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,

=mℓ

=

40,

, ms

=

ℓ-1/

2

n = 4, ℓ = 0, mℓ = 0, ms = -1/2

D)

n = 4, ℓ = 1, mℓ = 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 ℓ

for the

orbital

designatio

n 3s.

31)

______

A

)

n=

3, ℓ

= 1

n = 0, ℓ = 3

D)

n = 3, ℓ = 0

E)

n = 3, ℓ = 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, ℓ = 2,

mℓ = 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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