At $300 \ K$ temperature and $1 \ atm$ pressure,the weight of $1 \ L$ of a gas is $2 \ g$. If the pressure is changed to $0.75 \ atm$,at what temperature in $K$ will the weight of $1 \ L$ of the same gas be $1 \ g$?

Two closed bulbs of equal volume $V$ containing an ideal gas initially at pressure $P_i$ and temperature $T_1$ are connected through a narrow tube of negligible volume as shown in the figure below. The temperature of one of the bulbs is then raised to $T_2$. The final pressure $P_f$ is:

At constant pressure,the volume of a gas is $300 \ mL$. If the temperature is changed from $27 \ ^oC$ to $-3 \ ^oC$,what will be the final volume in $mL$?

For a fixed amount of gas,the volume is $x \ L$ at a pressure of $y \ atm$ and a temperature of $z \ K$. At which of the following conditions will the volume remain $x \ L$? (Consider $y \neq z$)

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

For one mole of an ideal gas, the slope of $V$ vs. $T$ curve at a constant pressure of $2 \ atm$ is $X \ L \ mol^{-1} \ K^{-1}$. The value of the ideal universal gas constant '$R$' in terms of $X$ is