Unformatted Attachment Preview
CHMY 373 2019 – Problem Set 3
Due: Friday Feb. 1
Reminder: See previous problem sets and/or the syllabus for rules regarding problem sets.
Reading: Chapter 19.7‐19.12, Simon & McQuarrie
1. What’s the difference between and ? Does it make a big difference whether our
device for measuring heat capacity a “calorimeter” is isobaric or isochoric?
a. Derive the difference between and
∆
starting from the
expression for the definition of enthalpy:
Hint: the result you are looking for has the form:
∆
where , , and are measurable variables of state from the subset
and both calorimeters are “closed” systems.
, ,
b. Using the expression derived above, find ∆ for an ideal gas.
c. Rearrange the expression derived in part a to obtain a much simpler general
expression in terms of the isothermal compressibility, , and the coefficient
of thermal expansion, , which we have previously defined as:
1
,
1
,
d. Write the expression derived in part c in intensive form as ∆
per mole .
2. Joule‐Thomson Inversion: real gases exhibit two distinct regions in their phase
diagram corresponding to different heat transfer effects upon Joule‐Thomson
expansion which we have seen is an “isenthalpic” or constant enthalpy process .
, determines this behavior: when
is
The sign of the Joule‐Thomson coefficient,
positive, cooling occurs upon expansion. This is the effect we are most familiar with,
and almost all gases exhibit cooling upon expansion at ambient temperature.
However, at very high temperatures for most gases ,
is negative, and heating
occurs upon expansion. The temperature at which this property changes is the
Joule‐Thomson inversion temperature, .
For a van der Waals gas, the Joule‐Thomson coefficient turns out to be:
2
2
a. Assume the isobaric heat capacity is independent of temperature. Derive an
expression for the Joule‐Thomson inversion temperature, , of a van der
Waals gas.
b. Simplify the inversion temperature derived in part a by assuming the system
to be in the “dilute limit.”
c. Determine the Joule‐Thomson inversion temperature in K for argon using
the van der Waals equation of state.
d. Will argon undergo heating or cooling if expanded isenthalpically at room
temperature?
e. Determine the Joule‐Thomson inversion temperature in K for helium using
the van der Waals equation of state.
f. Will helium undergo heating or cooling if expanded isenthalpically at room
temperature?
g. A brand new high‐pressure hydrogen gas cylinder filled to 200 bar has just
been delivered to your laboratory to replace the empty one, but someone
forgot to note which cylinder was empty and both now stand side by side and
look identical. Upon lifting the two cylinders, it’s too hard to tell which is the
full one and which is empty. Is it safe to quickly open the valve referred to as
the “packing nut” at the top of both cylinders without attaching a regulator
to see which is full? In other words, if isenthalpic expansion is assumed, will a
temperature difference ≫20 °C occur we usually start to feel burns at above
~45 °C or below ~‐60°C in the case of the full cylinder?
3. Calculate the average bond enthalpy in units of kJ mol
of the Si H bonds in
disilane gas Si H from the following data provided in units of kcal mol :
‐
‐
‐
‐
‐
‐
the standard molar enthalpy of combustion of Si H gas to 2 SiO2 solid and
liquid water is ‐637.23 kcal mol
the standard enthalpy of formation of SiO solid is ‐205.00 kcal mol
the standard enthalpy of formation of H O liquid is ‐68.32 kcal mol
Si → Si
∆ ○,
88.04 kcal mol
H
→H
∆
○
,
52.09 kcal mol
the bond enthalpy of the Si Si bond in disilane is 24.38 kcal mol
4. The standard enthalpies of combustion of ethanol liquid and methyl ether liquid
at 25 °C are ‐1235 kJ mol and ‐1247 kJ mol , respectively. Determine the
isomerization enthalpy ∆ ○ ,
for the following reaction:
CH OCH
→ CH CH OH
5. A 1.00 g sample of liquid benzene, C H , is burned in pure oxygen in a “Parr bomb
calorimeter” a closed, rigid calorimeter . The initial temperature is 25 °C and the
observed temperature increase is 1.681 °C. The heat capacity of the calorimeter
assembly heavy metal components is known to be 23.80 kJ K . Assuming ideal
gas behavior of the reaction products, find:
per mole and per gram of liquid benzene, and
a. Δ
b. Δ
per mole and per gram of liquid benzene.
c. Comment on the significance of the difference between Δ and Δ in this
experiment.