Assuming ideal gas behaviour,the ratio of density of ammonia to that of hydrogen chloride at the same temperature and pressure is: (Atomic wt. of $Cl = 35.5 \ u$)

At constant pressure,the temperature of $20 \ L$ of helium gas is increased from $100 \ K$ to $300 \ K$. What will be the change in volume in $L$?

At very low pressure,the compressibility factor $Z$ of a $CO_2$ gas with constant molar volume is:

For an ideal gas,the value of ${\left( {\frac{{dU}}{{dV}}} \right)_T}$ is ...... .

$A$ gas has a volume of $3.4 \ L$ at $25^{\circ} C$. What is the final temperature if the volume increases to $10.2 \ L$ at constant pressure (in $K$)?

Assuming the molar mass of air is $28.84 \, g \, mol^{-1}$,calculate the payload (lifting capacity) of a balloon of volume $10^6 \, L$ filled with $He$ at $27 \, ^\circ C$ and $1 \, atm$ pressure.