Question

Explain how (without doing any calculations), given heat capacities at different temperatures, you can find the entropy change upon heating a substance.

Answer #1

Entropy is the ratio of heat transferred to the temperature in the
equilibrium process.

So upon heating, we can multiply the change in temperature to the
heat capacities to obtain the heat transferred at a given
temperature.

The sum of the ratio of heat transferred to temperature will give
the total entropy change during the heating process.

To obtain the equilibrium like heat transfer through infinte no of
small steps with with infinitesimal temperature change, we
integrate the ratio of heat transfer to temperature to obtain the
entropy change for the given temperature change.

Explain why
A) If heat flows from high to low temperatures, the entropy
change in any process cannot be negative.
B) The specific heat of any substance is always lowest in the
vapor (gas) phase.

Consider two bodies with temperature independent heat capacities
C1 and C2, and initial temperatures T1 > T2.
(a) If the two bodies are brought into contact such that the
only heat exchange is between them, what is the final temperature
Tfinal , and what is the change in entropy.
(b) Suppose instead that the difference in temperature between
the two bodies is used to drive an ideal heat engine (Carnot
cycle). In one operation of the cycle some amount of...

5. You can tell a lot about an expression without doing any
computation. For example, the expression 16(5+t)(17-t) can be used
to model how high a toy rocket is in the air after t seconds. a.
Describe the expression. b. When is the value of the expression
negative? Explain how you know. c. What does it mean for the
expression to be negative in terms of the rocket?

Explain in the simplest way possible how you would find the
following volumes or capacities with a spirometer.
-Tidal volume
-Expiratory reserve volume
-Inspiratory reserve volume
-Vital Capacity

Assignment 3
Exercise 17.30
17 of 24
Constants | Periodic Table
Without doing any calculations, determine the sign of
ΔSsys and ΔSsurr for each of the chemical
reactions below.
Part A
2CO(g)+O2(g)→2CO2(g)ΔrH∘=
-566.0 kJmol−1
-566.0
ΔSsys>0, ΔSsurr>0
ΔSsys<0, ΔSsurr>0
ΔSsys>0, ΔSsurr<0
ΔSsys<0, ΔSsurr<0
Request Answer
Part B
2NO2(g)→2NO(g)+O2(g)ΔrH∘=
113.1 kJmol−1
113.1
ΔSsys>0, ΔSsurr>0
ΔSsys<0, ΔSsurr>0
ΔSsys>0, ΔSsurr<0
ΔSsys<0, ΔSsurr<0
Request Answer
Part C
2H2(g)+O2(g)→2H2O(g)ΔrH∘=
-483.6 kJmol−1
-483.6
ΔSsys>0, ΔSsurr>0
ΔSsys<0, ΔSsurr>0
ΔSsys>0, ΔSsurr<0
ΔSsys<0, ΔSsurr<0
Request Answer
Part D
CO2(g)→C(s)+O2(g)ΔrH∘=...

This problem examines the effects of mixing water at two
different temperatures and/or two different phases, such as
dropping ice cubes into warm water. Assume that heat of fusion is
333.55 J/g, that CP for ice is constant at 2.11 J/(g·K), and CP for
liquid water is constant at 4.19 J/(g·K). You can assume CP
approximately equals CV for solids and liquids. For each of the
following cases, assume the mixing is adiabatic and carried out at
atmospheric pressure. Find...

Heat is transferred from a substance. What can you say about the
change in entropy Δs if the process is reversible?
a. Δs ≥ 0
b. Δs = 0
c. Δs ≤ 0
d. Δs > 0
e. Δs < 0

how is it possible that assets without any physical substance
can have monetary value for accounting purposes?

How do you know that heat is a form of energy? Explain that heat
is not a substance that flows from a hotter body to a colder one.
Refer to specific observations. What is special about the form of
energy known as heat?

Kinetic energy causes disposition in the state of a substance.
For instance, heat energy on a block of ice changes it first into
water and finally into water vapor.
Describe the process that ice on Mount Everest goes through when
being heated from 10o Fahrenheit to 305o
Kelvin. Explain how the energy requirements change at different
steps of the heating curve. What are the energy transfers that
happen in the ice on Mount Everest?
How might temperature changes in the...

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