Calculate the volume of gas at $1.25 \ atm$,if the volume occupied by the gas at $1 \ atm$ and at the same temperature is $25 \ mL$. (in $mL$)

When the applied pressure is $16 \ atm$,the temperature is $27 \ ^oC$,and the volume is $9 \ L$,what will be the weight of $CH_4$ gas in $gm$? (Given $R = 0.08 \ L \ atm \ K^{-1} \ mol^{-1}$)

State Charles' law in brief.

Choose the correct option for the total pressure (in $atm$) in a mixture of $4 \ g$ $O_2$ and $2 \ g$ $H_2$ confined in a total volume of $1 \ L$ at $0^{\circ} C$ is :
$\left[ \text{Given } R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}, T = 273 \ K \right]$

$A$ vessel of $120 \, mL$ capacity contains a certain amount of gas at $35^{\circ} C$ and $1.2 \, bar$ pressure. The gas is transferred to another vessel of volume $180 \, mL$ at $35^{\circ} C$. What would be its pressure?

If the density of neon gas at $350 \ K$ is $0.9 \ g \ L^{-1}$,calculate the pressure of the gas. (in $bar$)