Solid State Test

Result

Solid State Test - 6

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Weekly Quiz Competition

Question 1
1 / -0

The SI unit of pressure is Pascal (Pa) or Nm^-1. The atmospheric pressure at the sea level in SI units is

A
1 Pa

B
10^-5 Pa

C
1.01325 X 10⁵ Pa

D
1.01325 X 10^-5 Pa

Solution

Atmospheric pressure at the sea level = 1 atm = 1.01325 X 10⁵ Pa
Question 2
1 / -0

Which of the following postulate of the kinetic theory of gases is a faulty assumption about the gaseous behaviour and is not true under all conditions of temperature and pressure?

A
Gases consist of particles in constant, random motion and while moving the gas molecules collide against each other and against the walls of the container.

B
Gas pressure is due to the molecules colliding against the walls of the container and these collisions are perfectly elastic.

C
The average kinetic energy of a gas is directly proportional to the temperature of the gas on the Kelvin scale.

D
Particles are point masses with no volume and the volume of the individual gas molecules is negligible as compared to the volume of the entire gas.

Solution

The Kinetic theory of gases is based on two faulty assumptions about the gases that there exist no mutual forces of attraction between the gas molecules and the volume of the individual molecules is negligible as compared to the volume of the gas.
These assumptions become true only when the pressure is very low and the temperature is very high and the gases display ideal behaviour.
Under ordinary conditions of temperature and pressure, the volume of the individual gas molecules as well as the inter-particle attractions cannot be ignored.
Question 3
1 / -0

The translational kinetic energy of an ideal gas depends only on:

A. Molecular mass of the gas
B. Temperature on the absolute scale
C. Product of pressure and volume

A
Both 'A' and 'B'

B
Both 'B' and 'C'

C
All 'A', 'B' and 'C'

D
'A' only

Solution

In ideal gases, there exist no inter-particle interaction. Therefore, only the kinetic energy contributes to the internal energy of the gas.
Kinetic energy = 3/2 RT ( for 1 mole of a gas)
Kinetic energy = 3/2 kT (for one molecule of a gas)
where K = Boltzman constant and T is the absolute temperature.
It can also be expressed as:
K.E = 3/2 PV
However, one must remember that PV is constant at a constant temperature (Boyle's Law)
Hence both the expressions 'B' and 'C' imply that Kinetic energy of a gas is a function of its temperature on the absolute scale.