




Consider one mole of an ideal gas at 25.0degree C. Calculate q, w, delta E, delta...
Suppose that we allow 3.50 mol of an ideal gas with Cv=5R/2 to expand isothermally and reversibly from 100 atm, 10 L to 10.0 atm and then the gas is allowed to expand adiabatically and reversibly to a final pressure of 1.00 atm. Calculate q, w, ΔU and ΔH for each step and the total values for the two steps. Suppose now that the processes are carried out irreversibly with pressure dropping discontinuously from 100 atm to 10.0 atm in...
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.
Calculate Delta U, Delta H, q and w when 1 mol of Ar at 25 C is allowed to expand isothermally from 3 atm to 1 atm a) reversibly and b) irreversibly against a constant external pressure of 1 atm.
**PLEASE ANSWER ALL SUB-QUESTIONS AND EXPLAIN STEP BY STEP.
THANK YOU!**
QUESTION 6 One mole of an ideal gas is compressed isothermally but irreversibly at 130 oC from 2.5 bar to 6.5 bar in a piston/cylinder device. The work required is 30 % greater than the work of reversible, isothermal compression. The heat transferred from the gas during compression flows to a heat reservoir at 25 °C. Calculate the entropy changes of the gas, the heat reservoir, and AStotal
QUESTION...
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
1. a) One mole of an ideal gas at 298.15 K is expanded reversibly and isothermally from 1.0 L to 15 L. Determine the amount of work in Joules. b) Determine the work done in Joules when one mole of ideal gas is expanded irreversibly from 1.0 L to 15.0 L against a constant external pressure of 1.0 atm.
One mole of ideal diatmic gas with Cv,m= 2.5 R at 27 C and .100 MPA is compressed adiabatically and reversibly to a final pressure of 1.00 MPa. Calculate the final temp, q,w, Delta U, and Delta H, and Delta S for the process.
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.
for the irreversible adiabatic heating of an ideal diatomic gas, calculate q, w, delta U, delta H, and the final temperature given p1 = 0.5 bar, p2 =3.5 bar, and T1 = 150 K
Interested in doing part B
1. a) One mole of an ideal gas is compressed irreversibly from 2 L to 1 L under a constant external pressure of 5 atm. The temperature is 300 K. Calculate the work done on the gas during the compression. b When the gas is cooled to sufficiently low temperatures, it is found experimentally that the equation of state for the gas no longer resembles the ideal gas law. Instead, what is found is that...