A balloon filled with helium $\left(32^{\circ} C \right.$ and $1.7\; atm$.) bursts. Immediately afterwards the expansion of helium can be considered as
A balloon filled with helium $\left(32^{\circ} C \right.$ and $1.7\; atm$.) bursts. Immediately afterwards the expansion of helium can be considered as
- [JEE MAIN 2020]
- A
Irreversible isothermal
- B
Irreversible adiabatic
- C
Reversible adiabatic
- D
Reversible isothermal
Similar Questions
$Assertion :$ In adiabatic compression, the internal energy and temperature of the system get decreased.
$Reason :$ The adiabatic compression is a slow process.
$Assertion :$ In adiabatic compression, the internal energy and temperature of the system get decreased.
$Reason :$ The adiabatic compression is a slow process.
- [AIIMS 2001]
Check the statement are trrue or false :
$1.$ For an adiabatic process $T{V^{\gamma - 1}}$ $=$ constant.
$2.$ Charging process of battery is a reversible process.
$3.$ Water falls below from height is a reversible process.
$4.$ Internal energy, volume and mass are intensive variable while pressure, temperature and density are extensive variables.
Check the statement are trrue or false :
$1.$ For an adiabatic process $T{V^{\gamma - 1}}$ $=$ constant.
$2.$ Charging process of battery is a reversible process.
$3.$ Water falls below from height is a reversible process.
$4.$ Internal energy, volume and mass are intensive variable while pressure, temperature and density are extensive variables.
The adiabatic elasticity of a diatomic gas at $NTP$ is ........ $N / m ^2$
The adiabatic elasticity of a diatomic gas at $NTP$ is ........ $N / m ^2$
Starting at temperature $300\; \mathrm{K},$ one mole of an ideal diatomic gas $(\gamma=1.4)$ is first compressed adiabatically from volume $\mathrm{V}_{1}$ to $\mathrm{V}_{2}=\frac{\mathrm{V}_{1}}{16} .$ It is then allowed to expand isobarically to volume $2 \mathrm{V}_{2} \cdot$ If all the processes are the quasi-static then the final temperature of the gas (in $\left. \mathrm{K}\right)$ is (to the nearest integer)
Starting at temperature $300\; \mathrm{K},$ one mole of an ideal diatomic gas $(\gamma=1.4)$ is first compressed adiabatically from volume $\mathrm{V}_{1}$ to $\mathrm{V}_{2}=\frac{\mathrm{V}_{1}}{16} .$ It is then allowed to expand isobarically to volume $2 \mathrm{V}_{2} \cdot$ If all the processes are the quasi-static then the final temperature of the gas (in $\left. \mathrm{K}\right)$ is (to the nearest integer)
- [JEE MAIN 2020]
One mole of an ideal gas $(\gamma = 1.4)$ is adiabatically compressed so that its temperature rises from $27\,^oC$ to $35\,^oC$ . The change in the internal energy of the gas is .... $J$. (given $R = 8.3\,J/mole-K$ )
One mole of an ideal gas $(\gamma = 1.4)$ is adiabatically compressed so that its temperature rises from $27\,^oC$ to $35\,^oC$ . The change in the internal energy of the gas is .... $J$. (given $R = 8.3\,J/mole-K$ )