In order to increase the volume of a gas by $10 \%$ at constant temperature,the pressure of the gas should be:

$A$ 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)

$A$ sample of gas has a volume of $95 \, cm^3$ at a pressure of $9.962 \times 10^4 \, N m^{-2}$ and constant temperature. What will be its volume at $10.13 \times 10^4 \, N m^{-2}$ pressure at the same temperature (in $, cm^3$)?

Calculate the density of methane at $27\,^oC$ and $2.0\, atm$ pressure in $g\, L^{-1}$.

At a constant pressure $p$,the plot of volume $(V)$ as a function of temperature $(T)$ for $2 \, mol$ of an ideal gas gives a straight line with a slope $0.328 \, L \, K^{-1}$. The value of $p$ (in $atm$) is closest to
[Gas constant,$R=0.0821 \, L \, atm \, mol^{-1} \, K^{-1}$ ]

Three bulbs are filled with $CH_4$,$CO_2$,and $Ne$ as shown in the picture. The bulbs are connected through pipes of zero volume. When the stopcocks are opened and the temperature is kept constant throughout,the pressure of the system is found to be $...... \ atm$. (Nearest integer)