$A$ gas cylinder contains cooking gas at $14.9 \ atm$ pressure. The pressure gauge of the cylinder reads $12 \ atm$ at $27 \ ^oC$. If the cylinder bursts due to a sudden fire in the building,at what temperature in $^oC$ will the cylinder burst?

An ideal gas expands against a constant external pressure of $3 \ atm$ from $4 \ dm^3$ to $6 \ dm^3$. The work done during this process is ..... $J$.

Match the following graphs of an ideal gas with their respective axes ($X$ and $Y$).
$(A)$ $P$ vs $V$ (at constant $T$)
$(B)$ $V$ vs $T$ (at constant $P$)
$(C)$ $P$ vs $T$ (at constant $V$)
List-$I$:
$(1)$ $P$ on $Y$-axis,$T$ on $X$-axis
$(2)$ $P$ on $Y$-axis,$1/V$ on $X$-axis
$(3)$ $V$ on $Y$-axis,$T$ on $X$-axis

Volume occupied by a gas at $1 \, \text{atm}$ pressure and $0 \, ^\circ C$ is $V \, mL$. Its volume at $273 \, K$ will be

Keeping temperature constant,the pressure of $11.2 \ dm^3$ of a gas was increased from $105 \ kPa$ to $420 \ kPa$. What is the new volume of the gas (in $dm^3$)?

At $25 \, ^\circ C$ temperature and $760 \, mm \, Hg$ pressure,the volume of a gas is $600 \, mL$. Calculate the pressure when the volume of this gas becomes $640 \, mL$ at $10 \, ^\circ C$ temperature. Use the ideal gas equation: $\frac{p_1 V_1}{T_1} = \frac{p_2 V_2}{T_2}$