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Consider 1.50 mol of a monoatomic ideal gas (Cv,m = 3/2R) thatis initially at 390.K (taken as 3 significant figures) and 2.20 atmpressure. For this system, calculate the change in entropy (ΔS),the change in internal energy (ΔU), and the change in enthalpy (ΔH)for a reversible adiabatic expansion of this gas to a finalpressure of 1.10 atm. Also calculate the final temperature (T) andvolume (V).

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Bunny Greenfelder
Bunny GreenfelderLv2
28 Sep 2019

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Related questions

One mole of a monoatomic ideal gas expands adiabatically from T= 298.15 K and P = 1 bar against a constant external pressure of0.75 bar. Find the final temperature of the gas, the molar workdone, and the change in the molar entropy for this process.

I understand the process is an irreversible adiabatic so I cannotuse PVδ=Constant

I Know:

q=0

ΔU=w=Cv(T2-T1)

w(irreversible)= -PextΔV

so, CvΔT=-PextΔV

Cv=3/2R, PV=nRT

Therefore : 3/2(R)(T2-T1) =-Pext{(RT2/Pext)-(RT1/P)}

I do not know how to solve forT2

I can finish the rest of the problem if someone could pleaseexplain (step-by-step) how to solve for T2

Any help would be greatly appreciated.

cyclic process

Consider an ideal gas with molar constant volume heat capacity, cV,m = 1.50 R. The gas undergoes the reversible four step cyclic process shown to the left: 1. During step 1, the gas expands isothermally from V1 to V2. 2. During step 2, the gas expands adiabatically from V2 to V3. 3. During step 3, the gas is compressed isothermally from V3 to V4. 4. During step 4, the gas is compressed adiabatically from V4 to V1. Given T1 = 350.0 K, P1 = 1.00 × 105 Pa, V1 = 5.82 × 10-2 m3 , V2 = 10.0 × 10-2 m3 , T3 = 175.0 K,

Perform the following calculations:

a. Determine the pressure, volume, and temperature of the gas at equilibrium points 1, 2, 3, and 4.

b. Calculate the work done on the gas during each step.

c. Calculate the transfer of energy into the gas as heat during each step.

d. Calculate the change in energy of the gas during each step.

e. Calculate q, w, and ΔU for the entire cyclic process.

f. Determine the enthalpy of the gas at equilibrium points 1, 2, 3, and 4.

g. Calculate the change in enthalpy of the gas during each step.

h. Calculate ΔH for the entire cyclic process.

i. Calculate the change in entropy of the gas during each step.

j. Calculate the change in entropy for the entire cyclic process

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