2. During some actual expansion and compression processes in piston-cylinder devices, the gases have been observed to satisfy the relationship PV" = C, where n and C are constants. Calculate the work done when a gas expands from 350 kPa and 0.03 m3 to a final volume of 0.2 m3 for the case of n = 1.5.

1. Calculate the work done in a polytropic (n=1.21) compression of a gas in a system with moving boundary from P1 = 15 psia, V1 = 1 ft3 to P2 = 150 psia, V2 = 0.15 ft3.

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A piston cylinder device has a volume of 0.04 m3 and initially contains air at 293 K and 1 bar.  This device is used to perform a cycle in which the gas is heated at a constant volume until the temperature reaches 1000 K.  The air is allowed to expand following an isothermal process until the volume is 3.5 times the original volume.  It is then cooled at a constant volume process.  The completion of the cycle is a PV1.36 = constant process back to the original state.  For the air, the specific heat is cv =0.79 kJ/(Kg K) = constant and its gas constant is RG=0.287 kJ/(Kg K).         Calculate the net work produced by this cycle, the required heat input to the cycle and its thermal efficiency. How much heat is removed from the system during the cycle? Could the heat removed from this cycle be used to heat or partial heat the water that is at an initial temperature of 298 K?  Would you recommend designing a heat recovery for this purpose?

An ideal gas in a leak tight cylinder-piston assembly undergoes an isobaric compression at a pressure of 4.94 bar, from V₁ = 9.46lt to V₂ = 3.37lt. Determine the work transferred to the gas during this process 1 -> 2 (absolute value). Ignore the pressure outside the piston and changes in the kinetic and potential energy. Present your answer in kilo Joules (kJ).

A gas with specific volume v₁ = 1 m³/Kg and pressure p₁=1bar in a closed system undergoes a thermodynamic cycle which consists of the following three separate processes: 1->2: Isobaric compression to v₂-0.25 m³/Kg 2->3: Isometric heating. 3->1: Isothermal expansion (pV = constant) to the initial volume. Calculate the specific work produced by the gas per cycle. Present your answer in kJ/kg.

An ideal gas with y= 1.30 occupies 7.0 L at 300 K and 200 kPa pressure. It is compressed adiabatically to 1/7 of its original volume, then cooled at constant volume to 300 K, and finally allowed to expand isothermally to 7.0 L. How much work does the gas do during this process? 6400 J O -980 J O -270,000 J O 980 J O -6400 J

In the process where the product of pressure and the volume is constant, a gas compression is carried out from an intial pressure of 200 kPa to a final pressure of 800 kPa. Consisting that the initial specific volume is 0.10 m^3 /kg, determine the work done per kilogram of gas.

A rigid tank of volume 10 m³ initially contains saturated water vapor at a temperature of 120 °C. Steam at a pressure 1.2 MPa and a temperature of 400 °C enters the tank through a valve in steam line that is connected to the tank until the final pressure in the tank is 800 kPa, at which time the temperature is 200 °C. All kinetic and potential energy effects can be neglected. A schematic of the problem and properties at all state points except state 1 are shown in the figure below. All of the properties at state 2 and the inlet state i are provided on the figure. Initial State in Tank T₁-120 °C, Sat. vapor u₁=? kJ/kg V₁=? m³/kg Pi=1.2 MPa, Ti-400 °C hi-3261.3 kJ/kg V=10 m³ Final State in Tank T: 200 °C, P₂-800 kPa u₂= 2631.1 kJ/kg v₂=0.26088 m³/kg Qout For Question 6: The initial specific internal energy, u1, of the saturated vapor in the tank in kJ/kg is

Calculate the amount of work necessary for the reversible compression of steam from 1 bar to 10 bar. The compression is to take place in a cylinder fitted with a weightless piston at the constant temperature of 500 oC. Under these conditions we have a superheated vapor. Assume that steam may be treated as an ideal gas. Report your answer in units of kJ/kg using three decimal places. For conversion, note that the molar mass of water is 18.015 g/mol.