$A$ 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?

At $300 \, K$ constant temperature,a gas having $20 \, cm^3$ volume and $1 \, bar$ pressure is converted into $50 \, cm^3$. Calculate the final pressure. (in $, bar$)

The temperature at which real gases obey the ideal gas laws over a wide range of pressure is called:

An $LPG$ (Liquefied Petroleum Gas) cylinder weighs $15.0 \ kg$ when empty. When full,it weighs $30.0 \ kg$ and shows a pressure of $3.0 \ atm$. In the course of usage at $27^{\circ}C$,the mass of the full cylinder is reduced to $24.2 \ kg$. The volume of the used gas in cubic metre at the normal usage condition ($1 \ atm$ and $27^{\circ}C$) is (assume $LPG$ to be normal butane and it behaves ideally). (in $m^3$)

The volume-temperature graph of a given mass of an ideal gas at constant pressure is shown below. What is the correct order of pressures?

Which of the following is equal to $[{\partial P/\partial V}]_T$ for an ideal gas?