Kinetic Theory

The energy associated with random motion of molecules is called:

1. Internal energy
2. Potential energy
3. Mechanical energy
4. Electrical energy

The pressure of a gas increases when:

1. Temperature decreases
2. Molecular collisions increase
3. Number of molecules decreases
4. Volume increases

At absolute zero temperature, the kinetic energy of molecules is theoretically:

1. Maximum
2. Minimum
3. Infinite
4. Constant

The kinetic energy of one mole of an ideal gas is:

1. 1/2 RT
2. 3/2 RT
3. RT
4. 2RT

The average speed of gas molecules increases when:

1. Temperature decreases
2. Temperature increases
3. Volume increases only
4. Pressure decreases only

The degrees of freedom of a monoatomic gas molecule are:

1. 1
2. 2
3. 3
4. 6

The pressure of an ideal gas is inversely proportional to volume when temperature remains constant. This is:

1. Charles' law
2. Boyle's law
3. Avogadro's law
4. Newton's law

The value of Boltzmann constant is approximately:

1. 1.38 × 10⁻²³ J/K
2. 6.02 × 10²³ J/K
3. 8.31 J/mol K
4. 9.8 m/s²

The root mean square speed of gas molecules is proportional to:

1. √T
2. T
3. 1/T
4. T²

An ideal gas is one in which:

1. Molecules have strong attraction
2. Molecules occupy large volume
3. Intermolecular forces are negligible
4. Molecules do not move

The SI unit of temperature used in kinetic theory is:

1. Celsius
2. Fahrenheit
3. Kelvin
4. Joule

The average kinetic energy of gas molecules is directly proportional to:

1. Pressure
2. Volume
3. Absolute temperature
4. Density

According to kinetic theory, the pressure exerted by a gas is due to:

1. Weight of molecules
2. Collision of molecules with container walls
3. Attraction between molecules
4. Size of molecules

The kinetic theory of gases assumes that gas molecules are:

1. At rest
2. In continuous random motion
3. Fixed at their positions
4. Without mass