Liquefied natural gas(LNG) is mainly methane. A $10.0 {\mathrm{m}}^3$ tank is constructed to store LNG at $-{164}^{\circ }\mathrm{C}$ and $1 \mathrm{atm}$ pressure, under this condition density of LNG is $416 \mathrm{kg}/{\mathrm{m}}^3$. The volume $(\mathrm{in} \mathrm{L})$ of a storage tank capable of holding the same mass of LNG as a gas, at ${27}^{\circ }\mathrm{C}$ and $1.642 \mathrm{atm}$ pressure is, $\mathrm{V}=\mathrm{x}\times {10}^5 \mathrm{L}$. What is the value of $\mathrm{x}$ ?

Which one of the following graphs is not correct for ideal gas?

$\mathrm{d}=$ Density, $\mathrm{P}=$ Pressure, $\mathrm{T}=$Temperature

One moles each of four ideal gases are kept as follows. 

I. $5 \mathrm{L}$ of gas $\left(\mathrm{A}\right)$ at $2 \mathrm{atm}$ pressure

II. $2.5 \mathrm{L}$ of gas $\left(\mathrm{B}\right)$ at $2 \mathrm{atm}$ pressure

III. $1.25 \mathrm{L}$ of gas $\left(\mathrm{C}\right)$ at $2 \mathrm{atm}$ pressure

IV. $2.5 \mathrm{L}$ of gas $\left(\mathrm{D}\right)$ at $2.5 \mathrm{atm}$ pressure

Which of the above gases is kept at highest temperature.

The volume of gas $\mathrm{A}$ is twice than that of gas $\mathrm{B}$. The compressibility factor of gas $\mathrm{A}$ is thrice than that of gas $\mathrm{B}$ at same temperature. What are the pressures of the gases for equal number of moles?

A container of volume $2.24 \text{L}$can with stand a maximum pressure of $2$ atm at $298 \text{K}$ before exploding. The maximum amount of nitrogen (in $\text{g}$) that can be safely put in this container at this temperature is closest to