$A$ $3.7 \ g$ sample of a gas occupies the same volume at $25 \ ^\circ C$ as $0.184 \ g$ of $H_2$ gas at $17 \ ^\circ C$ at the same pressure. The molecular weight of the gas is:

The following $P$ vs $V$ curve is plotted. What is the relation between $T_1$,$T_2$ and $T_3$?

For an ideal gas,the number of moles per litre in terms of its pressure $P$,gas constant $R$,and temperature $T$ is:

The mass of a gas in a container at $1 \, \text{atm}$ pressure and $200 \, K$ temperature is $3.2 \, g$. What will be the mass of the same gas in the same container at $500 \, K$ temperature and $10 \, \text{atm}$ pressure?

$A$ gas obeys Charles's law in the temperature range $0-500 \ K$ at a given pressure. Its volume changes to zero at a temperature of:

$A$ steel cylinder contains helium gas at $250 \, kPa$ pressure and $300 \, K$ temperature. The cylinder can withstand a maximum pressure of $1 \times 10^6 \, Pa$. The room in which the cylinder is placed catches fire. Predict whether the cylinder will burst before it melts. (Melting point of the cylinder = $1800 \, K$)