$A$ 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 ...... $^{\circ}C$.

The expansion of an ideal gas of mass $m$ at a constant pressure $P$ is given by the straight line $B$ in the $V-T$ graph. Then the expansion of the same ideal gas of mass $2m$ at a pressure $2P$ is given by the straight line:

$A$ 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?

$12\,g$ of gas occupies a volume of $4\times 10^{-3}\,m^3$ at a temperature of $7\,^oC$. After the gas is heated at constant pressure,its density becomes $6\times 10^{-4}\,g/cc$. Find the temperature $T$ (in $K$) to which the gas was heated.

The temperature of a gas having $2.0 \times 10^{25}$ molecules per cubic meter at $1.38 \text{ atm}$ (Given,$k = 1.38 \times 10^{-23} \text{ J K}^{-1}$) is: (in $\text{ K}$)

Which one of the following represents correctly the variation of volume $(V)$ of an ideal gas with temperature $(T)$ under constant pressure conditions?