The correct option for free expansion of an ideal gas under adiabatic condition is:

1.  $q=0,$ $∆T<0$ and $w>0$

2.  $q<0,$ $∆T=0$ and $w=0$

3.  $q>0,$ $∆T>0$ and $w>0$

4.  $q=0,$ $∆T=0$ and $w=0$

Under the isothermal condition, a gas at 300 K expands from 0.1 L to 0.25 L against a constant external pressure of 2 bar. The work done by the gas is:
[Given that 1 L bar = 100 J]

1. 30 J

2. –30 J

3. 5 kJ

4. 25 J

Reversible expansion of an ideal gas under isothermal and adiabatic conditions are as shown in the figure:

 

AB$\to$Isothermal expansion

AC$\to$Adiabatic expansion

Which of the following options is not correct?

1. $∆S_{isothermal}>∆S_{adiabatic}$

2. $T_A=T_B$

3. $W_{isothermal}>W_{adiabatic}$

4. $T_C>T_A$

Identify which of the following is the correct option for free expansion of an ideal gas under adiabatic condition.

1.  $\mathrm{ \Delta q}\ne 0,$ $∆\mathrm{T}=0,$ $\mathrm{W}=0$
2.  $\mathrm{ \Delta q}=0,$ $∆\mathrm{T}=0,$ $\mathrm{W}=0$
3.  $\mathrm{ \Delta q}=0,$ $∆\mathrm{T}<0,$ $\mathrm{W}\ne 0$
4.  $\mathrm{ \Delta q}=0,$ $∆\mathrm{T}\ne 0,$ $\mathrm{W}=0$

Identify the correct statement regarding entropy: