At $740 \ torr$ pressure,the volume of $N_2$ gas is $800 \ mL$. If the volume becomes $540 \ mL$ at constant temperature,calculate the pressure of the gas. (in $torr$)

Explain: Gay-Lussac's Law.

Molecular attraction and size of the molecules in a gas are negligible at :-

$A$ $3.7 \ g$ mass of a gas occupies a certain volume at $25 \ ^\circ C$. The same volume is occupied by $0.184 \ g$ of $H_2$ gas at the same pressure and $17 \ ^\circ C$. Calculate the molar mass of the gas.

For an ideal gas,what is the nature of the $pV$ versus $p$ graph at a constant temperature?

For $1 \ mol$ of an ideal gas at a constant temperature $T,$ the plot of $(\log \ P)$ against $(\log \ V)$ is a ($P :$ Pressure,$V:$ Volume)