1   Chemistry  122  (General  College  Chemistry  I)-­‐  Fall  2018   Discussion  Worksheet  Week  10  (Coordinated  by  Dr.  R.  Hatfield)     Topics:  equilibrium  state  and  the  equilibrium  constant  (K),  reaction  quotient  (Q),  expressing   equilibrium  with  pressure  terms-­‐  relationship  between  Kc  and  Kp,  determining  reaction  direction,   solving  a  variety  of  equilibrium  problems,  Le  Chatelier’s  principle     Relevant  Chapters  in  Silberberg,  8e:  Chapter  17  Sections  1-­‐6,  pp.  747-­‐780.       Student  Directions:    Try  all  problems  with  your  best  effort  and  bring  your  work  to  discussion.    Use   your  text  as  a  resource  for  any  constants  or  relationships  needed.  You  will  have  to  work  ahead.   When  topics  are  completely  covered  in  lecture,  go  back  and  redo  any  problems  you  did  not   understand.    See  pages  782-­‐783  of  your  text  for  a  summary  list  of  key  equations  and  relationships.     Basic  Math:  Review  the  general  form  for  quadratic  equations  and  solving  quadratic  equations.   Mon.,  Tues.,  and  Wed.  Discussions  Only:  Complete  up  through  #5  for  credit  this  week.       1. The  reaction  for  the  formation  of  ammonia  is  shown  as:       N!(g)    +    3  H!(g)    2NH!(g)     K!=  ?     a) Write  the  equilibrium  constant  expression  (K!)  for  this  reaction.   b) One  equation  for  the  breakdown  of  ammonia  is  shown  as:       NH!(g)     ! !  N!(g)    +     ! !  H!(g)        K!’  =  ?     Manipulate  the  reaction  for  ammonia  formation,  as  necessary,  to  express  K!’  in   terms  of  K!.    (Hint:  A  summary  table  for  ways  of  writing  and  calculating  K  is  found   on  page  755  of  your  text).       c) Calculate  the  value  of  K!  at  500.  K  for  the  formation  of  ammonia  in  part  a)  using  the   following  measured  concentrations  for  the  equilibrium  mixture:  [N!]  =  3.0  x  10-­‐2  M;   [H!]  =  3.7  x  10-­‐2  M;    [NH!]  =  1.6  x  10-­‐2  M.         [1.7  x  102]   d) Next,  calculate  the  value  of  K!  for  the  formation  of  ammonia  at  500.  K.       [0.10]     e) Using  the  calculated  value  of    K!  at  500.  K  from  part  a  as  well  as  the  expression.

1. 1
Chemistry
122
(General
College
Chemistry
I)-­‐
Fall
2018
Discussion
Worksheet
Week
10
(Coordinated
by
Dr.
R.
Hatfield)
Topics:
equilibrium
state
and
the
equilibrium

2. constant
(K),
reaction
quotient
(Q),
expressing
equilibrium
with
pressure
terms-­‐
relationship
between
Kc
and
Kp,
determining
reaction
direction,
solving
a
variety
of
equilibrium
problems,
Le
Chatelier’s
principle
Relevant
Chapters
in
Silberberg,

3. 8e:
Chapter
17
Sections
1-­‐6,
pp.
747-­‐780.
Student
Directions:
Try
all
problems
with
your
best
effort
and
bring
your
work
to
discussion.
Use
your
text
as
a
resource
for

4. any
constants
or
relationships
needed.
You
will
have
to
work
ahead.
When
topics
are
completely
covered
in
lecture,
go
back
and
redo
any
problems
you
did
not
understand.
See
pages
782-­‐783
of
your

5. text
for
a
summary
list
of
key
equations
and
relationships.
Basic
Math:
Review
the
general
form
for
quadratic
equations
and
solving
quadratic
equations.
Mon.,
Tues.,
and
Wed.
Discussions
Only:
Complete
up
through
#5

6. for
credit
this
week.
1. The
reaction
for
the
formation
of
ammonia
is
shown
as:
N!(g)
+
3
H!(g)
2NH!(g)
K!=
?

