Comparison and Explanation Melting point: Magnesium chloride and oxalic acid Boiling point: Acetic acid (Ethanoic acid) and n-Hexane Solubility in water: Sodium hydroxide and Chlorine gas (Cl2)
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A: This Question is based upon IR Spectroscopy.
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- A. DIRECTION: Define the following and give an example of each:1. Dispersion force2. Dipole-dipole attraction3. Hydrogen bond B. DIRECTION: Open the PhET States of Matter Simulation to answerthe following questions: Link: https://phet.colorado.edu/en/simulation/states-of-matter 1. Select the Solid, Liquid, Gas tab. Explore by selecting differentsubstances, heating and cooling the systems, and changing thestate. What similarities do you notice between the foursubstances for each phase (solid, liquid, gas)? What differencesdo you notice? 2. For each substance, select each of the states and record the giventemperatures. How do the given temperatures for each statecorrelate with the strengths of their intermolecular attractions?Explain.Compounds 1 and 2 have the same molecular weight. Identify and discuss all intermolecular forces for each molecule and clearly explain in terms of intermolecular forces why one of the compounds has a higher boiling point than the other. In your writing be sure to indicate which boiling point (3 °C and 25 °C) belongs to which compound. Please be sure to write in clear, well-written sentences that clearly illustrate your understanding and correctly uses appropriate terminology.Which type/s of intermolecular forces will be exhibited by a pure sample of PH3? Justify your answer
- Use the normal boiling pointspropane 1C3H82 -42.1 °Cbutane 1C4H102 -0.5 °Cpentane 1C5H122 36.1 °Chexane 1C6H142 68.7 °Cheptane 1C7H162 98.4 °Cto estimate the normal boiling point of octane 1C8H182.Explain the trend in the boiling points.Which of the following statements is/are true? a. Mixing acetone and ethanol resulted in an increase in volume despite adding equal volumes of each liquid because of H-bonding. b. Combining methanol and acetone involves the release of energy in order to overcome H-bonding, thus resulting in a decrease in volume. c. Methanol and ethanol can interact through dipole-dipole and LDF; thus, they will result in no change in volume. d. Due to the favorable compatibility of methanol and water via dipole-dipole and H-bonding, the mixture decreases in volume producing an endothermic process.Phys chem unit 4 . part 1 Kindly properly answer this? thank you so much :) 1. Based on the phase diagram of water explain the principle involve in each of the following:A. pressure cookingB. vacuum distillationC. vacuum fryingD. why it takes longer to cook food at high altitudes
- All compounds in a chemical series have the same commonality of structure, therefore the same predominant IMF. Using concepts of intermolecular forces, please explain thetrends of decreasing ΔTwith increasing molar mass within a chemical series.Rank the following in order of decreasingsurface tension ata given temperature, and explain your ranking:(a) CH₃OH(b) CH₃CH₃(c) H₂C=O1. Explanation of properties of solids, liquids and gas by using the kinetic molecular model. 2. Differences of Intermolecular forces (London Dispersion Forces, dipole-dipole Forces, Ion-Dipole Forces, and Hydrogen Bond) 3. In medical industry, Medical devices use adhesives as one example of application of Intermolecular Forces of Attraction. Adhesives are used extensively in th medical world, from simple plasters to advanced medical applications. Adhesives are integral to the production of paper tissues and nappies, allow tablets to be protected from the effects of moisture and allow wounds to be dressed. Trans dermal patches, such as nicotine patch, permit a controlled delivery of nicotine into the bloodstream to help smokers quit. What are other line of work that applies the Intermolecular forces of Attraction. At least one example and its use in the certain field of work. 4. Prediction of the type of Intermolecular forces that will be formed with the same kind of (a-c) and…
- Which intermolecular force(s) would you predict are present in a pure liquid sample of the molecule shown below? Select all that apply. -London Dispersion Interaction -Ion-dipole Interaction -H-bonding -Dipole-Dipole InteractionBelow are molecules with the same molecular formula () but different chemical structures. Identify which molecule/s (if any), can engage in hydrogen bonding. Assign each molecule to its normal boiling point, if one molecule has a normal boiling point of 97.2ºC and the other has 10.8ºC. Support your answer with valid concepts and reasoning between propanol and ethyl methyl etherA)What physical properties should you consider in comparing the strength of intermolecular forces in solids and in liquids---How would you measure stregnth of these forces? B) Arrange the following in order of increasing boiling point. Remember the stronger the intermolecular forces the higher the boiling point: RbF, CO2, CH3OH, CH3Br, methylamine,CH2F2. Explain your reasoning Remember O, N, and F for H-bonding.