Download Unit 10 Exam - Sharp Honors Chemistry Multiple Choice Identify the

Unit 10 Exam - Sharp Honors Chemistry
Multiple Choice
Identify the choice that best completes the statement or answers the question.
1.
The amount of energy needed to heat 2.00 g mercury from 50.0°C to 85.0°C is 9.87 J. The specific heat
capacity of this sample of mercury is
a. 0.141 J/g·°C b. 0.058 J/g·°C c. 0.282 J/g·°C d. 345 J/g·°C e. 691 J/g·°C
2.
A 4.60-g sample of iron is heated from 47.0°C to 75.0°C. The amount of energy required is 57.96 J. The
specific heat capacity of this sample of iron is
a. 0.450 J/g·°C b. 1.233 J/g·°C c. 2.07 J/g·°C d. 1623 J/g·°C e. 7465 J/g·°C
3.
A 6.75-g sample of gold (specific heat capacity = 0.130 J/g °C) is heated using 55.8 J of energy. If the
original temperature of the gold is 25.0°C, what is its final temperature?
a. 88.6 °C b. 38.6 °C c. 76.9 °C d. 73.6 °C e. 63.6 °C
4.
Heat is typically measured in
a. °C b. °F c. joules d. grams
5.
SI units for specific heat capacity are
a. cal b. cal/g c. J/g·°C d. g/mL
6.
e. g·°C/cal
How many joules of energy would be required to heat 15.9 g of carbon from 23.6°C to 54.2°C? (Specific
heat capacity of carbon = 0.71 J/g·°C.)
a.
b.
c.
e. none of
d.
these
7.
Calculate
given the following information:
a. 17 kJ b. 65 kJ c. –65 kJ d. –17 kJ e. 1.7 kJ
8.
A system absorbs 159 kJ of heat, and performs 89 kJ of work on the surroundings. What is
system?
a. 248 kJ b. –248 kJ c. 70 kJ d. –70 kJ e. 1.8 kJ
9.
2116.16 J of energy is equivalent to how many calories?
b. 0.505774
a.
10.
12.
cal
d. 2120.34
J
c. 1.33
b.
J
d. 0.754 J
cal
e. 505.774
cal
e.
Perform the indicated conversion:
7.079 kcal  ____ kJ
a. 29.62
kJ
kJ
b. 1.692
kJ
c. 0.5910
d.
e.
Perform the indicated conversion:
a. 686
13.
c. 2.11616
5.55 kcal of energy is equivalent to how many joules?
a. 23.2
11.
cal
of the
J
b.
c. 12.0
J
d.
e.
Determine the enthalpy change when 19.4 g of carbon is reacted with oxygen according to the reaction
a. 636
kJ
b.
c. –636
kJ
d. –7.64
kJ
e. 6.76 kJ
14.
For the reaction
Calculate the enthalpy change when 4.73 g of hydrogen gas is reacted with excess oxygen.
a. –60.5
kJ
b. 671
kJ
c. –671
kJ
d.
e. –
15.
A 100.0 g sample of water at 27.0°C is poured into a 77.4 g sample of water at 89.0°C. What will be the
final temperature of the water?
a. 88.7°C b. 424°C c. 23.6°C d. 185°C e. 54.1°C
16.
A 51.1-g sample of aluminum at 95.0°C is dropped into 35.0 g of water at 40.0°C. What is the final
temperature of the mixture? (specific heat capacity of aluminum = 0.89 J/g°C; specific heat capacity of
water = 4.184 J/g°C)
a. 53°C b. –8.0°C c. 101°C d. 24°C e. –15°C
17.
The specific heat capacity of gold is 0.13 J/g°C. How many calories of energy are needed to warm
0.570 g of gold from 30.0°C to 39.5°C?
a. 0.70 cal b. 0.17 cal c. 1.2 cal d. 2.9 cal e. 23 cal
18.
Which of the following processes is endothermic?
a. water droplets condensing on a soda can on a hot summer day b. an ice pack getting cold (due to
ammonium nitrate dissolving in water inside the pack) c. thermite reaction between iron(III) oxide and
aluminum (spectacular flames are observed) d. freezing water to make ice cubes e. none of the above
are endothermic processes
19.
Which of the following processes is exothermic?
a. rolling a ball up a hill b. boiling water in a beaker to make steam c. allowing meat to thaw after
taking it out of the freezer d. reacting hydrogen and oxygen gases to make water e. a popsicle melting
on a warm summer day
20.
____ is the ability to do work or produce heat.
a. Gravity b. Temperature c. Radiation d. Matter
e. Energy
21.
____ is a measure of the random motions of the components of a substance.
a. Heat b. Temperature c. Energy d. Radiation e. Matter
22.
____ is a flow of energy due to a temperature difference.
a. Heat b. Radiation c. Matter d. Gravity e. Work
23.
The first law of ____ states that the energy of the universe is constant.
a. matter b. mass c. thermodynamics d. motion e. energy
24.
In the equation
, the q represents
a. work b. change in energy c. moles of a substance
25.
d. mass
of a substance
e. heat
On a cold winter day, a steel metal fence post feels colder than a wooden fence post of identical size
because
a. the
specific heat capacity of steel is higher than the specific heat capacity of wood. b. the specific
heat capacity of steel is lower than the specific heat capacity of wood. c. steel has the ability to resist a
temperature change better than wood. d. the mass of steel is less than wood, so it loses heat faster.
e. Two of the above statements are true.
26.
