The vapors of $1 \ g$ of an element occupy $2.5625 \ L$ exerting a pressure of $0.5 \ atm$ at $1000 \ K$. What is the molar mass (in $g \ mol^{-1}$) of the element? (Assume vapors follow ideal gas equation. Given $R=0.082 \ L \ atm \ mol^{-1} \ K^{-1}$)

An ideal gas $(X)$ present in a vessel of volume $V \ L$ exerted a pressure of $16.4 \ atm$ at $200 \ K$. What is its concentration in $mol \ L^{-1}$? (Given $R=0.082 \ L \ atm \ mol^{-1} \ K^{-1}$)

$4 \ g$ of an ideal gas $A$ (molar mass $= M_A$) present in a vessel of a volume $V \ L$ exerted a pressure of $5 \ atm$ at $300 \ K$. When $16 \ g$ of another ideal gas $B$ (molar mass $= M_B$) was introduced into this vessel at the same temperature, the pressure increased to $10 \ atm$. What is the correct relationship between $M_A$ and $M_B$?

$A$ container is filled with nitrogen gas at a certain temperature and pressure. The mass of the gas is $0.6 \ g$. Now,the container is filled with another gas at the same temperature and pressure. If the mass of the second gas under the given conditions is $0.73 \ g$,identify the gas.

If the pressure and absolute temperature of $2 \ L$ of $CO_2$ are doubled,the volume of $CO_2$ would become ............... $L$.

Starting out on a trip into the mountains,you inflate the tires on your automobile to a recommended pressure of $3.21 \times 10^5 \ Pa$ on a day when the temperature is $-5.0 \ ^\circ C$. You drive to the beach,where the temperature is $28 \ ^\circ C$. Assume that the volume increased by $3 \%$. What is the final pressure in the tires?