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- Explain why ethanol (CH3CH2OH) is more soluble in water than is ethane (CH3CH3 )Circle the compound in the following pairs corresponding to the physical properties. Write the intermolecular force directly under each compound (ID,DD,HB). a) Highest BP: CH3OH or CH3SH b) Highest heat of Vap: H20 or Cl2 c) Highest surface tension: CH3CH2CH2CH3 or CH3CH2CH2CH2CH2CH3 d) Highest BP: Si(CH3)4 or NF3 e) Highest vapor pressure: CH3NHCH3 or BCl3Which has a higher boiling point? Explain using london dispersion forces, dipole dipole, or hydrogen bonding. (a) CH3CH3 or CH3CH2OH (b) CH3CH2CH2CH2CH2CH2CH3 or (CH3)3C-CH(CH3)2
- Which of the following should have the highest boiling point A) CH3-CH2-F B) CH3-CH2-CH3 C) CH3-CH2-CH2-CH3 D) CH3-CH2-O-HWhich of the following best exhibits hydrogen bonding? Explain your answer. H2Se CH4 HCl NH33. Which compound is likely to have a higher boiling point? Whya. A polar compound without O-H or N-H bonds, or a polar compound with O-H or N-H bondsb. CH3CH2CH2OH or CH3(CH2)4OH4. Compare boiling points and solubilities in water for each pair of compounds. Explain a. Ammonia, NH3 and methane, CH4b. Pentanol, C5H11OH, and pentane, C5H12
- Why does ethanol have a higher boiling point than dimethyl ether despite having the same molecular weight? Because alcohols are polar molecules. Neither Because alcohols show hydrogen bonding. Both1. Rank the following with increasing acidity: CH3OH, HCl, NH3, and CH4 2. Select the correct molecule with the lowest surface tension. a. CH3CH2CH2OH b. CH3CH2CH2NH2 c. CH3CH2CH2CH3 d. CH3CH2CH2ClWhy does water have a higher boiling point and lower vapor pressure than comparably sized molecules such a s dimethyl ether (CH3-O-CH3) or N2
