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Chapter 11: Problem 28

Why does the viscosity of a liquid decrease with increasing temperature?

Short Answer

Expert verified
The viscosity of a liquid decreases with increasing temperature due to increased kinetic energy of the particles, which reduces their interaction and thus the liquid's resistance to flow (viscosity).

Step by step solution

01

Understanding Viscosity

Viscosity can be thought of as a measure of a fluid's resistance to flow. The higher the viscosity, the thicker (or more resistive to flow) the fluid is.
02

Effect of Temperature on Liquids' Particles

Let's consider a certain liquid. As we increase the temperature, the kinetic energy of the particles of the liquid also increases. This increased energy allows the particles to move more freely.
03

Explain the Relation between Temperature and Viscosity

Given the increased kinetic energy from step 2, the interaction between the particles decreases. As a result, the liquid's resistance to flow, i.e. its viscosity, decreases. Thus, as temperature increases, viscosity decreases.
04

Concluding Statement

In essence, the reason why the viscosity of a liquid decreases with increasing temperature is because higher temperature implies higher kinetic energy for the particles. This increased movement reduces inter-particle interaction, decreasing the liquid's resistance to flow.

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Key Concepts

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

Fluid Resistance to Flow
The idea of fluid resistance to flow is commonly known as viscosity. It's a fundamental property that describes how a fluid behaves when it is in motion. Viscosity is the measure of the internal friction that occurs when one layer of fluid is made to move over another layer.

Picture honey and water - honey has a higher viscosity than water because it resists flow more, appearing thicker. In everyday life, this concept is important when considering substances like motor oil, which must maintain its ability to lubricate engine parts even at high temperatures where its viscosity would naturally decrease.
Kinetic Energy of Particles
When we talk about the kinetic energy of particles, we're referring to the energy that particles have due to their motion. The temperature of a substance is a direct measure of the average kinetic energy of its particles. The more heat we provide, the more energy these particles possess, leading to greater motion.

In a fluid, this translates to faster movement and more collisions among particles. As temperature goes up, particles move more vigorously, playing a crucial role in how the fluid flows.
Inter-Particle Interaction
The inter-particle interaction is about the forces acting between particles within a substance. These can be attractive or repulsive forces, and they significantly influence the physical properties of the material, including its viscosity.

Imagine a crowd in a room. When everyone is calm (cool conditions), they tend to stay closer, which is like higher viscosity. When the room heats up (increased temperature), people start to move away from each other to get comfortable, analogous to decreased inter-particle forces and, therefore, lower viscosity.
Effects of Heat on Liquids
Exploring the effects of heat on liquids reveals that as we increase a liquid's temperature, we're essentially providing energy to the system. This added energy disrupts the forces that hold the liquid together.

When heat is applied, it weakens the intermolecular forces that bind the particles, making it easier for them to slide over each other. Consequently, the higher the temperature, the lower the viscosity, enabling the liquid to flow more effortlessly. Therefore, heating a liquid changes its fluid dynamics by changing its internal interaction forces.

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Most popular questions from this chapter

Calculate the \(\Delta H^{\circ}\) for the following processes at \(25^{\circ} \mathrm{C}\) (a) \(\mathrm{Br}_{2}(l) \longrightarrow \mathrm{Br}_{2}(g)\) and (b) \(\mathrm{Br}_{2}(g) \longrightarrow\) \(2 \mathrm{Br}(g) .\) Comment on the relative magnitudes of these \(\Delta H^{\circ}\) values in terms of the forces involved in each case. \\{Hint: See Table \(9.4,\) and given that \(\left.\Delta H_{\mathrm{f}}^{\circ}\left[\mathrm{Br}_{2}(g)\right]=30.7 \mathrm{~kJ} / \mathrm{mol} .\right\\}\)

What kind of attractive forces must be overcome in order to (a) melt ice, (b) boil molecular bromine, (c) melt solid iodine, and (d) dissociate \(\mathrm{F}_{2}\) into F atoms?

Under the same conditions of temperature and density, which of the following gases would you expect to behave less ideally: \(\mathrm{CH}_{4}, \mathrm{SO}_{2} ?\) Explain.

Which of the following statements are false? (a) Dipole-dipole interactions between molecules are greatest if the molecules possess only temporary dipole moments. (b) All compounds containing hydrogen atoms can participate in hydrogen-bond formation. (c) Dispersion forces exist between all atoms, molecules, and ions. (d) The extent of ioninduced dipole interaction depends only on the charge on the ion.

The following compounds, listed with their boiling points, are liquid at \(-10^{\circ} \mathrm{C}:\) butane, \(-0.5^{\circ} \mathrm{C} ;\) ethanol, \(78.3^{\circ} \mathrm{C} ;\) toluene, \(110.6^{\circ} \mathrm{C}\). At \(-10^{\circ} \mathrm{C},\) which of these liquids would you expect to have the highest vapor pressure? Which the lowest? Explain.
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