Embibe Experts Solutions for Chapter: Kinetic Theory of Gases, Exercise 1: Exercise-1

When the temperature of an ideal gas is increased from $27 °\mathrm{C}$ to $227 °\mathrm{C},$ its rms speed is changed from $400 \mathrm{m} {\mathrm{s}}^{-1}$ to $v_{\mathrm{s}}.$ The $v_{\mathrm{s}}$ is:

Hydrogen gas is filled in a container of volume $20 \mathrm{litre}$. Average translational kinetic energy of all its molecules is $1.5\times {10}^5 \mathrm{J}.$ Pressure of hydrogen in cylinder is:

Root mean square speed of ideal hydrogen gas in closed chamber at $0 °\mathrm{C}$ is $3180 \mathrm{m} {\mathrm{s}}^{-1}$. Its pressure will be (density of hydrogen gas is $8.99\times {10}^{-2} \mathrm{kg} {\mathrm{m}}^{-3}, 1 \mathrm{atm}=1.01\times {10}^5 \mathrm{N} {\mathrm{m}}^{-2}$)

A flask contains argon and chlorine in the ratio $3:1$ by mass. The temperature of the mixture is $300 \mathrm{K}.$ If atomic mass of argon $=39.9 \mathrm{u}$ and molecular mass of chlorine $=70.9 \mathrm{u},$ then the ratio of average kinetic energy per molecule of argon to chlorine gas is:

The internal energy of a mono-atomic gas is,

According to law of equal distribution of energy, the mean energy of a molecule per degree of freedom is:

In the following $V-T$ diagram what is the relation between $P_1$ and $P_2$

An electric fan is switched on in a closed room. The air in the room is___.