The temperature of $4.0 \ mol$ of a gas occupying $5 \ dm^3$ at $3.32 \ bar$ is $(R = 0.083 \ bar \ dm^3 \ K^{-1} \ mol^{-1})$. (in $K$)

Pressure of $1 \ g$ ideal gas $X$ at $300 \ K$ is $2 \ atm$. When $2 \ g$ of another gas $Y$ is introduced in the same vessel at the same temperature,the total pressure becomes $3 \ atm$. The correct relationship between molar masses of $X$ and $Y$ is:

Two vessels are filled with ideal gases $A$ and $B$ and are connected through a pipe of zero volume as shown in the figure. The stop cock is opened and the gases are allowed to mix homogeneously and the temperature is kept constant. The partial pressures of $A$ and $B$ respectively (in $atm$) are:

$1 \ L$ closed flask contains a mixture of $4 \ g$ of methane and $4.4 \ g$ of carbon dioxide. The pressure inside the flask at $27^{\circ} C$ is [Assume ideal behaviour of gases] (in $atm$)

The density of neon will be highest at

For an ideal gas,the number of moles per litre in terms of its pressure $P$,gas constant $R$,and temperature $T$ is: