Imagine that you drop a brick on the ground and it lands with a thud. Apparently the energy of this system tends to spontaneously decrease. Explain why.

Short Answer

Expert verified

The energy is transferred from the brick to the ground, so the energy of the system tends to spontaneously decrease.

Step by step solution

01

Given information

A brick is dropped to the ground and it lands with a thud.

Energy of this system tends to spontaneously decrease,

02

Explanation

Helmholtz free energy can be determined by
F=U-T S
Where, F= Helmholtz free energy, U=Internal energy,T=absolute temperature of the system and S=entropy of the system.

The total energy of the brick = kinetic energy + potential energy

From the law of energy conservation this is always constant.

When the brick hits the ground, its kinetic energy is zero, but the potential energy remains the same. The kinetic energy is redistributed into the thermal energy of the molecules of the brick and to the ground where the brick hits.

So a part of the energy is transferred from the brick to the ground.

Therefore the energy of the system tends to spontaneously decrease.

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 Vaia!

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

Use a Maxwell relation from the previous problem and the third law of thermodynamics to prove that the thermal expansion coefficient β(defined in Problem 1.7) must be zero at T=0.

Assume that the air you exhale is at 35°C, with a relative humidity of 90%. This air immediately mixes with environmental air at 5°C and unknown relative humidity; during the mixing, a variety of intermediate temperatures and water vapour percentages temporarily occur. If you are able to "see your breath" due to the formation of cloud droplets during this mixing, what can you conclude about the relative humidity of your environment? (Refer to the vapour pressure graph drawn in Problem 5.42.)

Below 0.3 K the slope of the °He solid-liquid phase boundary is negative (see Figure 5.13).

(a) Which phase, solid or liquid, is more dense? Which phase has more entropy (per mole)? Explain your reasoning carefully.

(b) Use the third law of thermodynamics to argue that the slope of the phase boundary must go to zero at T = 0. (Note that the *He solid-liquid phase boundary is essentially horizontal below 1 K.)

(c) Suppose that you compress liquid *He adiabatically until it becomes a solid. If the temperature just before the phase change is 0.1 K, will the temperature after the phase change be higher or lower? Explain your reasoning carefully.

Because osmotic pressures can be quite large, you may wonder whether the approximation made in equation5.74is valid in practice: Is μ0really a linear function of Pto the required accuracy? Answer this question by discussing whether the derivative of this function changes significantly, over the relevant pressure range, in realistic examples.

μ0T,P2μ0T,P1+P2-P1μ0P......equation(5.74)

Derive the thermodynamic identity for G (equation 5.23), and from it the three partial derivative relations 5.24.

See all solutions

Recommended explanations on Physics Textbooks

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.

Sign-up for free