Question

a) Calculate delta S(system) for the reversible heating of 1 mol of ethane from 298K to 1500 K at constant pressure. Use Cp = 5.351 + 177.669x10-3 T – 687.01x10-7 T ^2 + 8.514x10-9 T ^3 (J/mol K). Consider the reversible Carnot cycle discussed in class with 1 mol of an ideal gas with Cv=3/2R as the working substance. The initial isothermal expansion occurs at the hot reservoir temperature of Thot=600C from an initial volume of 3.50 L to a volume 10.0 L. The system then undergoes an adiabatic expansion until the temperature falls to Tcold=150 C. The system then undergoes an isothermal compression until the initial state Thot = 600C and V = 3.5L is reached.

b)Calculate the work, q, U and H for each step in the cycle and for the total cycle.

Answer #1

Suppose 4.00 mol of an ideal gas undergoes a reversible
isothermal expansion from volume V1 to volume V2 = 8V1 at
temperature T = 300 K. Find (a) the work done by the gas and (b)
the entropy change of the gas. (c) If the expansion is reversible
and adiabatic instead of isothermal, what is the entropy change of
the gas?

A sample of 1.95 mol H2 (Cv = 20.5 J K-1 mol-1) at 21°C and 1.50
atm undergoes a reversible adiabatic compression until the final
pressure is 4.50 atm. Calculate the final volume of the gas sample
and the work associated with this process. Assume that the gas
behaves ideally.

Ideal gas ethylene undergoes a reversible adiabatic compression
by which its temperature increases from T1 = 300 K to T2 = 450 K.
The molar entropy in the initial state is given as s1 = 100 J K–1
mol–1, and here, for ethylene, cp = ?T + c0 with ? = 0.1 J K–2
mol–1 and c0 = 13.1 J K–1 mol–1. Determine the change of the molar
entropy s2 – s1 and the change of the chemical potential ?2...

Consider 5.000 mol of neon in a 208.7 cm^3 piston at 120.0 K. If
the gas undergoes isometric cooling to one-half of its initial
temperature and then undergoes isothermal reversible expansion to
four times of its initial volume, (a) compute the work done
assuming the gas behaves ideally. Next, (b) compute the work done
for the entire process assuming the gas behaves as a van der Waal's
gas (a = 0.2050 atmL^2/mol^2, b = 1.670 x 10^-2 L/mol). (c) Compare...

2.15 mol of an ideal gas with CV,m=3R/2
undergoes the transformations described in the following list from
an initial state described by T=350.K and
P=5.00bar.
1) The gas undergoes a reversible adiabatic expansion until the
final pressure is one-fourth its initial value.
2) The gas undergoes an adiabatic expansion against a constant
external pressure of 1.25 bar until the final pressure is
one-fourth its initial value.
3)The gas undergoes an expansion against a constant external
pressure of zero bar until...

N moles of this gas undergoes the following cyclical process
composed of four reversible steps:
i. Isovolumetric cooling from state 1 (T1 and P1) to State 2 (T2
and P2);
ii. Isothermal expansion from state 2 (T2 and P2) to state 3 (T2
and P3);
iii. Isovolumetric heating from state 3 (T2 and P3) back to
state 4 (T4 and P4); and
iv. Adiabatic compression from state 4 (T4 and P4) to state 1
(T1 and P1).
We know that...

) An ideal gas (Cp = 5 kcal/kmol, Cv = 3
kcal/kmol) is changed from 1 atm and 22.4 m3 to 10 atm
and 2.24 m3 by the following reversible process
(i) Isothermal
compression
(ii) Adiabatic
compression followed by cooling at constant volume
(iii) Cooling at
constant pressure followed by heating at constant volume
Calculate the heat, work requirement,
?U and ?H for each
process.

Calculate the change in entropy for one mole of ideal gas which
expands from an initial volume of 2 L and initial temperature of
500 K to a final volume of 6 L under the following conditions.
P(initial) refers to the pressure when T(initial)= 500K,
V(initial)= 2 L.
a) Irreversible expansion against a constant pressure of
Pinitial/2
b) Irreversible expansion against a vacuum...a 'free
expansion'.
c) Adiabatic irreversible expansion against a constant pressure
of Pfinal
d) Adiabatic reversible expansion

3.75 moles of ideal fas with CV,m=3/2R undergoes the
transformations described in the following list from an initial
state described by T=298K and P=4.50 bar.
c)The gas undergoes an expansion against a constant external
pressure of zero bar until the final pressure is one third its
initial value. Find S

A 0.505-mol sample of an ideal diatomic gas at 408 kPa and 309 K
expands quasi-statically until the pressure decreases to 150 kPa.
Find the final temperature and volume of the gas, the work done by
the gas, and the heat absorbed by the gas if the expansion is the
following.
(a) isothermal
final temperature K
volume of the gas
L
work done by the gas
J
heat absorbed
J
(b) adiabatic
final temperature K
volume of the gas L...

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