When an ideal gas undergoes unrestrained expansion,no cooling occurs because the molecules

$A$ student forgot to add the reaction mixture to the round bottomed flask at $27^{\circ} C$ but instead he/she placed the flask on the flame. After a lapse of time,he realized his mistake,and using a pyrometer he found the temperature of the flask was $477^{\circ} C$. What fraction of air would have been expelled out?

When $2 \ g$ of a gaseous substance $A$ is introduced into an initially evacuated flask at $25^{\circ} C$,the pressure is found to be $1 \ atm$. $3 \ g$ of another gaseous substance $B$ is added to it at the same temperature and pressure. The final pressure is found to be $1.5 \ atm$. Assuming ideal gas behaviour,the ratio of molar masses of $A$ and $B$ is:

If $P$,$V$,$M$,$T$ and $R$ are pressure,volume,molar mass,temperature and gas constant respectively,then for an ideal gas,the density is given by

$A$ car tyre is filled with nitrogen gas at $35 \ psi$ at $27^{\circ} C$. It will burst if pressure exceeds $40 \ psi$. The temperature in $^{\circ} C$ at which the car tyre will burst is ............ (Rounded-off to the nearest integer)

Which of the following equations represents the ideal gas equation?