At $25 \, ^oC$ and $730 \, mm$ pressure,$380 \, mL$ of dry oxygen gas is collected. If the temperature is kept constant,what will be the volume of oxygen gas at $760 \, mm$ pressure (in $, mL$)?

For an ideal gas obeying Boyle's Law,which of the following is correct? ($K$ is a constant)

$2 \ g$ of $O_2$ at $27 \ ^\circ C$ and $760 \ mm$ of $Hg$ pressure has volume ............. $L$.

For $1 \ mol$ of an ideal gas,an isochore is obtained. The slope of the isochore is $0.082 \ atm \ K^{-1}$. What will be its pressure (in $atm$) when the temperature is $12.2 \ K$? $(R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1})$.

$A$ 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:

$A$ $3.7 \ g$ 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: