The reversible expansion of an ideal gas under adiabatic and isothermal conditions is shown in the figure. Which of the following statement(s) is (are) correct?

Question

The reversible expansion of an ideal gas under adiabatic and isothermal conditions is shown in the figure. Which of the following statement(s) is (are) correct? (A) TI=T2 (B) T3>TI (C) w text isothermal >w text adiabatic  (D) Δ U text isothermal >Δ U text adiabatic

Tardigrade Admin · Accepted Answer

T 1= T 2 because process is isothermal. Work done in adiabatic process is less than in isothermal process because area covered by isothermal curve is more than the area covered by the adiabatic curve. In adiabatic process expansion occurs by using internal energy hence it decreases while in isothermal process temperature remains constant that's why no change in internal energy.

Q. The reversible expansion of an ideal gas under adiabatic and isothermal conditions is shown in the figure. Which of the following statement(s) is (are) correct?

$T_{I} = T_{2}$

$T_{3} > T_{I}$

$w_{isothermal} > w_{adiabatic}$

$Δ U_{isothermal} > Δ U_{adiabatic}$

Q. The reversible expansion of an ideal gas under adiabatic and isothermal conditions is shown in the figure. Which of the following statement(s) is (are) correct?

TI​=T2​

T3​>TI​

wisothermal ​>wadiabatic ​

ΔUisothermal ​>ΔUadiabatic ​

$T_{I} = T_{2}$

$T_{3} > T_{I}$

$w_{isothermal} > w_{adiabatic}$

$Δ U_{isothermal} > Δ U_{adiabatic}$