Question:

An ideal gas of density $\rho=02 \,kg \, m ^{-3}$ enters a chimney of height $h$ at the rate of $\alpha=08 \,kg \,s ^{-1}$ from its lower end, and escapes through the upper end as shown in the figure The cross-sectional area of the lower end is $A_1=01 \, m ^2$ and the upper end is $A_2=04 \, m ^2$ The pressure and the temperature of the gas at the lower end are $600 \,Pa$ and $300 \,K$, respectively, while its temperature at the upper end is $150 \,K$ The chimney is heat insulated so that the gas undergoes adiabatic expansion Take $g=10 \,ms ^{-2}$ and the ratio of specific heats of the gas $\gamma=2$ Ignore atmospheric pressure Which of the following statement(s) is(are) correct?
ideal gas of density

Updated On: Jul 14, 2024
  • The pressure of the gas at the upper end of the chimney is $300\, Pa$.
  • The velocity of the gas at the lower end of the chimney is $40 \,ms ^{-1}$ and at the upper end is $20\, ms ^{-1}$.
  • The height of the chimney is $590 \,m$.
  • The density of the gas at the upper end is $0.05\, kg\, m ^{-3}$.
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The Correct Option is B

Solution and Explanation

An ideal gas of density
\(\frac{dm}{dt} = p_1 A_1 v_1 = 0.8 \, \text{kg/s} \, A\)
\(v_1 = \frac{0.8}{0.2 \times 0.1} = 40 \, \text{m/s}\)

g = 10 m/s2 
\(\gamma = 2\)

Gas undergoes adiabatic expansion,
\(p_1 - \gamma T^{\gamma} = \text{Constant}\)
\(\frac{P_2}{P_1}=(\frac{T_1}{T_2})^{\frac{r}{1-\gamma}}\)

\(P_2=\frac{600}{4}=150P_a\)

Now \(\rho∝\frac{P}{T}\)

\(\frac{\rho_1}{\rho_2}=(\frac{P_1}{P_2})(\frac{T_1}{T_2})\)

\((\frac{150}{600})(\frac{300}{150})=\frac{1}{2}\)

Now
\(P_1 A_1 \Delta x_1 - P_2 A_2 \Delta x_2 = 2 mV_1 - mV_2 + mgh_2 - mgh_1 + \frac{f}{2}(P_2 V_2 - P_1 V_1)\)

Simplifying we get.  \(\frac{V_2}{V_1} - \frac{V_1}{V_2} = \frac{2P}{gh} \frac{m}{m}\)
\(⇒\frac{2\times600}{0.2}-\frac{2\times150}{0.1}\)

\(=\frac{20^2-40^2}{2}+10h\)
\(h = 360 m\)

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Concepts Used:

Kinetic Molecular Theory of Gases

Postulates of Kinetic Theory of Gases:

  • Gases consist of particles in constant, random motion. They continue in a straight line until they collide with each other or the walls of their container. 
  • Particles are point masses with no volume. The particles are so small compared to the space between them, that we do not consider their size in ideal gases.
  • Gas pressure is due to the molecules colliding with the walls of the container. All of these collisions are perfectly elastic, meaning that there is no change in energy of either the particles or the wall upon collision.  No energy is lost or gained from collisions. The time it takes to collide is negligible compared with the time between collisions.
  • The kinetic energy of a gas is a measure of its Kelvin temperature. Individual gas molecules have different speeds, but the temperature and
    kinetic energy of the gas refer to the average of these speeds.
  • The average kinetic energy of a gas particle is directly proportional to the temperature. An increase in temperature increases the speed in which the gas molecules move.
  • All gases at a given temperature have the same average kinetic energy.
  • Lighter gas molecules move faster than heavier molecules.