7.5) A 1.15 -mol quantity of monatomic ideal gas undergoes the following cyclic process. The gas starts at point a at STP. It expands isothermally to point b, where the volume is 2.2 times its original volume. Next, heat is removed while keeping the volume constant and reducing the pressure. Finally, the gas undergoes adiabatic compression, returning to point a.
a. Calculate the pressures at b and c. (answers in Pa)
**Find the volumes at a and b first.
**Use the relations between pressure and volume for isothermal and
adiabatic processes, as appropriate.Use the relation between the
volume and temperature for an adiabatic process.
b. Determine the temperature at c. (answer in kelvin)
c. Find the work W done by the gas, heat Q added to the gas, and the change in entropy ΔS of the gas in each step (a-b, b-c, c-a) --> (expecting 9 answers)
**Since T is constant in an isothermal process, ΔS = Q/T
**Use the relation dS = dQ/T, and note that dQ = dU for this process. Hence dS = (3/2) n R dT/T.
d. Calculate the efficiency e of this cycle.
7.5) A 1.15 -mol quantity of monatomic ideal gas undergoes the following cyclic process. The gas...
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