Describe how fractional distillation can better purify a mixture of liquids by discussing a liquid vapor phase diagram. Draw a liquid vapor phase diagram and use this in your answer.
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Describe how fractional distillation can better purify a mixture of liquids by discussing a liquid vapor phase diagram. Draw a liquid vapor phase diagram and use this in your answer.
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- Heating a solid until it passes directly from the solid phase into the gaseous phase. Separating a liquid from an insoluble solid sediment by carefully pouring the liquid from the solid without disturbing the solid. The process of vapor returning to the solid phase without a liquid phase in between. Heating a mixture to vaporize a volatile liquid component to make the remaining component dry. Separating a solid from a liquid using a porous material, such as paper, charcoal, or sand, as a filter. Using a solvent to selectively dissolve one or more components from a solid mixture. Answer Bank extraction filtration decantation deposition sublimation evaporationDue to the fact that the liquid you used was a volatile one, it will not completely recondense. Some of the liquid remains in the vapor phase, even at room temperature. If you were able to correct for this by making the vapors recondense completely, would your final molar mass value be greater than, less than or the same as the value you determined? Explain your reasoning.3. A student is trying to identify an unknown solid based on its melting point. She noted that the compound began to melt at 172°C and finished melting at 177°C. Knowing it is possible for there to be impurities in the sample, is this compound more likely to be camphor or hydroquinone. Explain your reasoning. 4. A young chemist has synthesized what he believed to be acetaminophen. He measured the melting point of this newly formed compound to be 163-178°C. If the literature value for the melting point of acetaminophen = 169-170.5°C, would the young chemist be wise to consume this product for headache relief? Why or why not?
- 2. a) How could you calculate a water pressure above a 1M NaCl solution (salt in water)? Could you explain what the meaning of your formula? What would be the boiling temperature of such solution at a normal external pressure? b) How could you separate components by distillation? Explain on a phase diagram.Miscible liquids form a homogeneous mixture when added together. Is toluene miscible with water? With ethyl alcohol?Chapter 11 Predicting relative boiling point elevations and freezing point depressions Four liquids are described in the table below. Use the second column of the table to explain the order of their freezing points, and the third column to explain the order of their boiling points. For example, select '1' in the second column next to the liquid with the lowest freezing point. Select '2' in the second column ne point the liquid with the next higher freezing point, and so on. In the third column, select '1' next to the liquid with the lowest boiling point, '2' next to the liquid with the next higher boiling point, and so on. Note: the density of water is 1.00 g/mL. solution 2.9 g of potassium chloride (KCI) dissolved in 300. mL of water 2.9 g of ethylene glycol (C₂H6O₂) dissolved in 300. mL of water 2.9 g of sucrose (C12H₂2O11) dissolved in 300. mL of water 300. mL of pure water alculating molality Michael nyamkimal freezing point boiling point 4 3 2 2 3 tudent dissolves 8.8 g of…
- What would be a Prerequisite Skill or Prior Knowledge that a 5th grade science class should know about Volcano Eruptions before using the below standard? Standard Conduct an investigation to determine whether the mixing of two or more substances results in new substances.2. Why does the temperature of a mixture of ice and water remain constant during melting and freezing?Why is it not advisable to freeze a sealed glass bottle that is completely filled with water? Use both macroscopic and microscopic models to explain your answer. Is a similar consideration required for a bottle containing pure ethanol? Why or why not?
- Aspirin has a higher molar mass compared to salicylic acid, however aspirin melts at a lower temperature than salicylic acid. Provide a brief explanation for this observation. Table 1 Compound: Formula: Salicylic Acid C;H6O3 Aspirin C9H3O4 Molar Mass: 138.12 Melting point: Ka 158-160°C 1.08 x 10³ 180.15 140-142°C 2.72 x 10$ pKa Solubility (g/100ML) 2.99 4.57 0.18 0.25Alcohol and kerosene create a layer of suspension when poured in the same bottle explain the observation at a molecular levelWhen potassium sulfite dissolves in water, the sulfite ion SO2−3 acts as a base. Write a balanced equation for the reaction of the sulfite ion with water. Express your answer as a chemical equation. Identify all of the phases in your answer.
