4) Problem 3.23 in book (with corrections): Treating the energy of an arbitrary system (e.g. no assumptions about ideality) as a function of temperature and volume, the following expression is the exact differential for dU: dU(T,V)= dT + dV. ÔT V T Using this expression, give the exact differential of dU for a van der Waals gas, for which the internal energy is as follows: 3 n2 U = nRT - - a. 2 V

Part A: 10 moles of ideal gas initially at 10 atm and 250 K is expanded isothermally and reversibly to a final pressure of 2 atm. Calculate W, AU, and Q in Joules. Part B: The same gas in problem A, starting in the same initial state, is expanded isothermally against a constant external pressure of 2 atm, to a final pressure of 2 atm. Calculate W, AU, and Q in Joules for this irreversible process. Part C: The same gas in part B, starting in the same initial state, is expanded isothermally to a final pressure of 2 atm. The process is carried out in 4 stages. First the gas is expanded against a constant pressure of 8 atm, to 8 atm. Then the gas is expanded against a constant pressure of 6 atm, to 6 atm. Then the gas is expanded against a constant pressure of 4 atm, to 4 atm. Finally, the gas is expanded against a constant pressure of 2 atm, to 2 atm. Calculate w, AU, and Q in Joules for the 4-step process. How do your answers compare to those you obtained for problems 5 and 6 above?

(c) Determine the average (internal) energy of the system, ⟨?⟩.

Problem 1: Describe a situation in which the entropy of a container of gas is constant. In other words, come up with your own problem where the answer is that AS = 0.

please answer v

Part A: 10 moles of ideal gas initially at 10 atm and 250 K is expanded isothermally and reversibly to a final pressure of 2 atm. Calculate W, AU, and Q in Joules. Part B: The same gas in problem A, starting in the same initial state, is expanded isothermally against a constant external pressure of 2 atm, to a final pressure of 2 atm. Calculate W, AU, and Q in Joules for this irreversible process. Part C: The same gas in part B, starting in the same initial state, is expanded isothermally to a final pressure of 2 atm. The process is carried out in 4 stages. First the gas is expanded against a constant pressure of 8 atm, to 8 atm. Then the gas is expanded against a constant pressure of 6 atm, to 6 atm. Then the gas is expanded against a constant pressure of 4 atm, to 4 atm. Finally, the gas is expanded against a constant pressure of 2 atm, to 2 atm. Calculate W, AU, and Q in Joules for the 4-step process.

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Please and thank you for your help! Make sure the answer is in the correct units! NO TUTOR HAD GOT THIS CORRECT

A sample of a monatomic ideal gas occupies 5.00 L at atmospheric pressure and 300 K (point A in the figure below). It is warmed at constant volume to 3.00 atm (point B). Then it is allowed to expand isothermally to 1.00 atm (point C) and at last compressed isobarically to its original state. Р (atm) 3 B 1 V (L) 5 10 15 (a) Find the number of moles in the sample. moles (b) Find the temperature at point B. K (c) Find the temperature at point C. (d) Find the volume at point C. L (e) Now consider the processes A - B, B → C, and C- A. Describe how to carry out each process experimentally.

An ideal gas, initially at a pressure of 10.3 atm and a temperature of 312 K, is allowed to expand adiabatically until its volume doubles.   What is the gas’s final temperature, in kelvin, if the gas is monatomic?  What is the gas’s final pressure, in atmospheres, if the gas is diatomic?