7. a) Write
the
equilibrium
constant
expression
(K!)
for
this
reaction.
b) One
equation
for
the
breakdown
of
ammonia
is
shown
as:
NH!(g)
!
!
N!(g)

8. +
!
!
H!(g)
K!’
=
?
Manipulate
the
reaction
for
ammonia
formation,
as
necessary,
to
express
K!’
in
terms
of
K!.
(Hint:

9. A
summary
table
for
ways
of
writing
and
calculating
K
is
found
on
page
755
of
your
text).
c) Calculate
the
value of K!
at
500.
K
for
the
formation
of

10. ammonia
in
part
a)
using
the
following
measured
concentrations
for
the
equilibrium
mixture:
[N!]
=
3.0
x
10-­‐2
M;
[H!]
=
3.7
x
10-­‐2
M;
[NH!]
=
1.6
x
10-­‐2
M.

11. [1.7
x
102]
d) Next,
calculate
the
value
of
K!
for
the
formation
of
ammonia
at
500.
K.
[0.10]
e) Using
the
calculated
value
of
K!
at

12. 500.
K
from
part
a
as
well
as
the
expression
you
derived
for
K!’
in
part
b,
calculate
the
value
of
K!’.
[7.7
x
10-­‐2]
2

13. 2. Equilibrium
terminology.
When
solving
equilibrium
problems,
K
and
Q
are
used.
Define
Q.
When
does
K
=
Q?
3. Balance
each
of
the
following

14. examples
of
heterogeneous
equilibria
and
write
each
reaction
quotient,
Q!:
a) KNO!(s)
KNO!(s)
+
O!(g)
b) HCl(g)
+
O!(g)

15. H!O(l)
+
Cl!(g)
4. Calculate
the
value
of
the
equilibrium
constant
at
427
°C
for
the
reaction:
Na!O
(s)
+
!

16. !
O!
(g)
Na!O!(s)
Kc
=
?
[4000]
Equilibrium
constants
for
the
following
reactions
are
given
at
427
°C:
Na!O(s)

17. 2
Na(l)
+
!
!
O!(g)
Kc
=
2
x
10-­‐25
Na!O!(s)
2
Na(l)
+
O!(g)

18. Kc
=
5
x
10-­‐29
5. Phosphine
(PH!)

19. decomposes
at
higher
temperatures
as
follows:
2
PH! (�)
P!
(g)
+
3
H!
(g)
Kp
=
398
at
873
K
a) If

20. the
initial
partial
pressures
are
PPH3
=
0.0260
atm,
PP2
=
0.871
atm,
PH2
=
0.517
atm,
calculate
Qp
and
determine
which
direction
the
reaction
proceeds
in
to
reach
equilibrium.

21. [178]
b) When
a
mixture
of
PH!,
P!,
and
H!
reaches
equilibrium
at
873
K,
PP2
=
0.412
atm
and
PH2
=
0.822
atm.
Find
PPH3.

22. [0.0240
atm]
3
6. Iodine
gas
and
hydrogen
gas
are
sealed
in
a
flask
and
heated
to
600.
K.
The
initial

23. partial
pressures
of
iodine
and
hydrogen
gas
at
600.
K
before
they
react
are:
PI2
=3.00
atm
and
PH2
=2.00
atm.
No
other
reactions
take
place.
Determine
the
equilibrium
partial
pressures

24. of
I!,H!,
and
HI
at
600.
K.
[I! =
1.13
atm]
[H!
=
0.134
atm]
I!(g)
+
H!(g)
2
HI(g)
K!
=
92

25. at
600.
K
[HI
=
3.73
atm]
7. In
the
decomposition
of
hydrogen
sulfide:
2H!S(g)
2H!(g)
+
S!(g)
Kc
=
9.30
x
10-­‐8

26. at
700
°C
If
0.51
mol
H!S is
placed
in
a
3.0
liter
container,
what
is
the
equilibrium
concentration
of
H!(g)
at
700
°C?
Can
the
small
x
approximation
be

27. used
here
when
solving
for
x?
[1.8
x
10-­‐3
M]
8. The
following
reaction
is
endothermic:

28. C(s)
+
H!O(g)
CO
(g)
+
H!(�)
For
a
reaction
mixture
at
equilibrium,
how
would
the
following
changes
affect
the
equilibrium
(shift

29. right,
shift
left,
no
change)
and
the
equilibrium
concentration
of
CO
(g)
(increase,
decrease,
no
change)?
Change
Effect
of
equilibrium
Effect
on
concentration
of
CO
Decreasing
the
temperature
Adding

