Question

. A container has n = 3 moles of a monoatomic ideal gas at a temperature of 330 K and an initial pressure of three times the atmospheric pressure. The gas is taken through the following thermodynamic cycle: 1.- The gas is expanded isobarically (constant pressure) to Vf = 2.5∙Vi. 2.- The pressure of the gas is decreased isochorically (constant volume) to half of the initial value. 3.- The gas is compressed isobarically back to its initial volume. 4.- The gas is brought to its original state by an isochoric compression. A) Use ideal gas law to find the initial volume of the gas. (2 pts) B) Draw a PV diagram describing the process. (2 pts) C) What is the work W done by the gas in the full cycle? D) What is the change in the internal energy of the gas in the full cycle? (2 pts) E) How much heat energy Q flows out of the gas during the full cycle?

Answer #1

3 moles of a monoatomic ideal gas with Cv=(32)RT occupies a
volume of 3.2L at a pressure of 1.9atm at point A. The gas is
carried through a cycle consisting of three processes:
1. The gas is heated at constant pressure until its volume is 4.4L
at point B.
2. The gas is cooled at constant volume until the pressure
decreases to 1.2atm (C).
3. The gas undergoes an isothermal compression back to point
A.
Find W for the isochoric...

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Use these steps to answer the questions below:
Step 1: A sample of monoatomic ideal gas, initially at pressure
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reversibly to a final pressure P2 and volume
V2
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Wsys (Step 1)
=
qsys (Step 2)
=

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A cylinder with a piston contains 0.100 mol of nitrogen at
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One mole of a monoatomic, ideal gas at initial pressure
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