chemicals‚ like sulphur dioxide (SO2)‚ acid gases‚ and air toxics‚ from the flue gas (which is the smoke from the fire of a boiler which is made up of mainly carbon dioxide‚ carbon monoxide‚ and nitrogen). The sorbent that they normally use is limestone (CaCO3). When the limestone is crushed into a powder‚ they then mixed it with water(H2O) and spray it into the gases from burning coal. This solution then captures the toxic sulphur gases (SO2) and pulls them out and all that is left is a dry powder. This
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cm3 of solution? 6. What is the molarity of 15.0 g of CuSO4.5H2O in 250 cm3 of solution? 7. What volume of a 0.833 moldm-3 solution of H2O2 will be required to make 250 cm3 of a 0.100 moldm-3 solution? 8. What volume of a 0.50 moldm-3 solution of HCl will be required to make 100 cm3 of a 0.050M solution? 9. How many moles of NaCl are there in 25 cm3 of a 50 gdm-3 solution? Reacting masses and volumes 1. 25 cm3 of a solution of 0.1 moldm-3 NaOH reacts with 50 cm3 of a solution of hydrochloric
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Lab #5 Chemical Reactions & Balancing Equations Objectives Observe and classify several chemical and physical changes. Give evidence for the occurrence of a chemical reaction. Write a balanced equation for a chemical reaction. Identify a reaction as a combination‚ decomposition‚ replacement‚ or combustion reaction. Background Physical properties can be observed without changing the chemical composition of the substance. Common physical properties that can be measured without changing the chemical
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constant. P1/T1 = P2/T2 5. What is the Ideal Gas Law in formula form? What is the value for the proportionality constant with units? Why are those units so important? b. PV = nRT c. C = PV / T 6. Write the balanced equations for CaCO3‚ BaCO3‚ Li2CO3‚ and Na2CO3 reactions with hydrochloric acid. 7. Calculate the molar mass of these same four metallic
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dissolved in the solvent. In this experiment we also used a chemical method known as extraction. This process of separation is used when only one component of the mixture is soluble in a specific solvent. In our case we had to use hydrochloric acid (HCl).Extractions‚ is a way to separate a desired substance when it is mixed with others. The mixture is brought into contact with a solvent in which the substance of interest is soluble‚ but the other substances present are insoluble. And below is a
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of calcium carbonate in egg shells reacts with an excess of hydrochloric acid so that it is sure that a reaction is occurring. The excess HCl is then diluted because of the egg shell with a drop of phenolphthalein added and is then titrated in aliquots with sodium hydroxide solution. This is the reaction for determining the excess of HCl: 2HCl (aq) + CaCO3(s) -→ Ca2+ (aq) + CO2(g) + H2O(l) + 2Cl- (aq) Materials: eggshell burette‚ 50 cm³‚ and stand pipette + filler‚ 20 cm³ plastic foil
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Unknown 2 Scheme “ Fair game” ions Cations: Na+‚ K+‚ NH4+ ‚ Ca2+‚ Mg(OH2)62+ ‚ Al(OH2)63+ Anions: SO42-‚ HSO4-‚ NO3-‚ OH-‚ Cl-‚ CO32-‚ HCO3- Insoluble Compounds: Ca(OH)2‚ CaSO4•2H2O‚ CaCO3‚ MgCO3‚ Mg(OH)2 I. Describe Sample a. Quick description of sample. Ex: Phase‚ color‚ odor‚ crystalline‚ amorphous‚ gel-like‚ powdery‚ etc. II. Flame Test a. Part 1 i. Orange Flame: Na+ is present. K+ ‚ NH4+ ‚ Ca2+‚ Mg(OH2)62 ‚ Al(OH2)63+ may also be present. ii. Purple Flame: K+ is present (no Na+
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Vicente Viloria CHM 130 LL Section 22258 Lab 12: Introduction to pH‚ Household Products and Buffers 12/9/14 Introduction In this experiment the students will be determining the pH of household products along with other solutions using several different indicators as well as a pH meter. The experiment also has the student determining what the buffer solution is in an aqueous solution. The student will also be testing the pH of milk of magnesia and will see how it affects the stomach acid. Lastly
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Chem 17 ▪ General Chemistry Laboratory II Experiment 1 Calorimetry INTRODUCTION Chemical reactions are usually accompanied by the evolution (exothermic reaction) or absorption (endothermic reaction) of heat energy. When measured at constant pressure‚ the heat evolved (qp < 0) or absorbed (qp > 0) is equal to the enthalpy change‚ symbolized by ΔH. ΔH is positive for an endothermic process and negative for an exothermic one. If H f is the enthalpy of the final state and Hi of the initial state
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tell you about their electronic structures? (2) 3 When calcium carbonate is heated it decomposes. The equation for this reaction is: CaCO3 → CaO + CO2 a Use numbers from the list to complete the sentences. 2 3 4 5 6 i The number of products in the equation is ....... (1) ii The formula CaCO3 shows that calcium carbonate was made from ....... different elements. iii The equation is balanced because there are ....... atoms on both sides
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