/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 49 Which of the following affects t... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 11: Problem 49

Which of the following affects the vapor pressure of a liquid? (a) Volume of the liquid, (b) surface area, (c) intermolecular attractive forces, (d) temperature, (e) density of the liquid.

Short Answer

Expert verified
The factors that affect the vapor pressure of a liquid are (c) intermolecular attractive forces and (d) temperature. Stronger intermolecular forces result in lower vapor pressure, while weaker intermolecular forces lead to higher vapor pressure. Additionally, the vapor pressure increases as temperature increases. The volume of the liquid, surface area, and density do not directly affect the vapor pressure.

Step by step solution

01

Option (a): Volume of the liquid

The volume of the liquid does not affect its vapor pressure. Vapor pressure depends on the equilibrium between the liquid and vapor phases, which is determined by intermolecular forces and temperature, irrespective of the volume of the liquid.
02

Option (b): Surface area

The surface area of a liquid does not directly affect its vapor pressure. However, surface area may influence the rate of evaporation of the liquid. But since vapor pressure is a property of the liquid-vapor equilibrium, it does not depend on the surface area.
03

Option (c): Intermolecular attractive forces

Intermolecular attractive forces play a crucial role in determining the vapor pressure of a liquid. Stronger intermolecular forces make it more difficult for the molecules to escape the liquid and enter the vapor phase, resulting in lower vapor pressure. On the contrary, weaker intermolecular forces lead to higher vapor pressure.
04

Option (d): Temperature

Temperature affects the vapor pressure of a liquid. As temperature increases, the kinetic energy of the liquid molecules increases, making it easier for them to escape into the vapor phase. Consequently, the vapor pressure of the liquid increases with increasing temperature.
05

Option (e): Density of the liquid

The density of the liquid does not directly affect its vapor pressure. However, it may be indirectly related to vapor pressure, as liquids with higher densities often have stronger intermolecular forces. But the density itself does not influence the vapor pressure.
06

Final Answer

Based on our analysis, the factors that affect the vapor pressure of a liquid are (c) intermolecular attractive forces and (d) temperature.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Understanding Intermolecular Forces
Intermolecular forces are the invisible glue that holds the molecules of a liquid together. These forces affect how tightly or loosely the molecules are packed. There are different kinds of intermolecular forces, including hydrogen bonds, dipole-dipole interactions, and dispersion forces, each having its own strength and characteristics.
  • **Hydrogen bonds** are the strongest among these forces. They occur when hydrogen is bonded to electronegative atoms like oxygen or nitrogen.
  • **Dipole-dipole interactions** happen in molecules that have a permanent electric dipole. These are generally weaker than hydrogen bonds but stronger than dispersion forces.
  • **Dispersion forces** are the weakest and occur in all molecules, mainly influencing non-polar substances.
The strength of these intermolecular forces significantly influences a liquid's vapor pressure. When intermolecular forces are strong, molecules find it harder to escape into the vapor phase, resulting in a lower vapor pressure. Conversely, weaker forces allow molecules to easily move into the vapor phase, increasing vapor pressure.
Temperature Effects on Vapor Pressure
Temperature is a driving force that plays a pivotal role in vapor pressure. When you heat a liquid, its molecules gain kinetic energy. With more energy, molecules move around more and eventually find it easier to break free into the vapor phase. This increase in movement with rising temperature leads to higher vapor pressure.
  • Every liquid has a unique vapor pressure curve, where temperature and vapor pressure are directly related. Higher temperature equals higher vapor pressure.
  • At a certain temperature, known as the boiling point, vapor pressure equals atmospheric pressure, causing the liquid to boil.
This principle is crucial for understanding phenomena like boiling and evaporation. Thermometers, pressure cookers, and even some cooking techniques rely heavily on the interplay between temperature and vapor pressure.
Liquid-Vapor Equilibrium Explained
Liquid-vapor equilibrium occurs when the rate of evaporation of a liquid equals the rate of condensation. In this balanced state, the vapor pressure remains constant. This equilibrium does not depend on how much liquid is present or the container's size. Rather, it is influenced by the nature of the liquid and external conditions.
  • The equilibrium is dynamic, meaning that although the rates are equal, molecules constantly move between the liquid and vapor phases.
  • Factors influencing liquid-vapor equilibrium include temperature and intermolecular forces, both crucial in determining the vapor pressure.
Understanding liquid-vapor equilibrium helps explain why certain liquid behaviors, such as evaporation and boiling, occur. It's a foundational concept in physical chemistry, vital for fields like chemical engineering, meteorology, and environmental science.

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Describe how a cholesteric liquid crystal phase differs from a nematic phase.

If 42.0 \(\mathrm{kJ}\) of heat is added to a \(32.0-\mathrm{g}\) sample of liquid methane under 1 \(\mathrm{atm}\) of pressure at a temperature of \(-170^{\circ} \mathrm{C}\) , what are the final state and temperature of the methane once the system equilibrates? Assume no heat is lost to the surroundings. The normal boiling point of methane is \(-161.5^{\circ} \mathrm{C}\) The specific heats of liquid and gaseous methane are 3.48 and \(2.22 \mathrm{J} / \mathrm{g}-\mathrm{K}\) , respectively. [ Section 11.4\(]\)

(a) When you exercise vigorously, you sweat. How does this help your body cool? (b) A flask of water is connected to a vacuum pump. A few moments after the pump is turned on, the water begins to boil. After a few minutes, the water begins to freeze. Explain why these processes occur.

Liquid butane \(\left(\mathrm{C}_{4} \mathrm{H}_{10}\right)\) is stored in cylinders to be used as a fuel. The normal boiling point of butane is listed as \(-0.5^{\circ} \mathrm{C}\) . (a) Suppose the tank is standing in the sun and reaches a temperature of \(35^{\circ} \mathrm{C}\) . Would you expect the pressure in the tank to be greater or less than atmospheric pressure? How does the pressure within the tank depend on how much liquid butane is in it? (b) Suppose the valve to the tank is opened and a few liters of butane are allowed to escape rapidly. What do you expect would happen to the temperature of the remaining liquid butane in the tank? Explain. (c) How much heat must be added to vaporize 250 \(\mathrm{g}\) of butane if its heat of vaporization is 21.3 \(\mathrm{kJ} / \mathrm{mol}\) ? What volume does this much butane occupy at 755 torr and \(35^{\circ} \mathrm{C} ?\)

The smectic liquid crystalline phase can be said to be more highly ordered than the nematic phase. In what sense is this true?
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Kinetics

Read Explanation

Inorganic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Analysis

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.