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Chapter 10: Problem 133

Which of the following statements is (are) true? a. LiF will have a higher vapor pressure at \(25^{\circ} \mathrm{C}\) than \(\mathrm{H}_{2} \mathrm{S}\) . b. HF will have a lower vapor pressure at \(-50^{\circ} \mathrm{C}\) than \(\mathrm{HBr}\) . c. \(\mathrm{Cl}_{2}\) will have a higher boiling point than Ar. d. HCl is more soluble in water than in \(\mathrm{CCl}_{4}\) e. \(\mathrm{MgO}\) will have a higher vapor pressure at \(25^{\circ} \mathrm{C}\) than \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) .

Short Answer

Expert verified
The true statements are: b. HF will have a lower vapor pressure at \(-50^{\circ} \mathrm{C}\) than HBr. c. Cl2 will have a higher boiling point than Ar. d. HCl is more soluble in water than in CCl4.

Step by step solution

01

Statement A: LiF will have a higher vapor pressure at 25°C than H2S

This statement is false. LiF is an ionic compound, while H2S is a covalent compound. Ionic compounds generally have lower vapor pressures than covalent compounds because the ionic bonds are stronger and prevent the molecules from vaporizing easily. In contrast, H2S has weaker covalent bonds and will have a higher vapor pressure than LiF.
02

Statement B: HF will have a lower vapor pressure at -50°C than HBr

This statement is true. HF has a higher boiling point than HBr because of the presence of hydrogen bonding. Hydrogen bonding is a stronger intermolecular force compared to the dipole-dipole interaction present in HBr. Due to the stronger intermolecular forces, HF has a lower vapor pressure compared to HBr at the same temperature.
03

Statement C: Cl2 will have a higher boiling point than Ar

This statement is true. Cl2 and Ar are both nonpolar, so the main intermolecular force between them is London dispersion forces. Cl2 has a higher molecular weight compared to Ar. As molecular weight increases, the strength of London dispersion forces increases, leading to a higher boiling point. Therefore, Cl2 will have a higher boiling point than Ar.
04

Statement D: HCl is more soluble in water than in CCl4

This statement is true. The solubility of a substance depends on the polarity of the solvent. Water is a polar solvent, while CCl4 is a nonpolar solvent. HCl is a polar covalent compound, which means it will easily dissolve in polar solvents like water. As the saying goes, "like dissolves like." Hence, HCl will be more soluble in water than in CCl4.
05

Statement E: MgO will have a higher vapor pressure at 25°C than CH3CH2OH

This statement is false. MgO is an ionic compound, while CH3CH2OH (ethanol) is a covalent compound. As mentioned before, ionic compounds generally have lower vapor pressures than covalent compounds due to the strong ionic bonds. Ethanol, a covalent compound, has weaker intermolecular forces (hydrogen bonding and London dispersion forces) and will have a higher vapor pressure than MgO.

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Most popular questions from this chapter

What quantity of energy is needed to heat a 1.00 -mole sample of \(\mathrm{H}_{2} \mathrm{O}\) from \(-30.0^{\circ} \mathrm{C}\) to $140.0^{\circ} \mathrm{C} ?\( (see Exercise 101\))$

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