$A$ $3.7 \ g$ sample of a gas occupies the same volume at $25 \ ^\circ C$ as $0.184 \ g$ of $H_2$ gas at $17 \ ^\circ C$ at the same pressure. The molecular weight of the gas is:

Match the following gas laws with their respective equations.

The initial volume of a gas cylinder is $750.0 \ mL$. If the pressure of gas inside the cylinder changes from $840.0 \ mm \ Hg$ to $360.0 \ mm \ Hg$,what will be the final volume of the gas (in $L$)?

If the density ratio of a gas is $1:2$ and the temperature ratio is $2:1$,what will be the ratio of their pressures?

Use of hot air balloons in sports and meteorological observations is an application of

$4 \ g$ 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 $M_B$?