At $300 \ K$ temperature,the pressure and volume of a gas are $1 \ bar$ and $10 \ L$ respectively. If the pressure becomes $2 \ bar$,calculate the volume of the gas at the same temperature. (in $L$)

An $LPG$ cylinder contains gas at a pressure of $300 \ kPa$ at $27^{\circ} C$. The cylinder can withstand a pressure of $1.2 \times 10^{6} \ Pa$. The room in which the cylinder is kept catches fire. The minimum temperature at which the bursting of the cylinder will take place is $.....^{\circ} C$. (Nearest integer)

$V_0$ and $V_t$ are the volumes of a fixed mass of an ideal gas at $0^\circ \text{C}$ and $t^\circ \text{C}$ respectively at constant pressure. Find the ratio $V_t / V_0$.

The density of $O_{2(g)}$ is maximum at?

At $400\, K$ temperature,the volume and pressure of a gas are $200\, mL$ and $1.5\, bar$ respectively. Calculate the volume,weight (assuming the gas is $N_2$),and the number of molecules at $STP$. $[R = 8.31 \times 10^{-2}\, L\, bar\, K^{-1}\, mol^{-1}]$.

For a fixed amount of gas at constant pressure,provide the plot of volume $(V)$ versus temperature $(T)$ in Kelvin. What does it represent?