Two moles of an ideal diatomic gas, with a ratio of heatcapacities γ = 1.40, initially has a pressure p1 = 0.500 atm, a volume V1 = 45.0 L and a temperature T1. Then thegas undergoes the following three-step cyclic process, as shown in the p-V diagram below.
(i) Adiabatic expansion from the temperatureT1, pressure p1, and volume V1 to a temperature T2, volume V2 = 65.0 L and pressure p2. (ii) Increase in pressure at constant volume to a pressure p3 and a temperature T3. (iii) Isothermal compression to the original starting pressure, volume, and temperature.question:(a) What is T1? (b) What are p2 and T2? (c) What are T3 and p3? (d) What is the work done by the gas during each of the three steps of the cycle? What is thenet work done by the gas during the entire cycle? (e) How much heat is absorbed by the gas during each of the threesteps of the cycle? What is the net heat absorbed by the gas duringthe entire cycle? Why should this last result be exactly the same as the last resultin part (d)? (f) If the cycle is repeated 15 times/second, what is the net workpower done by the system? What is the net heat power absorbedby the system?
