ThermodynamicsHard
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?
Options
A.T3 > T1
B.T1 = T2
C.wisothermal > wadiabatic
D.ᐃUisothermal > ᐃUadiabatic
Solution
T1 = T2 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.
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.
Create a free account to view solution
View Solution FreeMore Thermodynamics Questions
Calculate the equilibrium constant for the reaction :PCl5 ⇋ PCl3 + Cl2 (g) (g) (g)at 400K if ᐃHo = 69418.86 ...The above p-v diagram represents the thermodynamic cycle of an engine, operating with an ideal monoatomic gas. The amoun...Five moles of an ideal gas expand isothermally and reversibly from an initial pressure of 100 atm to a final pressure of...What is the free energy change, ΔG, when 1.0 mole of water at 100°C and 1 atm pressure is converted into steam at 100°C ...The efficiency of a Carnot cycle is 1/6. On decreasing the temperature of the sink by 65°C, the efficiency increases to ...