What Is the Average Kinetic Energy of a Nitrogen Molecule at 25°C?

In summary, the Kinetic Theory of Gases is a scientific model that explains the behavior and properties of gases based on the motion of their particles. It assumes that gases consist of small particles in constant, random motion, with negligible size and no attractive or repulsive forces between them. This theory also explains gas pressure as the result of collisions between gas particles and the walls of their container, and states that the average kinetic energy of gas particles is directly proportional to the temperature of the gas. Furthermore, the ideal gas law can be derived from the Kinetic Theory of Gases, as it describes the relationship between pressure, volume, temperature, and the number of gas particles.
  • #1
M9501
3
0

Homework Statement


The average kinetic energy of a nitrogen molecule at temperature 25c is _____ .

Select the correct answer.
1)5*10^(-21) J
2)3*10^(-20) J
3)1*10^(-20) J
4)9*10^(-20) J
5)8*10^(-21) J
(i guess they are all wrong )

Homework Equations


KE=3/2 K.T

The Attempt at a Solution



KE(av)=3/2 KT = 3/2 * 1.38*10^(-23) * (25+273)=6.1686*10^(-21) J

i just want to know whether my solution is correct or no ..
 
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  • #2
A nitrogen molecule is not a single atom. It can rotate...
 
  • #3
mfb said:
A nitrogen molecule is not a single atom. It can rotate...
got it thanks

K.E=5/2 KT
 

FAQ: What Is the Average Kinetic Energy of a Nitrogen Molecule at 25°C?

1. What is the Kinetic Theory of Gases?

The Kinetic Theory of Gases is a scientific model that explains the behavior and properties of gases based on the motion of their particles. It states that gases consist of a large number of small particles that are in constant, random motion, and that the average kinetic energy of these particles is directly proportional to the temperature of the gas.

2. What are the assumptions of the Kinetic Theory of Gases?

There are three main assumptions of the Kinetic Theory of Gases: 1) Gases are made up of particles that are in constant, random motion; 2) The size of the particles is negligible compared to the distance between them; and 3) The particles do not exert any attractive or repulsive forces on each other, except during collisions.

3. How does the Kinetic Theory of Gases explain gas pressure?

The Kinetic Theory of Gases explains gas pressure as the result of collisions between gas particles and the walls of their container. As the particles move and collide with the walls, they exert a force, which results in pressure. The more particles and collisions, the higher the pressure of the gas.

4. What is the relationship between temperature and kinetic energy in the Kinetic Theory of Gases?

The Kinetic Theory of Gases states that the average kinetic energy of gas particles is directly proportional to the temperature of the gas. This means that as the temperature increases, the particles move faster and have a higher kinetic energy, and vice versa.

5. How does the Kinetic Theory of Gases explain the ideal gas law?

The ideal gas law, PV = nRT, can be derived from the Kinetic Theory of Gases. It states that the pressure (P) of an ideal gas is directly proportional to the number of moles (n) of gas present, the temperature (T) in Kelvin, and inversely proportional to the volume (V) of the gas. This relationship is based on the motion and collisions of gas particles as described by the Kinetic Theory of Gases.

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