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How does entropy differ from energy?
Related Topics
Wize University Physics Textbook (Master) > Thermodynamics
Entropy
2 Activities
How does entropy differ from energy?
A. Entropy does not obey a conservation law.
B. Entropy may be spelled differently, but otherwise it is a form of energy.
C. Entropy always remains constant.
D. Entropy relates to the transfer of energy.
E. Energy can only decrease, but entropy can only increase.
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More Entropy Questions:
Entropy: Heat Engines
A cylinder contains Nitrogen gas (𝐶
v
= 20.8
J
m
o
l
.
K
\frac{J}{mol.K}
m
o
l
.
K
J
, 𝛾 = 1.4) at a pressure of 3 atm and a temperature of 250K. Its initial volume is 2.0 liters. The Nitrogen gas is next carried through the following processes:
a. It is heated in an isochoric process to a temperature of 375K
b. It is expanded at a constant temperature to a volume of 3.0 liters
Thermodynamics: Entropy
If 3.0 kg of water at 100.0℃ is mixed with 1.0kg of ice at −10.0℃ . Find the
final temperature and the total change in entropy of the system.
(
C
w
=
4190
J
k
g
⋅
K
,
C
i
=
2100
J
k
g
⋅
K
,
L
f
=
334
×
10
3
J
K
g
)
\left(C_w=4190\ \frac{J}{kg\cdot K},\ C_i=2100\ \frac{J}{kg\cdot K},\ L_f=334\times10^3\ \frac{J}{Kg}\right)
(
C
w
=
4190
k
g
⋅
K
J
,
C
i
=
2100
k
g
⋅
K
J
,
L
f
=
334
×
1
0
3
K
g
J
)
Entropy: Heat Engines
A cylinder contains a diatomic gas at a pressure of 3 atm and a temperature of 250K. Its initial volume is 4.0 liters. The gas is next carried through the following processes:
a. It is expanded isobarically to a temperature of 375K.
b. It is cooled down to 250K in an isochoric process.
Predict the sign of the ΔH, ΔS,(+ or -) and identify when the following reactions are spontaneous at low temperature, high temperature, or all temperatures (low, high, all). Use commas to write your answers ie. +,+,low
For freezing of a popsicle: ΔH is ___________, ΔS is ___________. Reaction is spontaneous at ____________________ temperatures
For evaporation of liquid water: ΔH is ___________, ΔS is ___________. Reaction is spontaneous at ____________________ temperatures
Arrange the following compounds in order of increasing entropy, assuming 1 mol of each compound:
A
r
(
g
)
F
e
(
s
)
C
H
3
C
H
2
C
H
3
(
g
)
H
O
C
H
2
C
H
2
C
H
2
O
H
(
l
)
Ar(g) \hspace{15pt}Fe(s)\hspace{15pt} CH_3CH_2CH_{3(g)} \hspace{15pt} HOCH_2CH_2CH_2OH_{(l)}
A
r
(
g
)
F
e
(
s
)
C
H
3
C
H
2
C
H
3
(
g
)
H
O
C
H
2
C
H
2
C
H
2
O
H
(
l
)
A
r
(
g
)
Ar(g)
A
r
(
g
)