$A$ gas at $27^\circ C$ temperature and $30$ atmospheric pressure is allowed to expand to atmospheric pressure. If the volume becomes $10$ times its initial volume,then the final temperature becomes ...... $^\circ C$.

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:

The $PV$ versus $T$ graph for equal masses of $H_2$,$He$,and $O_2$ is shown in the figure. Choose the correct alternative.

When air is filled in a balloon, both the pressure and volume increase while the temperature remains constant. Why is Boyle's law not obeyed in this case?

$A$ gas at a temperature of $27^{\circ}C$ has a volume $V$ and pressure $P$. If the pressure is doubled and the volume is tripled,what will be the new temperature in $^{\circ}C$?

The volume of a gas at pressure $21 \times 10^4 \ N/m^2$ and temperature $27^\circ C$ is $83 \ L$. If $R = 8.3 \ J/mol/K$,then the quantity of gas in $gm-mole$ will be: