Calculate the number of moles of the gas having volume $2.5 \ L$ at $300 \ K$ and $4.5 \ atm$? $(R=0.0821 \ atm \ dm^3 \ K^{-1} \ mol^{-1})$

Calculate the density of methane at $27\,^oC$ and $2.0\, atm$ pressure in $g\, L^{-1}$.

The correct gas equation is:

At constant pressure,by what percentage must the temperature in Kelvin be increased to increase the volume by $10\%$?

$A$ gas occupies $10 \ L$ at $0 \ ^{\circ}C$ and $2 \ atm$ pressure. At what temperature will the pressure in the container be $2.5 \ atm$,assuming the volume remains constant (in $^{\circ}C$)?

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 :
$\left[ \text{Given } R = 0.082 \ L \ atm \ mol^{-1} \ K^{-1}, T = 273 \ K \right]$