Two moles of nitrogen are initially at 10 bar and 600 K (state 1) in a horizontal piston/cylinder device. They are expanded adiabatically to 1 bar (state 2). They are then heated at constant volume to 600 K (state 3). Finally, they are isothermally returned to state 1. Assume that N2 is an ideal gas with a constant heat capacity as given on the back flap of the book (2.5*R for CV). Neglect the heat capacity of the piston/cylinder device. Supposed that heat can be supplied or reject as illustrated below. Assume each step of the process is reversible. Note: The figure is not shown but it consists of what is known as the Carnot Engine (Hot and Cold Reservoirs, Removable Insulation, and lid
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Two moles of nitrogen are initially at 10 bar and 600 K (state 1) in a horizontal piston/cylinder device. They are expanded adiabatically to 1 bar (state 2). They are then heated at constant volume to 600 K (state 3). Finally, they are isothermally returned to state 1. Assume that N2 is an ideal gas with a constant heat capacity as given on the back flap of the book (2.5*R for CV). Neglect the heat capacity of the piston/cylinder device. Supposed that heat can be supplied or reject as illustrated below. Assume each step of the process is reversible.
Note: The figure is not shown but it consists of what is known as the Carnot Engine (Hot and Cold Reservoirs, Removable Insulation, and lid that performs Ws)
- (a) Calculate the heat transfer and work done on the gas for each step and overall.
- (b) Taking state 1 as the reference state, and setting URig = 0, calculate U and H for the nitrogen at each state, and ΔU and ΔH for each step and the overall Q and WEC.
- (c) The atmosphere is at 1 bar and 298 K throughout the process. Calculate the work done on the atmosphere for each step and overall (Hint: Take the atmosphere as the system.) How much work is transferred to the shaft in each step and overall?
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