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What is the energy in joules of a mole of photons with the energy of the 434 nm spectral line of hydrogen?
Study Guide Home work.doc

ATLANTA METROPOLITAN COLLEGE SCIENCE, MATHEMATICS AND HEALTH PROFESSION DIVISION
FALL SEMESTER 2010 GENERAL CHEMISTRY I CHEM 1211
Examination: Quiz for Chapters SEVEN AND EIGHT
Name___________________________________
Date: NOVEMBER 11, 2010
INSTRUCTIONS:
(1) Please write your name and question ID on your scantron and your worksheet for your theory and calculation problems.
(2) Please use shade True = A and False = B
(3) Answer all multiple choice questions unto your scantron sheet
(4) Answer ONLY the two bold and underlined calculation problems on your clean worksheet.
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
1)

14.0 g of
metal at
24.0 °C
has 250
joules of
heat
added to
it. The
metal's
specific
heat is
0.105 J/g
°C. What
is its final
temperatu
re?

1)

_______
A)

[(914.0)

(0.105)/250] + 24.0
B)

(14.0)

(0.105)/250
C)

[250/(14.0)

(0.105)]
D)

(250)

(14.0)/0.105
E)

none of these

2)

Which of
the
following
is NOT a
thermody
namic
function
of state?

2)

______ _
A
)

eha
nlp
t y

density
D)

volume
E)

temperature

3)

The
complete
combustio
n of
propane,
C3H8(g),
is
represente
d by the
equation:
C3H8(g)
+ 5 O2(g)
3
CO2(g) +
4 H2O(l)
ΔH° =
-2220 kJ
How
much heat
is evolved
in the
complete
combustio
n of 20.0
L
C3H8(g)
at STP?

3)

______ _
A
)

1007 kJ

B)

1982 kJ

C)

2486 kJ

D)

495 kJ

E) 9 9


Oxygen
gas at
34.5 °C is
compress
ed from
45.7 L to
34.5 L
against a
constant
pressure
of 750
mmHg.
What is
the work
done in
joules by
the
system?

4)

______ _
A
)

1 ×
. 10
13
2

9.09 × 104
D)

-9.09 × 104
E)

-1.12 × 103

5)

How
much heat
is
involved
in the
complete
combustio
n of 2.50
kg
propane,
C3H8?
ΔHcomb
= -2219
kJ/mol.

5)

______ _
A
)

5 ×
. 10
53
5kJ

503 kJ
D)

1.26 × 105 kJ
E)

49.7 kJ

6)

The
combustio
n of 90.0
g of
oxalic
acid,
C2H2O4(
s) in a
bomb
calorimet
er whose
heat
capacity
is 4.60
kJ/°C
causes the
temperatu
re to rise
from 25.0
°C to 79.6
°C. What
is the heat
of
combustio
n of
oxalic
acid?

6)

______ _
A
)

- k
2J/
5m
1ol

-54.6 kJ/mol
D)

-211 kJ/mol
E)

-21.2 kJ/mol

7)

The heat
of
combustio
n,
ΔHcomb,
of 1butene(l),
C4H8(l),
is -2696.9
kJ/mole.
From the
following
values of
ΔH°f
CO2(g) =
-393.5
kJ/mol
and ΔH°f
H2O(l) =
-285.8
kJ/mol,
calculate
the
standard
enthalpy
of
formation
of
butene(l).

7)

______ _
A
)

-2017 kJ

B)

+2017 kJ

C)

-3376 kJ

D)

-20.30 kJ

E) - 1



Given that
ΔH°f
[CO(g)] =
-110.5
kJ/mol
and ΔH°f
[COCl2(g
)] =
-219.1
kJ/mol,
what is
the
enthalpy
of
reaction
for the
formation
of
phosgene,
COCl2
from
carbon
monoxide
, CO, and
chlorine
gas,
Cl2(g)?

8)

______ _
A
)

+329.6 kJ

B)

-219.1 kJ

C)

-110.5 kJ

D)

+110.5 kJ

E) - 1



Consider
the
reaction:
4 NH3(g)
+ 5 O2(g)
4
NO2(g) +
6 H2O(l)
ΔH°f
-46.19
0.00
90.37
-285.85
kJ/mol
Compute
ΔH° for
this
reaction.

