 → 2ClNO Also‚ nitrosyl chloride is produced by the action of chlorine on sodium nitrate; or by the reaction of nitrosyl sulfuric acid with hydrochloric acid: NaNO3 + Cl2 → ClNO + NaClO2 ONHSO4 + HCl → ClNO + H2 SO4 Nitrosyl
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NSS Chemistry Part 3 Metals HKCEE Past Paper Questions – Structural Questions 1. HKCEE 1995 Q1 Rubidium (Rb) and potassium belong to the same group in the Periodic Table. The relative atomic mass of rubidium is larger then that of potassium. (a) Explain whether rubidium is more reactive than potassium. (b) Write a chemical equation for the reaction between rubidium and water. (State symbols should be given.) (c) Suggest how rubidium can be stored safely in the laboratory.
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the tin and nitric acid inside. Heat for about 15 minutes‚ let the crucible with the now contained tin oxide‚ cool on the wire gauze again and measure its mass. Repeat the heating process without adding anything to the crucible for an additional 15 minutes. After finding the mass of the tin oxide‚ by subtracting the initial weight of the crucible from the weight of the crucible with the tin oxide‚ we can compare the two measurements. Data:
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yield a metal of greater than 75% purity. Final purification of nickel oxides is performed via the Mond process‚ which increases the nickel concentrate to greater than 99.99% purity. The Mond process‚ sometimes known as the carbonyl process is a technique created by Ludwig Mond in 1890 to extract and purify nickel. The process was used commercially before the end of the 19th century. It is done by converting nickel oxides (nickel combined with oxygen) into pure nickel. Spheres of Nickel
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amounts gas levels - co2 rises due to burning fossil fuels + deforestation - co rises due to incomplete combustion of fossil fuels - so2 rises due to volcanoes + burning sulfur impurities - methane rises due to cattle waste gases - nitrogen oxides rise due to lightning + car engines rocks - igneous formed when magma or lava cool to form solids - large crystals mean the rock cooled slowly - small crystals mean the rock cooled quickly - eg granite - sedimentary rock formed by layers
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into the corresponding oxides and carbon dioxide. The temperature of decomposition depends upon the activity of the metal; that is to say‚ the more active the metal‚ the more stable is the carbonate. Thus‚ the carbonates of sodium and potassium are stable at the highest temperature of a Bunsen burner flame‚ whereas the carbonates of silver and copper are easily decomposed. In this experiment copper (ii) carbonate will be decomposed at a high temperature‚ forming copper (ii) oxide and carbon dioxide:
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Chapter 1 Chemical Reactions and Equations Q.1. Why should magnesium ribbon be cleaned before burning in air ? Ans: Magnesium ribbon is a very reactive metal. When stored it reacts with oxygen to form a layer of magnesium oxide on its surface. This layer of magnesium oxide being a stable compound prevents further reaction of magnesium with oxygen. The magnesium is cleaned before burning in air to remove this layer so that the metal can be exposed to air properly. Q.2. Write the balanced equation
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