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Chapter 19: Q26P (page 578)

Question: What is the average translational kinetic energy of nitrogen molecules at 1600 K?

Short Answer

Expert verified

Answer

The average translational kinetic energy of nitrogen moleculesis3.31脳10-20J.

Step by step solution

01

Given data  

The temperature of the nitrogen gas molecules is 1600 K.

02

Understanding the concept

The expression for the average kinetic energy is given by,

Kavg=32KT

Here K is the Boltzmann constant, T is the temperature, Kavg is the average kinetic energy.

The value of k is equal to the1.38脳10-23鈥�J/molecule鈥�路K .

03

Calculate the average translational kinetic energy

Using the expression of the kinetic average energy,

Kavg=32KT

Substitute 1.38脳10-23鈥�J/molecule鈥�路Kfor k , 1600 k for T into the above equation,

Kavg=32脳1.38脳10-23脳1600Kavg=3.31脳10-20J

Therefore the average translational kinetic energy of nitrogen moleculesis3.31脳10-20J.

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Most popular questions from this chapter

The temperature of3.00鈥�molof a gas withCv=6.00鈥�cal/mol.K is to be raised50.0鈥�K . If the process is at constant volume, what are (a) the energy transferred as heat Q, (b) the work W done by the gas, (c) the change螖贰int in internal energy of the gas, and (d) the change螖碍 in the total translational kinetic energy? If the process is at constant pressure, what are (e) Q, (f) W, (g) 螖贰int, and (h) 螖碍? If the process is adiabatic, what are (i) Q, (j) W, (k)螖贰int , and (l)螖碍?

The temperature of 2.00of an ideal monatomic gas is raised 15.0鈥�Kin an adiabatic process. What are

(a) the work W done by the gas,

(b) the energy transferred as heat Q,

(c) the change螖贰int in internal energy of the gas, and

(d) the change螖碍in the average kinetic energy per atom?

Suppose 4.00 molof an ideal diatomic gas, with molecular rotation but not oscillation, experienced a temperature increase of 60.0Kunder constant pressure conditions. What are

  1. The energy transferred as heat Q .
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  3. The work W done by the gas.
  4. The change 螖Kin total translational kinetic energy of the gas?

Question: Water bottle in a hot car. In the American southwest, the temperature in a closed car parked in sunlight during the summer can be high enough to burn flesh. Suppose a bottle of water at a refrigerator temperature of 75 0C. Neglecting the thermal expansion of water and the bottle, find the pressure in the air pocket trapped in the bottle. (The pressure can be enough to push the bottle cap past the threads that are intended to keep the bottle closed.)

We give70鈥�Jas heat to a diatomic gas, which then expands at constant pressure. The gas molecules rotate but do not oscillate. By how much does the internal energy of the gas increase?
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