Multiple Choice
Identify the
letter of the choice that best completes the statement or answers the question.


1.

The
kinetic energy of an object increases as its ____ increases. a.  gravitational
energy  c.  specific
heat  b.  potential
energy  d.  velocity     


2.

The
SI unit for energy is the ____. a.  calorie  c.  meter per second  b.  joule  d.  kilogram     


3.

According to the law of conservation of energy, the total amount of energy in the
universe ____. a.  remains constant  c.  increases  b.  changes
constantly  d.  decreases     


4.

In a
chemical change, energy can be _____. a.  created, but not destroyed  c.  either created or destroyed  b.  destroyed, but
not created  d.  neither created
nor destroyed     


5.

The
two terms below that are identical in meaning are _____. a.  calorie and
Calorie  c.  Calorie and
joule  b.  calorie and joule  d.  kilocalorie and Calorie     


6.

If
the heat of reaction is negative, the reaction is _____. a.  endothermic  c.  negative  b.  exothermic  d.  positive     


7.

A
burger contains 220 nutritional Calories. Convert this energy into joules. a.  9.2 ´ 10 J  c.  2.2 ´ 10 J  b.  9.2 ´ 10
J  d.  5.5 ´ 10 J     


8.

Rice
contains 245 nutritional Calories. Calculate the energy in joules.


9.

What
is the energy required to raise the temperature of 1 g of a substance by 1ºC or 1
K? a.  specific
heat  c.  heat
capacity  b.  heat energy  d.  enthalpy of formation     


10.

A 4.0
g sample of iron was heated from 0ºC to 20.ºC. It absorbed 35.2 J of energy as heat. What
is the specific heat of this piece of iron? a.  2816 J/(g·ºC)  c.  2.27 J/g  b.  2.27
J/(g·ºC)  d.  0.44
J/(g·ºC)     


11.

How
much energy does a copper sample absorb as energy in the form of heat if its specific heat is 0.384
J/(g·ºC), its mass is 8.00 g, and it is heated from 10.0ºC to
40.0ºC? a.  0.0016
J/(g·ºC)  c.  92.2
J  b.  0.0016
J  d.  92.2
J/(g·ºC)     


12.

Find
the specific heat of a material if a 6.0 g sample absorbs 50. J when it is heated from 30ºC to
50ºC. a.  0.60
J  c.  0.42
J  b.  0.60
J/(g·ºC)  d.  0.42
J/(g·ºC)     


13.

How
much energy is absorbed as heat by 20. g of gold when it is heated from 25ºC to 35ºC? The
specific heat of gold is 0.13 J/g·ºC. a.  26 J  c.  0.0006 J  b.  26
J/(g·ºC)  d.  0.0006
J/(g·ºC)     


14.

A 5.0
g sample of silver is heated from 0ºC to 35ºC and absorbs 42 J of energy as heat. What is
the specific heat of silver? a.  0.24 J  c.  0.74 J  b.  0.24
J/(g·ºC)  d.  0.74
J(g·ºC)     


15.

The
Greek letter D stands
for a.  "heat
stored in."  c.  "rate
of."  b.  "mass of."  d.  "change in."     


16.

What
would likely happen if you were to touch the flask in which an endothermic reaction were
occurring? a.  The flask would
probably feel cooler than before the reaction started.  b.  The flask would
probably feel warmer than before the reaction started.  c.  The flask would
feel the same as before the reaction started.  d.  none of the
above   


17.

When
energy is changed from one form to another, ____. a.  some of the energy is lost entirely  b.  all of the
energy can be accounted for  c.  a physical change occurs  d.  all of the
energy is changed to a useful form   


18.

A
process that absorbs heat is a(n) ____. a.  endothermic process  c.  exothermic process  b.  polythermic
process  d.  ectothermic
process     


19.

How
many joules are in 148 calories? (1 cal = 4.18 J) a.  6.61 J  c.  148 J  b.  35.4
J  d.  619
J     


20.

