The volume of a gas at $20^{\circ}C$ is $200\, ml$. If the temperature is reduced to $-20^{\circ}C$ at constant pressure,its volume will be ...... $ml$.

$A$ cylinder contains $10 \, kg$ of gas at a pressure of $10^7 \, N/m^2$. What amount of gas in $kg$ must be removed so that the final pressure becomes $2.5 \times 10^6 \, N/m^2$?

$A$ gas is heated through $1\,^{\circ}C$ in a closed vessel. Its pressure is increased by $0.5\%$. The initial temperature of the gas is ...... $^{\circ}C$.

You have two containers of equal volume. One is full of helium gas. The other holds an equal mass of nitrogen gas. Both gases have the same pressure. How does the temperature of the helium compare to the temperature of the nitrogen?

Two spheres are connected to each other as shown in the figure. The volume of sphere $I$ is twice the volume of sphere $II$. They contain an ideal gas at temperatures $100 K$ and $200 K$,respectively. If the mass of the gas in sphere $I$ is $m$,what is the mass of the gas in sphere $II$?

The following graph represents the $T-V$ curves of an ideal gas (where $T$ is the temperature and $V$ is the volume) at three pressures $P_1, P_2$ and $P_3$ compared with those of Charles's law represented as dotted lines. Then the correct relation is: