This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Here are the solutions to the questions: 28. Which substance is the most soluble in water? Water is a polar solvent that forms hydrogen bonds. Substances that can form hydrogen bonds with water or are highly polar will be more soluble. • CH_4 and C_2H_6 are nonpolar hydrocarbons and are not soluble in water. • CH_3OH (methanol) and C_2H_5OH (ethanol) are alcohols, both capable of forming hydrogen bonds with water due to their -OH groups. • Solubility of alcohols in water decreases as the nonpolar hydrocarbon chain length increases. Methanol (CH_3OH) has a shorter nonpolar chain (one carbon) than ethanol (C_2H_5OH) (two carbons). Therefore, methanol is more soluble. The correct option is A. 29. State the intermolecular forces that exist between molecules of each of the following: a) dry ice, CO_2(s) Carbon dioxide is a linear, nonpolar molecule. Intermolecular forces: London dispersion forces b) NH_3(l) Ammonia is a polar molecule with N-H bonds, and nitrogen has a lone pair. Intermolecular forces: Hydrogen bonding, dipole-dipole forces, London dispersion forces c) N_2(l) Nitrogen gas is a diatomic, nonpolar molecule. Intermolecular forces: London dispersion forces d) CH_3OCH_3 Dimethyl ether is a polar molecule due to the bent structure around the oxygen and polar C-O bonds, but it lacks an H atom bonded to O, N, or F. Intermolecular forces: Dipole-dipole forces, London dispersion forces 30. Which of each pair has the lower boiling point? Lower boiling points correspond to weaker intermolecular forces. a) C_2H_6 and C_3H_8 Both are nonpolar hydrocarbons with only London dispersion forces. C_2H_6 has a smaller molecular mass and fewer electrons than C_3H_8, leading to weaker London dispersion forces. Lower boiling point: C_2H_6 b) H_2O and H_2S H_2O forms strong hydrogen bonds. H_2S is polar but does not form hydrogen bonds. The intermolecular forces in H_2S (dipole-dipole and London dispersion forces) are weaker than the hydrogen bonds in H_2O. Lower boiling point: H_2S c) Cl_2 and Br_2 Both are nonpolar diatomic halogens with only London dispersion forces. Cl_2 has a smaller molecular mass and fewer electrons than Br_2, leading to weaker London dispersion forces. Lower boiling point: Cl_2 d) HF and HCl HF forms strong hydrogen bonds. HCl is polar but does not form hydrogen bonds. The intermolecular forces in HCl (dipole-dipole and London dispersion forces) are weaker than the hydrogen bonds in HF. Lower boiling point: HCl That's 2 down. 3 left today — send the next one.