Application of First Law of Thermodynamics---
2. Compute w,q, and AU for the following processes by an ideal gas: 1) irreversible expansion against a constant ex...
1 mole 2. Compute w,q, and AU for the following processes by an ideal gas: 1) irreversible expansion against a constant external pressure of 2.00 atm from 5.00 L to 10.00 L at 30°C. 2) one irreversible compression using minimum external pressure to achieve the reverse process.
Compute the work done by a gas on the surrounds when it expands against a constant external pressure of 2.00 atm from 5.00 L to 10.00 L at 30C. If 2.00 atm is the gas pressure at 10.00 L, 30C, compute the number of mole of gas. Compute the work that must be done by the surrounds on the gas to return the gas to its initial state using one irreversible compression.
2) Construct a table (or use the one below) with 9,w, AU, AH as the headings. Determine whether each of these quantities is postive, negative, or zero for five (5) of the following nine processes. (If you choose more than five, only the first five answers will be graded, so decide which five you are most confident in and only answer those.) (4 pts each. 20 pts total) 1. Freezing of acetone at 1 atm and it's normal freezing point....
Consider the expansion of 1.00 mole of (ideal) Ne from 2.00 atm at 75.00 C: the volume is doubled in the process. Find q, w, Delta H and the final pressure and temperature for a) reversible adiabatic expansion b) reversible isothermal expansion c) reversible constant pressure expansion d) irreversible adiabat against 0.500 atm external pressure
2. One mole of an ideal gas at an initial state of 300 K, 2.4618 atm and 10.0 L is isothermally expanded to 20.0 L against a constant external pressure of 1.2309 atm. Calculate AU, W, q, and AS for the process. Show that the Clausius inequality is satisfied.
2. One mole of an ideal gas at an initial state of 300 K, 2.4618 atm and 10.0 L is isothermally expanded to 20.0 L against a constant external pressure of 1.2309 atm. Calculate AU, W, q, and AS for the process. Show that the Clausius inequality is satisfied.
Consider one mole of an ideal gas at 25.0degree C. Calculate q, w, delta E, delta H, delta S, and delta G for the expansion of this gas isothermally and irreversibly from 2.45 times 10^-2 atm to 2.45 times 10^-3 atm in one step. Calculate q, w, delta E, delta H, delta S, and delta G for the same change of pressure as in part (a) but performed isothermally and reversibly. Calculate q, w, delta E, delta H, delta S,...
10 moles of an ideal gas expands irreversibly against an unknown constant external pres- sure, Pert, from an initial volume Vİ-1 L to a final volume ½ 11 L. In the process, the temperature of the gas falls from T350 K to T2 250 K, and it absorbs heat q+7 L atm from the surroundings. (a) What is the external pressure, Pert (in atm)? [Note: this is an ideal gas, so its internal energy depends only on its temperature.] (b)...
Assume there's 1 mol ideal mono-atomic gas in a 22.4L container at 300K. The initial entropy of the system is 100J/K. For the following processes, calculate: a) q and w for a reversible expansion to twice the volume, isothermally. b) S and G for irreversible isothermal expansion against a constant 0.5 bar external pressure, to a final internal pressure of 0.5 bar. c) U and H for adiabatic reversible expansion to twice the volume.
(3). A sample of 1.00 mol ideal gas molecules with Com= 7/2 R is initially at p = 1.00 bar and V = 22.44 L and then put thought the following cycle in reversible processes: (a) constant-pressure expansion to twice its initial volume, (b) constant volume cooling to its initial temperature, (c) isothermal-compression back to 1.00 bar. Calculate q, w, AU, AH, AS for each process and for the whole cycle. (20 pts)