9)

______ _
A
)

-241.67 kJ

B)

-149.29 kJ

C)

-622.62 kJ

D)

-1168.9 kJ

E) 9 8

10)

Some
"beetles"
defend
themselve
s by
spraying
hot
quinone,
C6H4O2(
l), at their
enemies.
Calculate
Ho for
this
reaction.
C6H4(OH
)2(l) +
H2O2(l)

C6H4O2(
l) +
2H2O(l)
Given:
C6H4(OH
)2(l)
C6H4O2(
l) + H2(g)
+177.4 kJ
The
standard
enthalpies
of
formation
of
H2O2(l)
and
H2O(l)
are -187.4
and
-285.8
kJ/mol,
respective
ly.

10)

______
A
)

-561.6 kJ

B)

+79.00 kJ

C)

-384.2 kJ

D) - 2
11)



An
element
involved
in a
formation
reaction
as a
reactant is
NOT:

11)

______

pure
A
)

at 1.00 M

concentration
D)

at 1.00 atm

pressure
E)

none of these

12)

Calculate
the
quantity
of heat, in
kJ,
required
to raise
the
temperatu
re of a
2.15 kg
iron bar
24.0 °C
(specific
heat of
iron =
0.473 J/g
°C).

12)

______
A
)

109 kJ

B)

51.6 kJ

C)

24.4 kJ

D)

11.3 kJ

E) 2 3

13)

5.04 × 103 mole of
a
compoun
d is added
to 41.0 g
of water
in a
styrofoam
cup and
stirred
until it
dissolves.
The
temperatu
re of the
solution
changes
from
23.460 °C
to 23.420
°C. What
is the heat
of
solution
of the
compoun
d
expressed
in kJ/mol?
Assume
the
specific
heat of
the
solution is
4.18 J/g
°C.

13)

______
A
)

1 kJ/
. mo
4l

-2.8 kJ/mol
D)

2.8 kJ/mol
E)

-0.035 J/mol

14)

Determin
e the
enthalpy
change in
the
following
equation:
H2O(g)
H2(g)
+ 1/2
O2(g)
ΔH°f
H2O(l) =
-285.8
kJ/mol

14)

______
A
)

13.4 kJ

B)

285.8 kJ

C)

-241.8 kJ

D)

-285.8 kJ

E) 2 4

TRUE/FA
LSE.
Write 'T'
if the
statement
is true and
'F' if the
statement
is false.
15)

The
maximum
amount of
work is
provided
by a
reversible
process
because
equilibriu
m
between
the
system
and the
surroundi
ngs is
always
maintaine
d.

15)

______

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the
question.
16)

The two
things that
can
change
the
internal
energy of
a system
by their
absorptio
n are
work and:

16)

______

m
ass
A
)

pressure
D)

color
E)

none of these

TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false.
17)

An
expansion
of gas by
a system
means
that the
internal
energy of
the
system
increases.

17)

______

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the
question.
18)

Oxygen
gas at
34.5 °C
expands
from 34.5
L to 45.7
L against
a constant
pressure
of 750
mmHg.
What is
the work
done in
joules by
the
system?

18)

______
A
)

- 9 ×
910
. 4
0

4.55 × 103
D)

-1.12 × 103
E)

9.09 × 104

19)

The heat
of
combustio
n of
methane
is -50.38
kJ/mol.
How
many
moles of
methane
must be
burned to
produce
137 kJ of
heat?

19)

______

2.72
A
)

0.367
D)

1.37
E)

none of these

20)

Lead,
water,
sulfur,
and
arsenic
have
specific
heats of
0.128,
4.18,
0.706, and
0.329 J g1 oC-1,
respective
ly. Which
of the
following
would
need the
smallest
quantity
of heat to
change
the
temperatu
re of 5 g
by 10oC?

20)

______
A
)

arsenic

B)

lead

C)

sulfur

D) w a

21)

What is
the
reaction
for the
standard
enthalpy
of
formation
for
CdSO4(s)
? (Cd(s) is
the stable
form of
cadmium.
)

21)

______
A
)

C2
H
dSO
( (a
4
N
q)
O

32
) HN
2O3
( (aq
a) +
qCd
) SO
4(s
+)

CdO(s) +

SO3(l) CdSO4(s)
D)

Cd2+ (aq) + 2 SO42- CdSO4(s)
E)

none of these

22)

What is
the
reaction
for the
standard
enthalpy
of
formation
for
HCl(g)?

