The gas equation $\frac{PV}{T} = \text{constant}$ is true for a constant mass of an ideal gas undergoing:

The temperature of an open room of volume $30\ m^3$ increases from $17^\circ C$ to $27^\circ C$ due to sunshine. The atmospheric pressure in the room remains $1 \times 10^5\ Pa$. If $n_i$ and $n_f$ are the number of molecules in the room before and after heating,then $n_f - n_i$ will be:

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

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

The $P-T$ graph shows a gas being heated. During this process from point $1$ to $2$,the volume of the gas:

If $300 \ ml$ of a gas at $27^{\circ}C$ is cooled to $7^{\circ}C$ at constant pressure,then its final volume will be ...... $ml$.