The figure shows the volume versus temperature graph for the same mass of an ideal gas corresponding to two different pressures $P_1$ and $P_2$. Then,

What is the nature of the $P$ versus $1/V$ graph at a constant temperature?

Three containers of the same volume contain three different gases. The masses of the molecules are $m_1, m_2$ and $m_3$ and the number of molecules in their respective containers are $N_1, N_2$ and $N_3$. The gas pressures in the containers are $P_1, P_2$ and $P_3$ respectively. All the gases are now mixed and put in one of the containers. The pressure $P$ of the mixture will be

Air is filled at $60^{\circ} C$ in a vessel of open mouth. The vessel is heated to a temperature $t^{\circ} C$ so that $\frac{1}{4}$th of the air escapes from the vessel. Assuming air as an ideal gas and the volume of the vessel remains constant, the value of '$t$' is: (in $^{\circ} C$)

Explain Avogadro's hypothesis by relating pressure,temperature,and volume of a gas.

The expansion of an ideal gas of mass $m$ at a constant pressure $P$ is given by the straight line $B$. Then the expansion of the same ideal gas of mass $2\, m$ at a pressure $2\,P$ is given by the straight line