What is the new temperature of a gas when its initial volume $3 \ dm^3$ at $300 \ K$ is doubled at constant pressure (in $K$)?

The value of the gas constant $R$ is closest to which of the following values?

For $1 \ mol$ of an ideal gas,an isochore is obtained. The slope of the isochore is $0.082 \ atm \ K^{-1}$. What will be its pressure (in $atm$) when the temperature is $12.2 \ K$? $(R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1})$.

The following $P$ vs $V$ curve is plotted. What is the relation between $T_1$,$T_2$ and $T_3$?

Pressure remaining the same,the volume of a given mass of an ideal gas increases for every degree centigrade rise in temperature by a definite fraction of its volume at:

$A$ dry gas occupies $136.5 \, cm^3$ at $STP$. If the same mass of gas is collected over water at $27 \, ^oC$ and a total pressure of $725 \, torr$,what volume will it occupy in $cm^3$? (Vapour pressure of water at $27 \, ^oC$ is $25 \, torr$.)