At $300 \ K$ temperature,the pressure and volume of a gas are $1 \ bar$ and $10 \ L$ respectively. If the pressure becomes $2 \ bar$,calculate the volume of the gas at the same temperature. (in $L$)

The following data is obtained for $1 \ mole$ of a gas. The gas behaves as an ideal gas in the pressure range (in $bar$):

$P \ (bar)$	$\frac{PV}{RT}$
$1$	$1$
$2$	$1$
$3$	$1$
$4$	$1.5$
$5$	$2.0$

At $27\, ^\circ C$ temperature and $1\, bar$ pressure,the volume of a gas is $25\, L$. If the temperature becomes $77\, ^\circ C$ at constant pressure,calculate the volume of the gas. (in $, L$)

Two separate bulbs contain ideal gases $A$ and $B$. The density of gas $A$ is $4$ times that of gas $B$. The molecular mass of $A$ is half that of gas $B$. The two gases are at the same temperature. The ratio of the pressure of $A$ to that of gas $B$ is

$4 \ g$ of an ideal gas occupies $5.6035 \ L$ of volume at $546 \ K$ and $2 \ atm$ pressure. What is its molecular weight?

$A$ $10 \, L$ cylinder contains $0.4 \, g$ of helium,$1.6 \, g$ of oxygen,and $1.4 \, g$ of nitrogen at $27 \, ^\circ C$. Calculate the total pressure of the mixture and the partial pressure of helium gas. Assume ideal gas behavior. $(R = 0.082 \, L \, atm \, K^{-1} \, mol^{-1})$