At $NTP$,$10 \ g$ of a gas occupies $5 \ L$ of volume. At what temperature will the volume become double for the same mass of gas at the same pressure?

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)

$A$ plot of volume $(V)$ of the gas versus temperature ($T$ in $K$) is shown below. Which of the following options is correct for the plot?

What will be the volume in $L$ of $2.8 \ g$ of carbon monoxide at $27 \ ^oC$ temperature and $0.821 \ atm$ pressure? $(R = 0.0821 \ L \ atm \ mol^{-1} K^{-1})$

What is the ideal gas equation? Derive the equation for an ideal gas and describe the characteristics of $R$ and its value.

At $0\, ^\circ C$ and $1\, atm$ pressure,a gas occupies $100\, cc$. If the pressure is increased to $1.5$-times and temperature is increased by one-third of its absolute temperature,then the final volume of the gas will be .............. $cc$.