Kinetic Theory ...

The molecules of a given mass of gas have rms velocity $$200\ ms^{-1}$$ at $$27^{\circ}C$$ and $$10^5\ Nm^{-2}$$ pressure. When the absolute temperature is doubled and the pressure is halved, the rms speed of the molecules of the same gas is:

In a thermodynamic system, working substance is ideal gas, its internal energy is in the form of  

For gas, if the ratio of specific heats at constants pressure $$P$$ and constant volume $$V$$ is $$\gamma $$, then the value of degree of freedom is:

The speed of a longitudinal wave in a mixture containing 4 moles of He and 1 mole of Ne at 300 K will be

The internal energy of an ideal gas increases during an isothermal process when the gas is 

One-gram mole of nitrogen occupies $$ 2 \times 10^4 $$ cc at a pressure of $$ 10^6  dynes/cm^2 $$. The average energy of a nitrogen molecule (in erg) will be:$$ (Avogadro's number = 6 \times 10^25 ) $$

In a process the pressure of gas is inversely proportional to the square of volume If temperature of the gas is increased then work done by the gas

In a thermodynamic system, working substance is ideal gas, its internal energy is in the form of

$$T_1$$ is the temperature of oxygen enclosed in a cylinder. The temperature is increased to $$T_2$$ and Maxwellan distribution curves for $$O_2$$ at temperature $$T_1$$ and $$T_2$$ are plotted. If $$A_1$$ and $$A_2$$ are the areas under the curves and the speed axis, in both cases , then 

 The total kinetic energy of $$8$$ litres of helium molecules at $$5$$ atmosphere pressure will be
($$1$$ atmosphere = $${ 1.013\times 10 }^{ 5 }$$pascal)