22)

______
A
)

I 2H
C (g
3
l )
3
( HI(
gg)
) + 3
HC
+l(g)

1/2 H2(g) +

Cl2(g) HCl(g)
D)

NH3(g) +

Cl2(g) NH2Cl(g) + HCl(g)
E)

none of these

23)

Using the
heat of
combustio
n of
methanol
as -726.6
kJ and the
following
data:
C(graph)
+ 1/2O2

CO(g)
ΔH°
= -110.5
kJ
C(graph)
+ O2(g)

CO2(g)
ΔH°
= -393.5
kJ
H2(g)
+
1/2O2(g)

H2O(l)
ΔH°
= -285.8
kJ
Determin
e ΔH° for
the
following
reaction:
CO(g) + 2
H2(g)
CH3OH(l
)

23)

______
A
)

-157.8 kJ

B)

-128 kJ

C)

157.8 kJ

D)

-349 kJ

E) 1 2

24)

Choose
the
INCORR
ECT
statement.

24)

______
A
)

P en
oerg
t y is
eene
nrgy
t in
i acti
aon.
l

Heat moves

from a warmer body to a colder one.
D)

Kinetic energy is the energy of motion.
E)

Heat is energy transferred as a result of a temperature difference.

SHORT ANSWER. Write the word or phrase that best completes each statement or answers the question.
25)

The
standard
heat of
formation
of solid
ammoniu
m
bromide
is -270.8
kJ/mol.
Write the
chemical
equation
for the
reaction
to which
this value
applies.

25)

______ _______

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or
answers the question.
26
)

The four
quantum
numbers
of the
LAST
electron
to be
placed
into a Ca
atom are:

26)

______
A
)

n=
1,
=m
=
40,
, ms
=
-1/
2

n = 4, = 0, m = 0, ms = -1/2
D)

n = 4, = 1, m = 0, ms = +1/2
E)

none of these

27)

Choose
the
INCORR
ECT
statement
concernin
g
electroma
gnetic
radiation.

27)

______
A
)

A
00
An
pgst
hro
oms
t has
oone
n hal
f as
w
i mu
t ch
hene
rgy
aas
a
ph
w
aoto
vn
ewit
l h a
ewa
nvel
geng
t th
hof
25
o00
f An
gst
5ro
0ms.

The greater the frequency of the electromagnetic radiation, the greater the energy of the radiation.
D)

The speed of ultraviolet light rays is faster than x-rays in a vacuum.
E)

Infrared light

28)

has a longer wavelength than ultraviolet light.

When an
electron
goes from
a high
energy
state to a
low one,
what
occurs?

28)

______
A
)

T
om
hmo
eves
fast
aer.
t

Light is given off.
D)

This process is not possible.
E)

none of these

29)

Use the
spdf
notation
to write
out the
complete
electron
configurat
ion of Br.

29)

______
A
)

[ 3d
K
10
r2
4s
4p

4

[Ar] 3d94s24p6
D)

[Ar]

3d104p65s2
E)

[Ar] 4s24p24d9

30)

How
many
unpaired
electrons
are in the
ground
state
electron
configurat
ion of
calcium?

30)

______
A
)

2

B)

5

C)

3

D)

1

E) 0

31)

Write the
appropriat
e values
of n and
for the
orbital
designatio
n 3s.

31)

______
A
)

n=
3,
= 1

n = 0, = 3
D)

n = 3, = 0
E)

n = 3, = 2

32)

A
radiation
detector
exposed
to
sunlight
records
the
energy
falling on
a given
area each
unit time.
If such a
detector
has a
reading of
0.698 cal
cm-2 min1, how
many
photons
of
sunlight
are
striking
each cm2
in one
minute?
Assume
the
average
wavelengt
h of
sunlight is
460. nm.
(4.184 J =
1 calorie)

32)

______
A
)

12 ×
. 10
618

4.32 × 1019
D)

9.63 × 1019
E)

6.76 × 1018

33)

Which of
the
following
statement
s
concernin
g
quantum
numbers
is NOT
correct?

33)

______
A
)

"ien
tati
m
"on
of
dan
eorb
nital
owit
t h
eres
spec
t to
othe
r oth
ers.

The four

quantum numbers are derived from wave mechanics.
D)

"n" relates the most probable distance from the nucleus.
E)

"l" denotes

34)

geometric shape.

Use the
Balmer
equation
to
determine
n for the
spectral
line of
wavelengt
h 434 nm.

34)

______
A
)

7

B)

3

C)

5

D)

6

E) 4

35)

Which of
the
following
is NOT
true of a
wave
function
as
suggested
by Erwin
Schroding
er?

