Questions in Kinetic Theory of Gases

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	If an ideal gas has volume V at 27°C and it is heated at a constant pressure so that its volume becomes 1.5V. Then the value of final temperature will be
	The temperature of an ideal gas at atmospheric pressure is $300K$ and volume $1m^3$. If temperature and volume become double, then pressure will be
	What is the mass of 2 litres of nitrogen at 22.4 atmospheric pressure and 273K
	The value of $PV/T$ for one mole of an ideal gas is nearly equal to
	A tyre kept outside in sunlight bursts off after sometime because of
	If the volume of the gas containing n number of molecules is $V$, then the pressure will decrease due to force of intermolecular attraction in the proportion
	In Boyle's law what remains constant
	Equation of gas in terms of pressure ($P$), absolute temperature ($T$) and density ($d$) is
	At constant pressure, the ratio of increase in volume of an ideal gas per degree raise in Kelvin temperature to its original volume is ($T$ = absolute temperature of the gas)
	Figure shows two flasks connected to each other. The volume of the flask 1 is twice that of flask 2. The system is filled with an ideal gas at temperature 100 K and 200 K respectively. If the mass of the gas in 1 be $m$ then what is the mass of the gas in flask 2