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Use the Maxwell distribution to calculate the average value of v2for the molecules of an ideal gas. Check that your answer agrees with equation 6.41.

Short Answer

Expert verified

The required average value is 3kTmand it matches with the given equation.

Step by step solution

01

Step1. Given information

The Maxwell speed distribution function is give by

Dv=m2Ï€kT324Ï€v2e-mv22kT................................(1)

02

Step 2. Calculation

The formula to calculate the average of v2is given by

v2=∫0∞v2Dvdv....................(2)

Substitute the distribution function from equation (1) into equation (2) to calculate the required average value.

v2=∫0∞v2m2πkT324πv2e-mv22kTdv=4πm2πkT32∫0∞v4e-mv22kTdv................(3)

Substitute xfor m2kTvinto equation (3) and evaluate the required value.

role="math" localid="1647007293675" v2=4πm2πkT322kTm52∫0∞x4e-x2dx=4πm2πkT322kTm523π8=3kTm

The rms speed is defined as

vrms=v2...................(4)

Substitute 3kTmfor v2into equation (4) to obtain the rms speed.

vrms=3kTm

Thus, the above equation exactly matches with equation 6.41.

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Most popular questions from this chapter

Some advances textbooks define entropy by the formula

S=-k∑sPslnPs

where the sum runs over all microstates accessible to the system and Psis the probability of the system being in microstate s.

(a) For an isolated system, role="math" localid="1647056883940" Ps=1Ωfor all accessible states s. Show that in this case the preceding formula reduces to our familiar definition of entropy.

(b) For a system in thermal equilibrium with a reservoir at temperatureT,role="math" localid="1647057328146" Ps=e-EskTZ. Show that in this case as well, the preceding formula agrees with what we already know about entropy.

Use Boltzmann factors to derive the exponential formula for the density of an isothermal atmosphere, already derived in Problems 1.16 and 3.37. (Hint: Let the system be a single air molecule, let s1 be a state with the molecule at sea level, and let s2 be a state with the molecule at height z.)

Carefully plot the Maxwell speed distribution for nitrogen molecules at T=300K and atT=600K. Plot both graphs on the same axes, and label the axes with numbers.

A particle near earth's surface traveling faster than about 11km/shas enough kinetic energy to completely escape from the earth, despite earth's gravitational pull. Molecules in the upper atmosphere that are moving faster than this will therefore escape if they do not suffer any collisions on the way out.

(a) The temperature of earth's upper atmosphere is actually quite high, around 1000K.Calculate the probability of a nitrogen molecule at this temperature moving faster than 11km/s, and comment on the result.

(b) Repeat the calculation for a hydrogen molecule (H2)and for a helium atom, and discuss the implications.

(c) Escape speed from the moon's surface is only about 2.4km/s. Explain why the moon has no atmosphere.

This problem concerns a collection of N identical harmonic oscillators (perhaps an Einstein solid or the internal vibrations of gas molecules) at temperature T. As in Section 2.2, the allowed energies of each oscillator are 0, hf, 2hf, and so on. (

a) Prove by long division that

11-x=1+x+x2+x3+⋯

For what values of x does this series have a finite sum?

(b) Evaluate the partition function for a single harmonic oscillator. Use the result of part (a) to simplify your answer as much as possible.

(c) Use formula 6.25 to find an expression for the average energy of a single oscillator at temperature T. Simplify your answer as much as possible.

(d) What is the total energy of the system of N oscillators at temperature T? Your result should agree with what you found in Problem 3.25.

(e) If you haven't already done so in Problem 3.25, compute the heat capacity of this system and check t hat it has the expected limits as T→0 and T→∞.

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