the bacteria is positive‚ then we chlorinate the well. After we make sure all the chlorine is throughout the house‚ we let it sit for 24 hours to disinfect the pipes and the well. Then we flush the system so there is no more chlorine and resample the bacteria. If you have high nitrates or pesticides‚ then you should activate carbon and chlorinate at the end. If you have high metals‚ then you should add chlorine at
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warfare relies on the physiological effects of specific chemicals. Chemical warfare was a great weapon in wars due to it being a silent‚ invisible‚ and a very deadly way to harm enemies. Chemical warfare started in 1915 where the German army used chlorine gas against the allied troops during World War I. There are many types of chemical warfare agents such as‚ choking gases and lung irritant agents‚ blister agents‚ blood agents‚ and nerve agents. Choking gases and lung irritant agents affect the breathing
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ferons) are stable non-corrosive and inert compounds containing chlorine‚ fluorine and carbons. They are extensively used as the coolants in refrigerators‚ air conditioners and as propellants in aerosol cans and in plastic forms. These CFC molecules‚ once they escape into the atmosphere‚ migrate to the stratosphere and decompose to release chlorine atoms in the ozone layer. CCL2F2 CCLF2 + Cl---------- (i) Then the chlorine atom attacks the ozone moleculs Cl + O3 ClO + O2-------------(ii)
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reaction using thionyl chloride. The carboxylic acid is converted into an acyl chloride because the acyl chloride is more reactive. In this step‚ hydrochloric acid is formed from a hydrogen on the carboxylic acid and a chlorine from the thionyl chloride atoms binding together. A chlorine atom then attaches itself to a double bonded oxygen on the acyl chlorosulfite‚ kicking the double bonded oxygen’s electrons up making it negatively charged. The negatively charged
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Chemistry F332 Notes Ions in solids and solutions: Structure of an ionic lattice (Sodium Chloride): * Consists of sodium ions (Na+) surrounded by six chloride ions (Cl-) * Chloride ions also surrounded by six sodium ions. * Held together by attraction of oppositely charged ions. * Giant ionic lattice. * Electrostatic bonds hold lattices together. * Structure is simple cubic. * Some ionic crystals contain water. * Known as water of crystallisation. * These crystals
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1: The reaction between chlorine and iron(II) ions Chlorine gas oxidises iron(II) ions to iron(III) ions. In the process‚ the chlorine is reduced to chloride ions. You would have to know this‚ or be told it by an examiner. In building equations‚ there is quite a lot that you can work out as you go along‚ but you have to have somewhere to start from! You start by writing down what you know for each of the half-reactions. In the chlorine case‚ you know that chlorine (as molecules) turns into
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Sometimes you will have a high level of salt or not enough chlorine. In order to maintain a safe swimming pool you need to be sure that everything is working as it should be. If you find that you are frequently running into problems one easy solution could be to monitor it more closely. If you spend an hour per week
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Cfcs Cause Deterioration of the Ozone Layer The deterioration of the ozone layer ‚ caused by Cfcs‚ endangers the lives of humans ’. Cfcs have a diminishing effect on the ozone layer. Furthermore‚ the deterioration of the ozone cause an increase of Ultraviolet (UV) radiation which can have a negative effect on human skin and eyes. As a writer for newsweek‚ I have investigated the scenario and found the following information. The earth ’s atmosphere is a blanket of air that surrounds the planet
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react • The ability to oxidise decreases down Group 7 • This can be shown by halogen displacement reactions where elements higher up the group will displace elements further down the group • This can be done with chlorine dissolved in water or by bubbling chlorine gas through NaBr(aq) or NaI(aq) Cl2 + 2NaBr ( 2NaCl + Br2 Pale green solution Yellow solution/orange in hexane Cl2 + 2NaI ( 2NaCl + I2 Pale green solution Brown solution/purple
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FORM 4G ELECTROLYSIS WORKSHEET TERM 3 2010-2011 1.Figure 1 below is a diagram of the apparatus used in the electrolysis of fused sodium bromide. Figure 1 a)Write the formulae for the ions present in the fused sodium bromide. b)Write an ionic equation to represent the reaction taking place at the positive and negative electrodes. c)When the heat source was removed‚ the crucible cooled and the lamp went out. Explain why the lamp went out when the crucible cooled. d)At the end of the experiment
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