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(3) Adiabatic and isothermal processes drawn in p-V diagrams are called adiabats and isotherms,
respectively. Show the following relation between adiabats and isotherms for ideal gas:
(др
av
ad
= Y
(ap
Ꭷv .
T

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3. Compute the heat and work for the following reversible processes of a monatomic ideal gas (see the graph below): (a) isothermal expansion from (P1, V1, T1) to (P2, V2, T1), namely the path A; (b) adiabatic expansion from (P1, V1, T1) to (P3, V2, T2) followed by an constant-volume heating to (P2, V2, T1), namely path B+C; (c) constant expansion from (P1, V1, T1) to (P1, V2, T3) followed by a constant-volume cooling to (P2, V2, T1), namely path D+E. Numerical values of some variables: P1=2 bar, Vı=1 L, Ti=300 K, 3R P2=1 bar, V2= 2 L, Cy = 2 P1, V1, T1 P.V2, T3 A E P P2, V2, T1 C B 'P3, V2, T2 V
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An ideal gas with γ =1.4 occupies 4.5 LL at 300 K and 110 kPa pressure and is heated at constant volume until its pressure has doubled. It's then compressed adiabatically until its volume is one-fourth its original value, then cooled at constant volume to 300 K, and finally allowed to expand isothermally to its original state. Find the net work done on the gas in joules.
Correction: "There is an adiabatic expansion to point B"
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