What kind of intermolecular forces act between a chloromethane (CH3C1) molecule and a hydrogen sulfide molecule? Note: If there is more than one type of intermolecular force that acts, be sure to list them all, with a comma between the name of each force.
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- What kind of intermolecular forces act between two chloromethane (CH₂C1) molecules? Note: If there is more than one type of intermolecular force that acts, be sure to list them all, with a comma between the name of each force. XWould you expect butanone, CH;COCH;CH3 where the CO is a double bond, to have a higher or lower boiling point than acetone? Explain your reasoning. Propanol, CH3CH2CH2OH, has a molar mass of 60.1 g/mol and a boiling point of 97.4°C. Use intermolecular forces to explain why propanol has a higher boiling point than butane or acetone.3. Consider the following table. List three substances as having the strongest intermolecular forces. Explain your reason. Formula CH4 HOH C₂H6 CH₂OH C3H8 CH₂CH₂OH C4H10 CH3CH₂CH₂OH Name methane water ethane methanol propane ethanol butane 1-propanol Molar Mass Boiling Point (°C) -164 100 -89 65 -42 78 16 18 30 32 44 46 58 60 97
- What are ALL the types of intermolecular bonding does n-pentane have? What are ALL the types of intermolecular bonding does 1-butane have?Why does styrene have a higher boiling point, 145 °C, than isopropanol, 83 °C? Based on the types and strength of intermolecular forces?Look up the formulas and correct Lewis structures for Pentane and Tetrachloromethane. Then explain the relative positions of the boiling points. 1000, Boiling Point 76.5/ 100 36.1/ Pentane Tetrachloro-/iWater/ methane 800 760 600 Atmospheric Pressure 400 200 20 40 60 80 100 Temperature (°C) Vapor pressure (mm Hg)
- 11 What type of organic molecule is this? ketone alcohol aldehyde organic acidEthanol and dimethyl ether have the same molecular formula C2H6O. Ethanol is liquid at room teperature while dimethyl ether is gas. How is this possible? Explain.What type(s) of intermolecular forces are expected between CH3CH₂NH2 molecules? H H tr N- H H H H H- Indicate with a Y (yes) or an N (no) which apply. dipole forces induced dipole (London dispersion) forces hydrogen bonding
- Consider the data in the table. Compound Melting point (°C) ????? (??/???)ΔHfus (kJ/mol) Boiling point (°C) ????? (??/???)ΔHvap (kJ/mol) HFHF −83.11 4.577 19.54 25.18 HClHCl −114.3 1.991 −84.9 17.53 HBrHBr −86.96 2.406 −67.0 19.27 HIHI −50.91 2.871 −35.38 21.16 Using the data in the table, calculate Δ?fus and Δ?vap for HF. Δ?fus= J/(K⋅mol) Δ?vap= J/(K⋅mol) Determine the entropy change when 8.70 mol HF(g) condenses at atmospheric pressure. Δ?= J/KHydrogen peroxide is a liquid at room temperature with a boiling point of 150°C, whereas ethyne is a gas at room temperature with a boiling point of -84°C. Draw the molecules. Based on intermolecular forces, explain this difference in physical properties of these compounds that have similar chemical formulas and molar masses.Consider the data in the table. Compound Melting point (°C) ????? (??/???)ΔHfus (kJ/mol) Boiling point (°C) ????? (??/???)ΔHvap (kJ/mol) HFHF −83.11 4.577 19.54 25.18 HClHCl −114.3 1.991 −84.9 17.53 HBrHBr −86.96 2.406 −67.0 19.27 HIHI −50.91 2.871 −35.38 21.16 Using the data in the table, calculate Δ?fusΔSfus and Δ?vapΔSvap for HF.HF. Δ?fus=ΔSfus= J/(K⋅mol)J/(K⋅mol) Δ?vap=ΔSvap= J/(K⋅mol)J/(K⋅mol) Determine the entropy change when 7.60 mol HF(l)7.60 mol HF(l) boils at atmospheric pressure. Δ?=ΔS= J/K