Question

n = 3.39 mol of Hydrogen gas is initially at T = 364.0 K
temperature and p_{i} = 3.36×10^{5} Pa pressure.
The gas is then reversibly and isothermally compressed until its
pressure reaches p_{f} = 9.88×10^{5} Pa. What is
the volume of the gas at the end of the compression process?

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How much work did the external force perform?

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How much heat did the gas emit?

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How much entropy did the gas emit?

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What would be the temperature of the gas, if the gas was allowed to adiabatically expand back to its original pressure?

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Answer #1

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n = 4.42 mol of Hydrogen gas is initially at T = 304.0 K
temperature and pi = 3.23×105 Pa pressure.
The gas is then reversibly and isothermally compressed until its
pressure reaches pf = 8.93×105 Pa. What is
the volume of the gas at the end of the compression process?
Tries 0/12
How much work did the external force perform?
Tries 0/12
How much heat did the gas emit?
Tries 0/12
How much entropy did the gas emit?
Tries...

n = 3.71 mol of Hydrogen gas is initially at T = 300.0 K
temperature and pi = 2.78×105 Pa pressure.
The gas is then reversibly and isothermally compressed until its
pressure reaches pf = 9.52×105 Pa. What is
the volume of the gas at the end of the compression process?
Tries 0/20
How much work did the external force perform?
Tries 0/20
How much heat did the gas emit?
Tries 0/20
How much entropy did the gas emit?
Tries...

n = 3.63 mol of Hydrogen gas is initially at T = 316.0 K
temperature and pi = 2.58×105 Pa pressure.
The gas is then reversibly and isothermally compressed until its
pressure reaches pf = 8.99×105 Pa. What is
the volume of the gas at the end of the compression process?
Tries 0/20
How much work did the external force perform?
Tries 0/20
How much heat did the gas emit?
Tries 0/20
How much entropy did the gas emit?
Tries...

n = 4.13 mol of Hydrogen gas is initially at T = 367.0 K
temperature and pi = 1.85×105 Pa pressure.
The gas is then reversibly and isothermally compressed until its
pressure reaches pf = 6.59×105 Pa. What is
the volume of the gas at the end of the compression process?
A. How much work did the external force perform?
B. How much heat did the gas emit?
C. How much entropy did the gas emit?
D. What would be...

n = 4.44 mol of Hydrogen gas is initially at T = 357.0 K
temperature and pi = 3.03×105 Pa pressure. The gas is then
reversibly and isothermally compressed until its pressure reaches
pf = 9.97×105 Pa.
a) What is the volume of the gas at the end of the compression
process?
b) How much work did the external force perform?
c) How much heat did the gas emit?
d) How much entropy did the gas emit?
e) What would...

n = 3.50 mol of Hydrogen gas is initially at T = 309.0 K
temperature and pi = 2.34×105 Pa pressure.
The gas is then reversibly and isothermally compressed until its
pressure reaches pf = 8.91×105 Pa.
1. What is the volume of the gas at the end of the compression
process? 1.01×10-2
m^3
2. How much work did the external force perform?
3. How much heat did the gas emit?
4. How much entropy did the gas emit?
5....

n = 2.58 mol of Hydrogen gas is initially at T = 376 K
temperature and pi = 1.88×105 Pa pressure. The gas is then
reversibly and isothermally compressed until its pressure reaches
pf = 8.78×105 Pa. What is the volume of the gas at the end of the
compression process? What would be the temperature of the gas, if
the gas was allowed to adiabatically expand back to its original
pressure?

n = 3.50 mol of Hydrogen gas is initially at T = 310 K
temperature and pi = 3.22×105 Pa pressure.
The gas is then reversibly and isothermally compressed until its
pressure reaches pf = 7.51×105 Pa. What is
the volume of the gas at the end of the compression process??

You have 1.25 mol of hydrogen gas (CV =
5R/2 and Cp= 7R/2) at absolute
temperature 325 K. You allow the gas to expand adiabatically to a
final temperature of 195 K.
1) How much work does the gas do while being compressed?
2) What is the ratio of its final volume to its initial
volume?
3) What is the ratio of the final gas pressure to the initial
gas pressure?

In this problem, 1.10 mol of an ideal gas at 300 K undergoes a
free adiabatic expansion from V1 = 12.3 L to V2 = 22.2 L. It is
then compressed isothermally and reversibly back to its original
state.
(a) What is the entropy change of the universe for the complete
cycle?
J/K
(b) How much work is lost in this cycle?
J

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