At $27^{\circ} C$ in a $10 \ L$ flask,$4.0 \ g$ of an ideal gaseous mixture containing $He$ (molar mass $4.0 \ g \ mol^{-1}$) and $Ne$ (molar mass $20 \ g \ mol^{-1}$) has a pressure of $1.23 \ atm$. What is the mass $\%$ of neon? $(R = 0.082 \ L \ atm \ K^{-1} \ mol^{-1})$

Which of the following equations does $NOT$ represent Charles's law for a given mass of gas at constant pressure?

Calculate the volume of $6.022 \times 10^{21}$ molecules of $CO_2$ at $300 \ K$ temperature and $2 \ bar$ pressure. $[R = 8.314 \times 10^{-2} \ bar \ L \ K^{-1} \ mol^{-1}]$ (in $mL$)

$A$ 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?

$A$ monoatomic ideal gas,initially at temperature $T_1$,is enclosed in a cylinder fitted with a frictionless piston. The gas is allowed to expand adiabatically to a temperature $T_2$ by releasing the piston suddenly. $L_1$ and $L_2$ are the lengths of the gas columns before and after the expansion,respectively. The ratio $\frac{T_2}{T_1}$ is:

An open vessel at $300 \ K$ is heated until $2/5$ of the air in it is expelled. Assuming that the volume of the vessel remains constant,the temperature to which the vessel is heated is $..... \ K$.