What is the use of Fisher-Johns apparatus, Gallenkamp apparatus, and automatic melting point apparatus in terms of melting point determination?
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What is the use of Fisher-Johns apparatus, Gallenkamp apparatus, and automatic melting point apparatus in terms of melting point determination? (Own words)
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- What is the reason for the stoke shift for a fluorophore ? Please shortly answer at your own words. Answer should be to the point(specific).3. The phase diagram for the simple system aluminum copper is drawnbelow. Answer the following questions by referring to this diagram.A. How many phases will be present if an aluminum-copper mixture containing 80% copper is heated to 1000oC?B. If the system described in (A) is slowly cooled, at what temperature willa solid start to appear? What is this solid?C. What phases will be present if the mixture (A) is further cooled down to600oC?D. What is the concentration of the saturated solution of copper inaluminum at 800oC?E. For a mixture given in (A), at what temperature will the eutectic mixturecrystallize out?F. What is the percentage by weight of copper in the eutectic mixture formed in (E)?In order to obtain accurate data it is important to add hear slowly and steadily when the temperature gets close to the melting point of a sample. Why is necessary?
- 1.) While determining the pressure during the Dumas experiment, if the barometric pressure reported were lower than the actual vapor pressure (Part I), how would this error affect the calculated molar mass of the unknown volatile liquid? Explain.What limitations are encountered in the apolication of sublimation as a general method of purification?7.58. Do communities that use salt in the winter use enough to form the low-melting eutectic betweenand , or are they taking advantage of the freezing-point depression phenomenon in general? How can you tell?
- A student obtained a solid product in laboratory synthesis. To verify the identity of the solid, she measured the milting point and found that the material melted over a 12°C range. After it had cooled, she measured the melting point of the same sample again and found that this time the solid HUD a sharp melting point at the temperature that is characteristic of the desired product Why were the two melting points different? What was responsible for the change in the melting point?1. To determine the melting point of aspirin, Gerald placed the sample in a capillary tube tied to a thermometer and heated them in an oil bath. Which constitute the system and the surroundings? a.system: aspirin, thermometer, oil, alcohol lamp; surroundings: Gerald b.system: aspirin; surroundings: thermometer, oil, alcohol lamp c.system: aspirin, thermometer, oil; surroundings: alcohol lamp d. system: aspirin, thermometer; surroundings: oil, alcohol lamp 2. Which of the following processes is exothermic, given the following: N2(g) + 2O2(g) → N2O4(l) ΔHo = 9.67 kJ mol-1N2(g) + 2O2(g) → 2NO2(g) ΔHo = 67.70 kJ mol-1 a.2NO2(g) → N2O4(l) b.2N2(g) + 4O2(g) → 2N2O4(l) c.N2(g) + O2(g) → N2O4(l) +NO2(g) d.(1/2)N2(g) + O2(g) → NO2(g)Why does the experimentally observed van't Hoff factor frequently differ from the predicted value? answer choices: a. Varying degrees of residual ionic attractions prohibit the ions as acting as totally independent particles b. Compounds that completely dissociate have a van't Hoff factor twice of that predicted c. A complete lack of particle interaction results in a lowered experimental value d. A complete lack of particle interaction results in an increased experimental value e. Interference from nonelectrolytes lowers the experimental value
- Aromatic compound naphthalene melts sharply at 79–81 °C. The melting range will be significantly depressed when very small amounts of impurities are present. Investigate the structure of naphthalene and propose an explanation of why very minor impurities have a very significantly disrupt formation of crystals.Proposed a laboratory procedures on how to determine polymer molecular weight based on osmotic pressure and dilute solution viscosity measurements.Characterize the intermolecular forces in solutions made by the following phases.• Acetone/chloroform, (………………………………………………………)• Benzene/Acetone, (………………………………………………………)• Ethane/propane, (………………………………………………………)• Hexane/water.
