$A$ perfect gas at $27^{\circ}C$ is heated at constant pressure so as to double its volume. The final temperature of the gas will be,close to ...... $^{\circ}C$

If a given mass of gas occupies a volume of $10\, cc$ at $1\, atm$ pressure and a temperature of $100^{\circ}C$ $(373.15\, K)$,what will be its volume at $4\, atm$ pressure,assuming the temperature remains constant?

On which does the value of $\alpha_V$ depend for an ideal gas?

Two different isotherms representing the relationship between pressure $p$ and volume $V$ at a given temperature for the same ideal gas are shown for masses $m_1$ and $m_2$ of the gas respectively in the figure given. Then:

The molecular weight of a gas is $44$. The volume occupied by $2.2 \, g$ of this gas at $0^\circ C$ and $2 \, atm$ pressure will be ....... $lit$.

The pressure-temperature graph for an ideal gas is shown in the figure. At point $A$,the density of the gas is $\rho_0$. What will be the density at point $B$?