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Chapter 1: Problem 23

Which substance would have the highest vapor pressure? (A) Ethanol, because of the hybridization of its carbon atoms (B) Actone, because it exhibits the weakest intermolecular forces (C) Ethylene glycol, because it has the most lone pairs assigned to individual atoms (D) All three substances would have similar vapor pressure because they have a similar number of electrons.

Short Answer

Expert verified
The substance that would have the highest vapor pressure is Acetone because it exhibits the weakest intermolecular forces.

Step by step solution

01

Analyzing the Options

First, it's necessary to grasp the properties of each option. Ethanol and ethylene glycol can form hydrogen bonds because they have -OH groups. Acetone, however, has a carbonyl group and can only produce dipole-dipole interactions. Ethylene glycol, due to its two -OH groups, can form stronger intermolecular forces than ethanol. Thus, the strongest intermolecular forces are likely in ethylene glycol, then ethanol, and lastly acetone.
02

Relate Intermolecular Forces to Vapor Pressure

Next, one needs to understand how intermolecular forces relate to vapor pressure. The stronger the intermolecular forces, the lower the vapor pressure. This is because strong intermolecular forces hold the molecules together, making it difficult for molecules to escape to the vapor phase. Hence, among the substances given, acetone which exhibits the weakest intermolecular forces should have the highest vapor pressure.
03

Rule out Incorrect Answers

Finally, you can rule out the incorrect answers. The hybridization of carbon atoms in ethanol (A) or the number of lone pairs in ethylene glycol (C) are not directly related to vapor pressure. The number of electrons (D) also does not directly influence vapor pressure. Therefore, the only reasonable answer is (B), Acetone.

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Most popular questions from this chapter

1.50 g of \(\mathrm{NaNO}_{3}\) is dissolved into 25.0 \(\mathrm{mL}\) of water, causing the temperature to increase by \(2.2^{\circ} \mathrm{C}\) . The density of the final solution is found to be 1.02 \(\mathrm{g} / \mathrm{mL}\) . Which of the following expressions will correctly calculate the heat gained by the water as the NaNO, dissolves? Assume the volume of the solution remains unchanged. (A) \((25.0)(4.18)(2.2)\) (B) \(\frac{(26.5)(4.18)(2.2)}{1.02}\) (C) \(\frac{(1.02)(4.18)(2.2)}{1.50}\) (D) \((25.0)(1.02)(4.18)(2.2)\)

The following reaction is found to be at equilibrium at 25°C: \(2 \mathrm{SO}_{3}(g) \leftrightarrow \mathrm{O}_{2}(g)+2 \mathrm{SO}_{2}(g) \quad \Delta H=-198 \mathrm{kJ} / \mathrm{mol}\) What is the expression for the equilibrium constant, \(K_{\mathrm{c}} ?\) (A) \(\frac{\left[\mathrm{SO}_{3}\right]^{2}}{\left[\mathrm{O}_{2}\right]\left[\mathrm{SO}_{2}\right]^{2}}\) (B) \(\frac{2\left[\mathrm{SO}_{3}\right]}{\left[\mathrm{O}_{2}\right] 2\left[\mathrm{SO}_{2}\right]}\) (C) \(\frac{\left[\mathrm{O}_{2}\right]\left[\mathrm{SO}_{2}\right]^{2}}{\left[\mathrm{SO}_{3}\right]^{2}}\) (D) \(\frac{\left[\mathrm{O}_{2}\right] 2\left[\mathrm{SO}_{2}\right]}{2\left[\mathrm{SO}_{3}\right]}\)

$$2 \mathrm{NOCl} \rightarrow 2 \mathrm{NO}+\mathrm{Cl}_{2}$$ The reaction above takes place with all of the reactants and products in the gaseous phase. Which of the following is true of the relative rates of disappearance of the reactants and appearance of the products? (A) NO appears at twice the rate that NOCl disappears. (B) NO appears at the same rate that NOCl disappears. (C) NO appears at half the rate that NOCl disappears. (D) \(\mathrm{Cl}_{2}\) appears at the same rate that NOCl disappears.

A solution of \(\mathrm{Co}^{2+}\) ions appears red when viewed under white light. Which of the following statements is true about the solution? (A) A spectrophotometer set to the wavelength of red light would read a high absorbance. (B) If the solution is diluted, the amount of light reflected by the solution will decrease. (C) All light with a frequency that is lower than that of red light will be absorbed by it. (D) Electronic transmissions within the solution match the wavelength of red light.

Which of the following pairs of substances would make a good buffer solution? (A) \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)\) and \(\mathrm{NaC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)\) (B) \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)\) and \(\mathrm{LiOH}(a q)\) (C) \(\mathrm{HCl}(a q)\) and \(\mathrm{KCl}(a q)\) (D) \(\mathrm{HF}(a q)\) and \(\mathrm{NH}_{3}(a q)\)
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