An ideal gas has volume ${V_0}$ at ${27^{\circ}C}$. It is heated at constant pressure so that its volume becomes $2{V_0}$. The final temperature is

$A$ gas is contained in a $5 \, L$ vessel at a pressure of $0.8 \, m$. It is connected to another evacuated vessel of $3 \, L$ capacity. What will be the resultant pressure in $m$ (at constant temperature)?

The state of an ideal gas was changed isobarically. The graph depicts three such isobaric lines. Which of the following is true about the pressures of the gas?

From the following $P-T$ graph,what inference can be drawn?

The figure shows the pressure $P$ versus volume $V$ graphs for two different gas samples at a given temperature. $M_A$ and $M_B$ are the masses of the two samples,and $n_A$ and $n_B$ are the numbers of moles. Which of the following must be incorrect?

$4$ moles of an ideal gas is at $0^\circ C$. At constant pressure,it is heated to double its volume. Its final temperature will be ...... $^\circ C$.