Problem 8 solution a cylinder contains nitrogen n2 at

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Unformatted text preview: n 10 minutes if the cubes were instead arranged as in diagram b? Problem 8 Solution A cylinder contains nitrogen N2 at a pressure of 4.00 atm. The volume is 2.00 L, and the temperature is 300 K. Assume that the nitrogen may be treated as an ideal gas. The Nitrogen is carried through the following processes: Process 1, the gas is heated at constant pressure from the initial state to T = 360 K. Process 2, the gas is cooled at constant volume to 250 K. Process 3, the gas is compressed at constant temperature to a volume of 2.00 L. Process 4, the gas is heated at constant volume to 300 K. (a) Draw the PV curve of this process (b) What is the efficiency of this device as a heat engine? (c) What is the change in entropy for process 3? Problem 7 1 Litre of Helium gas at room temperature (27°C) is heated at a constant volume from 1atm to 4atm. Then, it is expanded at a constant temperature to twice the volume. Then, it is expanded adiabatically to it’s original pressure. Finally it is compressed at a constant pressure to it’s initial state. a) Draw the PV curve of this process b) Find P, V, T at each state c) Find ΔU, Q, W in each step d) What is the efficiency of this process if this were a heat engine? e) What is the change in entropy for the Process 2? f) (at home, how would your answers change if we used Hydrogen gas instead?) Problem 8 A cylinder contains nitrogen N2 at a pressure of 4.00 atm. The volume is 2.00 L, and the temperature is 300 K. Assume that the nitrogen may be treated as an ideal gas. The Nitrogen is carried through the following processes: Process 1, the gas is heated at constant pressure from the initial state to T = 360 K. Process 2, the gas is cooled at constant volume to 250 K. Process 3, the gas is compressed at constant temperature to a volume of 2.00 L. Process 4, the gas is heated at constant volume to 300 K. (a) Draw the PV curve of this process (b) What is the efficiency of this d...
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This document was uploaded on 02/13/2014.

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