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**1. A fresh air is composed of nitrogen N2(78%) and oxygen O2(21%). Find the rms speed of N2 and O2 at 20°C.**

**Solution:**

For Nitrogen,

Molar mass *m* = 0.0280 kg/mol

Temperature T = 20°C =
20 + 273 = 293K

**Ans: For vrms = 511 m s-1**

**For O2vrms = 478 m s-1**

** **

**2. If the rms speed of methane gas in the Jupiter’s atmosphere is 471.8 m s-1, show that the surface temperature of Jupiter is sub-zero.**

**Solution:**

RMS speed of methane
gas = 471.8 ms^{-1} =V_{rms}

Sub-zero temperature
Molar mass of methane gas

= 16.04 × 10-3 kg mol^{-1}

Surface temperature of
Jupiter T = ?

Gas constant R =8.31

**Ans: -130°C**

** **

**3. Calculate the temperature at which the rms velocity of a gas triples its value at S.T.P.**

**Ans: T1 = 273 K, T2 = 2457 K**

** **

**4. A gas is at temperature 80°C and pressure 5 × 10-10 N m-2. What is the number of molecules per m3 if Boltzmann’s constant is 1.38 × 10-23 J K-1**

**Solution:**

Temperature of gas T =
80°C = 80 + 273 = 353*K*

Pressure of gas P = 5 ×
10^{-10} Nm^{-2}

Boltzmann’s constant k
= 1.38 × 10^{-23} J*k*^{-1}

Volume of gas V = 1 m^{3}

No. of molecules *n* = ?

**Ans: 1.02 × 1011**

** **

**5. From kinetic theory of gases, show that Moon cannot have an atmosphere (Assume k = 1.38 × 10-23 J K-1 Temperature T=0°C=273K).**

**Ans: vescape = vrms= 1.86 km s-1**

** **

**6. If 1020 oxygen molecules per second strike 4 cm2 of wall at an angle of 30° with the normal when moving at a speed of 2 × 103 m s-1, find the pressure exerted on the wall. (mass of 1 atom = 1.67 × 10-27 kg)**

**Solution**

Mass of 1 O_{2}
atom = 2.67 × 10^{-26} kg

Mass of 10^{20}
O_{2} atom = 2.67 × 10^{-26} kg

= 26.72 × 10^{-27} × 10^{20}

Momentum P = *mv*

= 26.72 × 10^{-7}
× 8 × 2 × 10^{3}

= 427.5 × 10^{-4}
kgm s^{-1}

Component of momentum
normal to wall is 30°

= 427.5 ×10^{-4}
× cos 30° .

**Ans: 92.4 N m-2**

** **

**7. During an adiabatic process, the pressure of a mixture of monatomic and diatomic gases is found to be proportional to the cube of the temperature. Find the value of γ = ( Cp/CV)**

**Solution**

**Ans: 3/2**

** **

**8. Calculate the mean free path of air molecules at STP. The diameter of N2 and O2 is about 3 × 10-10 m**

*Solution*

**Ans: λ≈9 × 10-8 m**

** **

**9. A gas made of a mixture of 2 moles of oxygen and 4 moles of argon at temperature T. Calculate the energy of the gas in terms of RT. Neglect the vibrational modes.**

**Ans: 11RT**

** **

**10. Estimate the total number of air molecules in a room of capacity 25 m3 at a temperature of 27°C.**

**Solution:**

Volume of the room V =
25.0m^{3}

Temperature of the room
T = 27°C = 300K

Pressure in the room P
= estimate

= 1 × 1.013 × 10^{5}
Pa

The ideal gas equation
relating pressure (P), volume (v) absolute temperature (T) can be written is

PV = K_{B} NT

**Ans: 6.1 × 1026 molecules**

A football at 27°C has 0.5 mole of air molecules. Calculate the internal energy of air in the ball.

The internal energy of ideal gas = 3/2 *NkT*. The number of air molecules is given in terms of number of moles so, rewrite the expression as follows

Temperature T =273+27=300K

U = 3/2 × 0.5 × 8.31 × 300 = 1869.75J

This is approximately equivalent to the kinetic energy of a man of 57 kg running with a speed of 8 m s-1.

A room contains oxygen and hydrogen molecules in the ratio 3:1. The temperature of the room is 27°C. The molar mass of 02 is 32 g mol-1 and for *H*2 2 g mol-1. The value of gas constant R is 8.32 J mol-1K-1

(a) rms speed of oxygen and hydrogen molecule

(b) Average kinetic energy per oxygen molecule and per hydrogen molecule

(c) Ratio of average kinetic energy of oxygen molecules and hydrogen molecules

(a) Absolute Temperature

T=27°C =27+273=300 K.

Gas constant R=8.32 J mol-1k-1

For Oxygen molecule: Molar mass

M=32 gm=32 x 10-3 kg mol-1

Note that the rms speed is inversely proportional to √M and the molar mass of oxygen is 16 times higher than molar mass of hydrogen. It implies that the rms speed of hydrogen is 4 times greater than rms speed of oxygen at the same temperature.

1934/484 ≈ 4 .

(b) The average kinetic energy per molecule is 3/2 kT. It depends only on absolute temperature of the gas and is independent of the nature of molecules. Since both the gas molecules are at the same temperature, they have the same average kinetic energy per molecule. *k* is Boltzmaan constant.

(c) Average kinetic energy of total oxygen molecules = 3/2 N0*k*T where N0 - number of oxygen molecules in the room

Average kinetic energy of total hydrogen molecules = 3/2 NHkT where NH - number of hydrogen molecules in the room.

It is given that the number of oxygen molecules is 3 times more than number of hydrogen molecules in the room. So the ratio of average kinetic energy of oxygen molecules with average kinetic energy of hydrogen molecules is 3:1

Ten particles are moving at the speed of 2, 3, 4, 5, 5, 5, 6, 6, 7 and 9 m s-1. Calculate rms speed, average speed and most probable speed.

The average speed

The most probable speed is 5 ms-1 because three of the particles have that speed.

Calculate the rms speed, average speed and the most probable speed of 1 mole of hydrogen molecules at 300 K. Neglect the mass of electron.

The hydrogen atom has one proton and one electron. The mass of electron is negligible compared to the mass of proton.

Mass of one proton = 1.67 × 10−27*kg*.

One hydrogen molecule = 2 hydrogen atoms = 2 × 1.67 × 10−27*kg*.

The average speed

Find the adiabatic exponent γ for mixture of μ 1 moles of monoatomic gas and μ2 moles of a diatomic gas at normal temperature.

An oxygen molecule is travelling in air at 300 K and 1 atm, and the diameter of oxygen molecule is 1.2 × 10−10*m*. Calculate the mean free path of oxygen molecule.

We have to find the number density *n* By using ideal gas law

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