Equal amounts of gases are kept in two separate containers. If the densities of the two gases are in $1:2$ ratio and their temperatures are in $2:1$ ratio, calculate the ratio of their respective pressures.

$100 \, g$ of an ideal gas is kept in a cylinder of $416 \, L$ volume at $27^{\circ} C$ under $1.5 \, bar$ pressure. The molar mass of the gas is $.... \, g \, mol^{-1}$. (Nearest integer) (Given : $R = 0.083 \, L \, bar \, K^{-1} \, mol^{-1}$)

At $300 \ K$,the following graph is obtained for one mole of an ideal gas. If its pressure is $10 \ atm$,then its volume (in $L$) will be

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 $R=0.082 \ L \ atm \ mol^{-1} \ K^{-1}$)

Calculate the weight of $CH_4$ in a $9 \ L$ cylinder at $16 \ atm$ and $27 \ ^\circ C$ in grams.

$V_0$ and $V_t$ are the volumes of a fixed mass of an ideal gas at $0^\circ \text{C}$ and $t^\circ \text{C}$ respectively at constant pressure. Find the ratio $V_t / V_0$.