30. C
to
the
mixture
Adding
H!O
to
the
mixture
Adding
a
catalyst
Adding
H!
to
the
mixture
Lowering
the
volume

31. Adding
an
inert
gas
PACIFIC PALM RESORT 5
PACIFIC PALM RESORT
Name
Institution
Professor
Course
Running Head: PACIFIC PALM RESORT 1
Date
On touring pacific palm resort, I found that its one of the well
known resort in Southern California. Its 650 acres. The resort
has fabulous fireside dining overlooking celebration lake,
current spa and fitness center, and a legendary industry Hills
Golf Club featuring The Ike and the Babe championship
courses. In addition, the hotel has 292 guestrooms and suites
which are beautifully appointed and spacious, equipped with
balconies and fine interior furnishings with complementary
coffee and WIFI. Also, there is nearby four main airports and
interstate who makes going there a breeze to enjoy the, the red

32. restaurant and Bar, and the Cima Restaurant.
Rooms in the pacific Palm resort are equipped with continental
breakfast and afternoon refreshment in the Executive Lounge
accompanied by a voucher for a couple of drinks. Also, the
floor ceiling windows and balcony with mountain views with
free Wi-Fi. Within the rooms there are 40-inch flat screen TV
and user-friendly workstation ergonomic chairs.
According to the company’s management people get to know
how to multi-task, communicate and relate freely throughout in
the resort. John Semcken being a senior Vice President in this
resort is one of the owners of the same. The hardest bit of it is
to balance full time working hours while you’re a full time
student participating as a part time worker. The management
leads with fear instead of through positive encouragement. Once
an error is done by any of the employees, they are called in
front of their own team, which sounds humiliating and an
embarrassment to the employees. In this company, advancement
is a big problem since the managers has been there for decades.
Also I found that job turnover is a consistent issue though the
problem is not acknowledged.
In every hotel industry room’s division manager holds a senior
position since they are responsible for overseeing both front
office and operations undertaken in housekeeping of the resort.
According to the room’s division manager I interviewed, his
workday in the front office management included works in
reception, switchboards, reservations, concierge and night
auditor. On the side of housekeeping department, he is engaged
in laundry, linen, cleaning of the rooms any other public
location within the resort. He felt that his most important
aspect of his job position is to be able to oversee, monitor,
manage and report on the above mentioned essential
departments within the resort. It’s his duty to ensure that the
standards and quality of the resort is maintained as required by
the guests. Also, he deals with complaints launched by the
guests and ensures their comfort and safety for all who visit the
resort.

33. Within this resort, despite the advantages gained by visitors,
there is also strength and weakness that is felt by the workers.
The management is very tough on workers and hence job
turnover has been a big problem to this property. In addition,
workers are paid poorly compared to the number of hours they
work. The Rooms Division Manager affirmed that he cannot
advice a student to wish to be in the industry. The environment
may not favor students due to time compatibility and the
management strictness. He added that he had been in the same
position for decades serving in the same industry. Therefore,
this means that leadership is an issue in the property. However,
sometimes the workers feels humiliated when they do mistakes
by being called in front of their co-workers, they are allowed to
learn how to multi-task while interacting freely with each other.
Furthermore, the Rooms Division manager added that during his
service there unforgettable service experience. Despite room’s
division manager being his position, he leads with fear rather
than leading via positive enforcement. Also, the rate of job
turnover has not been of good image to the leaders since they
are aware it’s due to the poor salaries the resort offer.
Therefore, if money was no object, in regard to the manager, he
would reform the management within the property to ensure at
least employees are retained. Also he wished that rewarding
strategies could be implemented to motivate the employees for
them to feel appreciated for their effort in the hotel.
My opinion to the company was that the leaders who have been
in position for a long period should retire. This will allow
young youths to lead since they would ensure employees are not
humiliated in front of their co-workers hence eradicating the
rate of job turnover in the resort. Therefore, with these reforms
the resort’s image will be appealing and many students who
wish to work in such industry may send their applications. Also,
such changes will directly impact the services and maybe,
revenue earned from the resort will increase.
In conclusion, on interviewing the managers, I realized that the
company’s competitors is any other resort that pays their

34. employees well, that changes management by alternating them
in different positions. Also, its competitors are the companies
that retain employees and also absorb those who leave Pacific
Palm Resort. The Resort’s main experienced group is diploma
holder since the managers are of diploma level.
References
Rate, R., & Date. C.O. (2000). General Meeting Information.