K K Sharma Solutions for Chapter: Kinetic Theory, Exercise 1: TOPICWISE QUESTIONS

If RMS velocity of a gas is $v_{rms}$$=1840 \mathrm{m} {\mathrm{s}}^{-1}$ and its density $\rho =8.99\times {10}^{-2} \mathrm{kg} {\mathrm{m}}^3$, then the pressure of the gas will be 

If the RMS velocity of hydrogen becomes equal to the escape velocity from the Earth's surface, then the temperature of hydrogen gas would be

At temperature $T$, $N$ molecules of gas $A$ each having mass $m$ and at the same temperature $2N$ molecules of gas $B$ each having mass $2m$ are filled in a container. The mean square velocity of molecules of a gas $B$ is $v^2$ and $x$ component of mean square velocity of molecules of gas $A$ is $w^2$. The ratio of $\frac{w^2}{v^2}$ is,

The RMS velocity of gas molecules of a given amount of a gas at $27 \text{°C}$ and $1.0\times {10}^5 \mathrm{N} {\mathrm{m}}^{-2}$ pressure is $200 \mathrm{m} {\mathrm{s}}^{-1}$. If temperature and pressure are, respectively, $127 °\mathrm{C}$ and $0.5\times {10}^5 \mathrm{N} {\mathrm{m}}^{-2}$, then the RMS velocity will be,

Suppose a container is evacuated to leave just one molecule of a gas in it. Let $v_a$ and $v_{\mathrm{RMS}}$ represent the average speed and the RMS speed of the gas. Then 

The RMS speed of oxygen molecules in a gas is $v$. If the temperature is doubled and the ${\mathrm{O}}_2$ molecules dissociate into oxygen atoms, then the RMS speed will become

If the temperature of the gas is increased to three times, it's root mean square velocity becomes

Consider a mixture of oxygen and hydrogen kept at room temperature. As compared to a hydrogen molecule, an oxygen molecule hits the wall