ch4ptest - CH201
SI:
CHAPTER
4
PRACTICE
TEST


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Unformatted text preview: CH201
SI:
CHAPTER
4
PRACTICE
TEST
 For
the
following
reaction
at
298K:
 2NO2(g)
 
N2O4(g)
 1.
Determine
the
standard
enthalpy
and
standard
entropy
for
the
reaction
from
 tabulated
values.
 
 
 
 
 ΔH0
=
 ______________
kJ
 ΔS
0
=
 ___________
J*K‐1
 2.
Use
standard
enthalpy
of
reaction
and
standard
entropy
of
reaction
to
determine
 the
standard
free
energy
of
the
reaction.

Find
Keq
for
the
reaction.
 
 
 
 
 
 ΔG
0
=
______________
kJ
 Keq
=
_________________
 3.
Circle
All
correct
statements
about
this
reaction:
 
 
 
 
 
 
 
 a.
The
reaction
is
exothermic.
 b.
The
free
energy
of
the
products
is
greater
than
the
reactants.
 c.
As
temperature
increases
the
reaction
becomes
less
extensive.
 d.
As
temperature
decreases
Keq
decreases.
 e.
At
298K
equilibrium
favors
products.
 f.
All
of
the
above
statements
are
incorrect.
 4.
Determine
Q
for
this
reaction
if
PNO2
=
0.24
atm
and
PN2O4
=
1.73
atm.
 
 
 
 Q
=
________________
 
 5.
Determine
ΔG
for
the
reaction
from
#4.
 
 
 
 ΔG
=
____________
kJ
 
 6.
Circle
the
correct
answer.

This
reaction
is
spontaneous
to
the:
 
 LEFT
 
 /
 RIGHT

 
 7.
See
previously
emailed
practice
test.
 8.
Determine
the
equilibrium
pressures
of
NO2
and
N2O4
at
equilibrium
for
the
 reaction
from
#4.
(This
type
of
problem
will
be
covered
in
Chapter
5,
but
I’ve
 included
it
here
for
completeness.

After
we
cover
Chapter
5
material
look
back
over
 this
problem
and
see
how
it
fits
into
the
‘scheme’
of
this
worksheet)
 
 
 
 
 
 PNO2
=
__________
atm
 PN2O4
=
__________
atm
 /
 NEITHER
 ...
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This note was uploaded on 01/27/2011 for the course CHEM 201 taught by Professor Wilson during the Spring '10 term at N.C. Central.

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