$A$ syringe has a volume of $10.0 \text{ cm}^3$ at a pressure of $1 \text{ atm}$. If the end is sealed and the plunger is pushed down at a constant temperature, what will be the final volume when the pressure becomes $3.5 \text{ atm}$ (in $\text{ cm}^3$)?

The pressure exerted by a non-reactive gaseous mixture of $6.4 \ g$ of methane and $8.8 \ g$ of carbon dioxide in a $10 \ L$ vessel at $27^{\circ} C$ is .............$kPa$.
(Round off to the Nearest Integer).
[Assume gases are ideal,$R = 8.314 \ J \ mol^{-1} K^{-1}$
Atomic masses $: C = 12.0 \ u, H = 1.0 \ u, O = 16.0 \ u]$

Calculate the volume in liters for $7 \ g$ of $O_2$ gas at $27 \ ^\circ C$ and $750 \ mm$ of $Hg$ pressure.

$A$ sealed flask with a capacity of $2 \, dm^{3}$ contains $11 \, g$ of propane gas. The flask is so weak that it will burst if the pressure becomes $2 \, MPa$. The minimum temperature at which the flask will burst is $....... \, ^{\circ}C$. [Nearest integer] (Given: $R = 8.3 \, J \, K^{-1} \, mol^{-1}$. Atomic masses of $C$ and $H$ are $12 \, u$ and $1 \, u$ respectively.) (Assume that propane behaves as an ideal gas.)

What is the value of the ratio of density $(d)$ to molar mass $(M)$ for an ideal gas?

An air bag on adiabatic expansion undergoes $5 \%$ increase in its volume. The percentage change in pressure is $\left[\gamma_{air}=1.4\right]$ (in $\%$)