For irreversible expansion of an ideal gas under isothermal condition, the correct option is:

Question

For irreversible expansion of an ideal gas under isothermal condition, the correct option is: (A) Δ U =0, Δ S text total =0 (B) Δ U ≠ 0, Δ S text total ≠ 0 (C) Δ U =0, Δ S text total ≠ 0 (D) Δ U ≠ 0, Δ S text total =0

Tardigrade Admin · Accepted Answer

For an isothermal process, Δ T =0 ∴ Δ U =0 For an irreversible expansion, Δ S text total ≠ 0

Q. For irreversible expansion of an ideal gas under isothermal condition, the correct option is:

$Δ U = 0, Δ S_{total} = 0$

$Δ U \neq = 0, Δ S_{total} \neq = 0$

$Δ U = 0, Δ S_{total} \neq = 0$

$Δ U \neq = 0, Δ S_{total} = 0$

For an isothermal process, $Δ T = 0$
$∴ Δ U = 0$
For an irreversible expansion, $Δ S_{total} \neq = 0$

Q. For irreversible expansion of an ideal gas under isothermal condition, the correct option is:

ΔU=0,ΔStotal ​=0

ΔU=0,ΔStotal ​=0

ΔU=0,ΔStotal ​=0

ΔU=0,ΔStotal ​=0

For an isothermal process, ΔT=0 ∴ΔU=0 For an irreversible expansion, ΔStotal ​=0

$Δ U = 0, Δ S_{total} = 0$

$Δ U \neq = 0, Δ S_{total} \neq = 0$

$Δ U = 0, Δ S_{total} \neq = 0$

$Δ U \neq = 0, Δ S_{total} = 0$

For an isothermal process, $Δ T = 0$
$∴ Δ U = 0$
For an irreversible expansion, $Δ S_{total} \neq = 0$