$A$ container of fixed volume contains a gas at $27^{\circ} C$. To double the pressure of the gas,the temperature of the gas should be raised to . . . . . . ${ }^{\circ} {C}$.

$A$ gas container $A$ is in thermal equilibrium with another gas of the same mass in container $B$. If we denote the corresponding pressures and volumes by the suffixes $A$ and $B$,then which of the following statements is most likely to be true?

State Boyle's law and Charles's law.

$A$ container $AB$ in the shape of a rectangular parallelepiped of length $5 \,m$ is divided internally by a movable partition $P$ as shown in the figure. The left compartment is filled with a given mass $m$ of an ideal gas of molar mass $M_1 = 32$ while the right compartment is filled with an equal mass $m$ of another ideal gas of molar mass $M_2 = 18$ at the same temperature. What will be the distance of $P$ from the left wall $A$ when equilibrium is established (in $\,m$)?

The pressure of a given mass of gas at $20^{\circ}C$ is $P$. At constant volume,at what temperature in $^{\circ}C$ will the pressure of the gas become $2P$?

At constant pressure,the ratio of the increase in volume of an ideal gas per degree rise in temperature to its original volume is ... (where $T$ is the absolute temperature of the gas).