Pressure of $1 \ g$ ideal gas $X$ at $300 \ K$ is $2 \ atm$. When $2 \ g$ of another gas $Y$ is introduced in the same vessel at the same temperature,the total pressure becomes $3 \ atm$. The correct relationship between molar masses of $X$ and $Y$ is:

$A$ gas cylinder containing cooling gas can withstand a pressure of $14.9 \text{ atm}$. The pressure gauge of the cylinder indicates $12 \text{ atm}$ at $27 \,^oC$. Due to a sudden fire in the building,the temperature starts rising. The temperature at which the cylinder explodes is ............. $^oC$. (in $.5$)

$A$ certain mass of a gas occupies a volume of $2 \,L$ at $STP$. To what temperature must the gas be heated to double its volume, keeping the pressure constant?

What is the molar volume of a gas? What is its value taken as?

If a gas occupies $1 \, L$ volume at atmospheric pressure,what will be the volume of the same amount of gas at $750 \, mm \, Hg$ pressure at the same temperature?

What does the following graph represent?