____ is a measure of disorder or randomness.
a. Entropy b. Enthalpy c. Calorimetry d. Internal energy
e. Hess's
law
True/False
Indicate whether the statement is true or false. Mark “A” for TRUE and “C” for FALSE.
27.
True or false? The law of conservation of energy states that energy can be converted from one form to
another but can be neither created nor destroyed.
a. True
28.
True or false? Energy can be classified as either potential or kinetic energy.
a. True
29.
b. False
True or false? The energy gained by the surroundings must be equal to the energy lost by the system.
a. True
30.
b. False
b. False
True or false? The calorie is defined as the amount of energy (heat) required to raise the temperature of
one gram of water by one degree Celsius.
a. True
b. False
Unit 10 Exam - Sharp Honors Chemistry
Answer Section
MULTIPLE CHOICE
1. ANS:
KEY:
2. ANS:
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3. ANS:
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4. ANS:
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5. ANS:
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KEY:
21. ANS:
KEY:
22. ANS:
KEY:
23. ANS:
KEY:
24. ANS:
A
PTS: 1
DIF:
calorimetry | specific heat
MSC:
A
PTS: 1
DIF:
calorimetry | specific heat
MSC:
A
PTS: 1
DIF:
heat | heat of reaction
MSC:
C
PTS: 1
DIF:
heat
MSC: general chemistry
C
PTS: 1
DIF:
calorimetry | specific heat
MSC:
A
PTS: 1
DIF:
heat | heat of reaction
MSC:
B
PTS: 1
DIF:
energy | internal energy
MSC:
C
PTS: 1
DIF:
energy | internal energy
MSC:
E
PTS: 1
DIF:
calorimetry | measuring heats of reaction
E
PTS: 1
DIF:
calorimetry | measuring heats of reaction
A
PTS: 1
DIF:
calorimetry | measuring heats of reaction
B
PTS: 1
DIF:
calorimetry | measuring heats of reaction
C
PTS: 1
DIF:
heat | measuring heats of reaction
MSC:
C
PTS: 1
DIF:
heat | measuring heats of reaction
MSC:
E
PTS: 1
DIF:
calorimetry | heat capacity
MSC:
A
PTS: 1
DIF:
calorimetry | specific heat
MSC:
B
PTS: 1
DIF:
calorimetry | heat of reaction
MSC:
B
PTS: 1
DIF:
heat | heat of reaction
MSC:
D
PTS: 1
DIF:
heat | heat of reaction
MSC:
E
PTS: 1
DIF:
first law of thermodynamics
MSC:
B
PTS: 1
DIF:
si unit | temperature
MSC:
A
PTS: 1
DIF:
heat | heat of reaction
MSC:
C
PTS: 1
DIF:
first law of thermodynamics
MSC:
E
PTS: 1
DIF:
moderate
TOP:
general chemistry
moderate
TOP:
general chemistry
moderate
TOP:
general chemistry
easy
TOP:
thermochemistry | heats of reaction
easy
TOP:
general chemistry
moderate
TOP:
general chemistry
easy
TOP:
general chemistry
easy
TOP:
general chemistry
easy
TOP:
MSC:
easy
TOP:
MSC:
easy
TOP:
MSC:
easy
TOP:
MSC:
moderate
TOP:
general chemistry
moderate
TOP:
general chemistry
difficult
TOP:
general chemistry
difficult
TOP:
general chemistry
moderate
TOP:
general chemistry
easy
TOP:
general chemistry
easy
TOP:
general chemistry
easy
TOP:
general chemistry
easy
TOP:
general chemistry
easy
TOP:
general chemistry
easy
TOP:
general chemistry
easy
TOP:
thermochemistry | heats of reaction
thermochemistry | heats of reaction
thermochemistry | heats of reaction
thermochemistry | heats of reaction
thermochemistry | heats of reaction
thermochemistry | heats of reaction
thermochemistry | heats of reaction
thermochemistry | heats of reaction
general chemistry
thermochemistry | heats of reaction
general chemistry
thermochemistry | heats of reaction
general chemistry
thermochemistry | heats of reaction
general chemistry
thermochemistry | heats of reaction
thermochemistry | heats of reaction
thermochemistry | heats of reaction
thermochemistry | heats of reaction
thermochemistry | heats of reaction
thermochemistry | heats of reaction
thermochemistry | heats of reaction
thermochemistry | thermodynamics
general concepts | measurement
thermochemistry | heats of reaction
thermochemistry | thermodynamics
thermochemistry | heats of reaction
KEY:
25. ANS:
KEY:
26. ANS:
KEY:
energy | internal energy
MSC:
B
PTS: 1
DIF:
calorimetry | specific heat
MSC:
A
PTS: 1
DIF:
second law of thermodynamics | entropy
general chemistry
easy
TOP: thermochemistry | heats of reaction
general chemistry
easy
TOP: thermochemistry | thermodynamics
MSC: general chemistry
T
PTS: 1
energy | law of conservation of energy
T
PTS: 1
energy | kinetic energy
T
PTS: 1
first law of thermodynamics
T
PTS: 1
energy | kinetic energy
easy
TOP:
general chemistry
easy
TOP:
general chemistry
easy
TOP:
general chemistry
easy
TOP:
general chemistry
TRUE/FALSE
27. ANS:
KEY:
28. ANS:
KEY:
29. ANS:
KEY:
30. ANS:
KEY:
DIF:
MSC:
DIF:
MSC:
DIF:
MSC:
DIF:
MSC:
thermochemistry | heats of reaction
thermochemistry | heats of reaction
thermochemistry | thermodynamics
thermochemistry | heats of reaction