35)

______
A
)

I ma
t the
ma
i tica
sl
equ
aati
on.

It is denoted by psi (Ψ).
D)

It can describe any particle with wavelike motions.
E)

It corresponds to a standing wave within the boundary of the system.

36)

What is
the
energy in
joules of
the 656
nm
spectral
line of
hydrogen.

36)

______
A
)

1 ×
. 10448
5J

1.30 × 10-22 J
D)

3.03 × 10-28 J
E)

4.35 × 10-31 J

37)

Calculate
the
energy in
kJ/mol of
light with
a
wavelengt
h of 360
nm.

37)

______
A
)

02
. kJ/
3mo
3l

6.63 × 103

kJ/mol
D)

332 kJ/mol
E)

5.52 × 10-19

38)

kJ/mol

What is
the
wavelengt
h
associated
with
electrons
traveling
at one
onehundredth
the speed
of light?

38)

______
A
)

42
1nm

243 nm
D)

12.5 nm
E)

7.98 × 10-2 nm

39)

The
existence
of
discrete
(quantize
d) energy
levels in
an atom
may be
inferred
from:

39)

______
A
)

es
xon
pthe
eph
r oto
i ele
m
ctri
ec
neff
t ect

x-ray

diffraction by crystals
D)

atomic line

spectra
E)

visible spectrum

40)

The fact
that the
valence
orbital
configurat
ion of
nitrogen
in the
ground
state is
2s2,
2px12py1
2pz1 is an
illustratio
n of:

40)

______
A
)

t i
hEx
eclu
sio
Pn
aPri
unci
l ple

the Bohr

Theory
D)

the Aufbau

Principle
E)

the Heisenberg Uncertainty Principle

41)

What is
an
acceptabl
e value
for the
missing
quantum
number?
n
= 4, = 2,
m = 0,
ms = ?

41)

______
A
)

3/2

B)

0

C)

2

D)

1/2

E) 1

42)

Which of
the
following
subshells
is
correctly
designate
d?

42)

______
A
)

2p6

B)

1p5

C)

3f2

D)

3s3

E) 4 d
43)



What is
the
energy in
joules of
a mole of
photons
with the
energy of
the 434
nm
spectral
line of
hydrogen
?

43)

______
A
)

26 ×
. 1074 J

5.78 × 10-25 J
D)

434 J
E)

9.21 × 10-4 J

44)

How
many
photons
of light
with
frequency
5.50 ×
1015 Hz
are
required
to provide
1 kJ of
energy?

44)

______
A
)

3 10
. -16
6ph
4oto
ns
×

2.74 × 1020

photons
D)

4.56 × 10-4

photons
E)

3.64 × 10-18

45)

photons

What is
the
wavelengt
h of the
line in the
Balmer
series of
hydrogen
correspon
ding to
the
transition
from n =
5 to n =
2? The
constant
for
Balmer's
equation
is 3.2881
× 1015 s1.

45)

______
A
)

535 nm

B)

304 nm

C)

30.4 nm

D)

329 nm

E) 4 3

46)

The
relationsh
ip
between
the
frequency
of light
and the
energy of
the light
was
postulated
by:

46)

______
A
)

R
rt
oBu
bnse
en

Max Planck
D)

Albert Einstein
E)

Johannes

Rydberg


47)

Exception
s to
________
are
represente
d by
chromium
and
copper in
the 4th
row of the
periodic
table.

47)

______
A
)

H
d's
uRul
ne

the Bohr

Theory
D)

the Heisenberg Principle
E)

the Aufbau

48)

Principle

The
ground
state
electron
configurat
ion for
antimony
is:

48)

______
A
)

[ 5s2
Kd
5
r 10
5p

3

[Xe]

5s25d105p3
D)

[Xe]

5s24d105p2
E)

[Kr]

4d105s25p3

49)

What is
the orbital
designatio
n for the
quantum
numbers
n = 2, l =
1?

49)

______
A
)

2d

B)

3s

C)

3p

D)

2p

E) 2 s
50)



Which of
the
following
is NOT
true about
zero-point
energy?

50)

______
A
)

I ow
t est
ene
i rgy
sval
ue
t of
ha
epar
ticl
l e.

Because the

zero point energy is not zero, the particle can not be at rest.
D)

energy corresponds to n = 1.

Zero point
E)

It's value can be zero.

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