Molecules of a gas are in incessant random motion colliding against one another and with the walls of the container.
BThe gas is not isotropic and the constant $(1/3)$ in equation $P = (1/3)\rho v^2_{rms}$ is result of this property
C
The time during which a collision lasts is negligible compared to the time of free path between collisions.
D
There is no force of interaction between molecules among themselves or between molecules and the wall except during collision.
Medium
Download our app for free and get started
BThe gas is not isotropic and the constant $(1/3)$ in equation $P = (1/3)\rho v^2_{rms}$ is result of this property
b $B)$ incorrect Isotropic property says that the various properties of a material are independent of direction hence the constant $\left(\frac{1}{3}\right)$ is the result of the assumption that the velocity of molecule is same in all three axis $x, y, z$
Download our app
and get started for free
Experience the future of education. Simply download our apps or reach out to us for more information. Let's shape the future of learning together!No signup needed.*
A horizontal uniform glass tube of $100 \,cm$, length sealed at both ends contain $10 \,cm$ mercury column in the middle. The temperature and pressure of air on either side of mercury column are respectively $81°C$ and $76\, cm$ of mercury. If the air column at one end is kept at $0°C$ and the other end at $273°C$, the pressure of air which is at $0°C$ is (in $cm$ of $Hg$)
When a gas filled in a closed vessel is heated by raising the temperature by $1^{\circ} C$, its pressure increase by $0.4 \%$. The initial temperature of the gas is ..........$K$
This question has Statement $- 1$ and Statement $-2$. Of the four choices given after the Statements, choose the one that best describes the two Statements.
Statement $1$ : The internal energy of a perfect gas is entirely kinetic and depends only on absolute temperature of the gas and not on its pressure or volume.
Statement $2$ : A perfect gas is heated keeping pressure constant and later at constant volume. For the same amount of heat the temperature of the gas at constant pressure is lower than that at constant volume.
Consider two ideal diatomic gases $\mathrm{A}$ and $\mathrm{B}$ at some temperature $T$. Molecules of the gas $A$ are rigid, and have a mass $m$. Molecules of the gas $\mathrm{B}$ have an additional vibrational mode, and have a mass $\frac{\mathrm{m}}{4} .$ The ratio of the specific heats $(\mathrm{C}_{\mathrm{v}}^{\mathrm{A}}$ and $\mathrm{C}_{\mathrm{v}}^{\mathrm{B}})$ of gas $\mathrm{A}$ and $\mathrm{B}$, respectively is
An ideal gas with adiabatic exponent $(\gamma=1.5)$ undergoes a process in which work done by the gas is same as increase in internal energy of the gas. The molar heat capacity of gas for the process is -
Two moles of an ideal gas with $\frac{\mathrm{C}_{\mathrm{P}}}{\mathrm{C}_{\mathrm{V}}}=\frac{5}{3}$ are mixed with $3$ moles of another ideal gas with $\frac{\mathrm{C}_{\mathrm{P}}}{\mathrm{C}_{\mathrm{V}}}=\frac{4}{3} .$ The value of $\frac{\mathrm{C}_{\mathrm{P}}}{\mathrm{C}_{\mathrm{V}}}$ for the mixture is