sodium chlorite‚ NaClO2; sodium hypochlorite‚ NaClO; and sodium chloride‚ NaCl. All are white solids at room temperature. It is possible to determine the chemical equation for the decomposition of sodium chlorate by applying the principles of stoichiometry to the masses of the reactants and products. Safety Precautions: Sodium chlorate is a strong oxidizing agent and a dangerous fire risk; it is slightly toxic by ingestion. Contact with metal powders or combustible organic compounds may cause
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mCn Hm + (n +m/4)O2 = nCO2 + m/2 H2O + Q S + O2 = SO2 + 9260 kJ/kg of sulfur Calcination CaCO3 = CaO + CO2 – 1830 kJ/kg of CaCO3gCO3 = MgO + CO2 – 1183 kJ/kg of MgCO3. Sulfation CaO + SO2 + 1/2 O2 = CaSO4 + 15141 kJ/kg S. Basic Stoichiometry C + O2 = CO2 + q 1 kmol of carbon combines with 1 kmol of oxygen to produce 1 kmol of carbon dioxide and release q amount of heat. 1 kmol of reactant = M kg of the reactant when M is the molecular weight of the reactant. So mass
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Synopsis The objective of this experiment is to determine the percentage by mass of calcium carbonate‚CaCO3 in toothpaste using back titration technique. A known weight portion of toothpaste is obtained to react with known volume and concentration of standard acid solution. After completing the reaction‚ the resulting solution containing excess acid is back titrated with known volume and concentration of standard base solution. Determination of excess acid after reaction allow us to calculate the
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MAC1105 CO-REQUISITES: CHM1045L Upon successful completion of this course‚ the students should be able to demonstrate a familiarity with introductory material in general chemistry such as units for measurement‚ formula writing and nomenclature‚ stoichiometry‚ atomic structure‚ periodicity and bonding‚ terms and problem solving in the areas of changes of state‚ acid and base chemistry‚ ionic reactions‚ oxidation-reduction reactions‚ solutions and descriptive chemistry of selected non-metals. The students
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potassium iodide. The reaction will release iodine:Example: (a) With KMnO4 2MnO4- + 16H+ + 10I(b) With KIO3 IO3- + 5I+ 6H+ 3I2 + 3H2O 2Mn2+ + 5I2 + 8H2O The iodine that is released is titrated against a standard thiosulphate solution. From the stoichiometry of the reaction‚ the amount of iodine can be determined and from this‚ the concentration of the oxidising agent which released the iodine‚ can be calculated. In an iodometric titration‚ a starch solution is used as an indicator as it can absorb
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Manufacture of Paracetamol Introduction Paracetamol‚ the most common medicine nowadays‚ has been used by people
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1 Class XII: Chemistry Chapter 1: The Solid State Concept 1. Solid: Solid is a state of matter in which the constituting particles are arranged very closely. The constituent particles can be atoms‚ molecules or ions. Properties of solids: a. They have definite mass‚ volume and shape. b. Intermolecular distances are short and hence the intermolecular forces are strong. c. Their constituent particles have fixed positions and can only oscillate about their mean positions. d. They are incompressible
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Abstract Gold‚ silver‚ copper‚ lead‚ and mercury are some of the ancient elements. Hennig Brand discovered phosphorus the first element. After the discovery of phosphorus‚ many more elements were discovered. Johann Dobereiner discovered that elements could be grouped in three sets and proposed the Law of Triads. Later‚ A.E.Beguyer de Chancourtois arranged the elements according to their atomic mass and created the first geometrical representation of the periodic table. John Newlands proposed the
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combined is the equivalence point. An example of this is shown in the equation: HCl(aq)+NaOH(aq)NaCl(aq)+H2O(l). The number of moles is given by knowing the exact concentration and volume added of the titrant. The latter‚ in turn‚ is related by stoichiometry to the number of moles of acid initially present in the unknown. To detect the equivalence point‚ indicators are usually added to acid-base titrations. The point at which the indicator changes color and signals the equivalence point has been reached
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objective was to accurately and precisely convert the unknown sample containing the chloride analyte to another known solid‚ silver chloride. Once the mass of the known solid is measured‚ the percentage of chloride analyte can be calculated using stoichiometry. The chemical reaction occurring in this particular experiment involved the mixing of silver nitrate and the soluble salt in water containing nitric acid. Both reactants break into their ionic components allowing the silver ion and chloride ion
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