The
specific heat of silver is 0.24 . How many joules of
energy are needed to warm 4.37 g of silver from 25.0C to 27.5C? a.  2.62
J  c.  45.5
J  b.  0.14
J  d.  0.022
J     


21.

Calculate the kinetic energy in J of an electron (mass = 9.11 x 10^{28} kg)
moving at 6.00 x 10^{6} m/s. a.  4.98 x 10^{48}  d.  2.49 x 10^{48}  b.  3.28 x
10^{14}  e.  6.56 x
10^{14}  c.  1.64 x 10^{14}     


22.

The
kinetic energy of a 7.3 kg steel ball traveling at 18.0 m/s __________ J. a.  1.2 x
10^{3}  d.  1.3 x
10^{2}  b.  66  e.  7.3  c.  2.4 x 10^{3}     


23.

Calculate the kinetic energy (J) of a 150 lb jogger (68.1 kg) traveling at 12.0
mile/hr (5.36 m/s). a.  1.96 x 10^{3}  d.  183  b.  365  e.  68.1  c.  978     


24.

Determine the kinetic energy (J) of an 80.0 g bullet traveling at 300.0
m/s. a.  3.60 x
10^{6}  d.  12.0  b.  1.20 x 10^{4}  e.  80.0  c.  3.60 x 10^{3}     


25.

Work
equals force _____ distance. a.  plus  d.  divided by  b.  times  e.  combined
with  c.  minus     


26.

One
Joule equals __________. a.  1 kgm^{2}/s^{2}  d.  1 gcm/s  b.  2
kg  e.  none of
these  c.  4.184 cal     


27.

At
what velocity (m/s) must a 20.0 g object be moving in order to possess a kinetic energy of 1.00
J? a.  1.00  d.  1.00 x
10^{3}  b.  100 x 10^{2}  e.  50.0  c.  10.0     


28.

How
much kinetic energy (in J) is possessed by a 23.2 g object moving at a speed of 81.9
km/hr? a.  1900  d.  1.43 x
10^{3}  b.  77.8  e.  6.00  c.  145     


29.

At
what speed must a 35.0 mg object be moving in order to possess 1.20 J of kinetic
energy? a.  0.262
km/hr  d.  943
km/hr  b.  15.7 km/hr  e.  26.9 km/hr  c.  262
km/hr     


30.

The
first law of thermodynamics states that __________. a.  all spontaneous
processes are accompanied by an increase in disorder  b.  energy is
conserved during any process  c.  the entropy of a pure, crystalline substance at absolute zero
is zero  d.  the amount of work done during a change is independent of the
pathway of that change  e.  none of these   


31.

What
is the DE (in J) of a
system that releases 12.4 J of heat and does 4.2 J of work on the surroundings? a.  16.6  d.  16.6  b.  12.4  e.  8.2  c.  4.2     


32.

The
value of DE for a system that performs 213 kJ of work on its surroundings and loses 79 kJ of
heat is __________ kJ. a.  +292  d.  134  b.  292  e.  213  c.  +134     


33.

Calculate the value of DE (in J) for a system that loses 50 J of heat and has 150 J of work
performed on it by the surroundings. a.  50  d.  200  b.  100  e.  +200  c.  100     


34.

Which
of the following is a statement of the first law of thermodynamics? a.  Ek =
1/2mv^{2}  b.  a negative DH corresponds to an exothermic process  c.  DE = E_{final}  E_{initial}  d.  Energy lost by
the system must be gained by the surroundings.  e.  1 cal = 4.184 J
(exactly)   


35.

A
_____ q corresponds to an _____ process. a.  negative, endothermic  d.  zero, exothermic  b.  negative,
exothermic  e.  zero,
endothermic  c.  positive, exothermic     


36.

What
is the change in the internal energy (in J) of a system that absorbs 2,500 J of heat and that does
7,655 J of work on the surroundings? a.  10,155  d.  10,155  b.  5,155  e.  1.91 x
10^{7}  c.  5,155     


37.

What
is the change in the internal energy (in J) of a system that releases 2,500 J of heat and that does
7,655 J of work on the surroundings? a.  10,155  d.  10,155  b.  5,155  e.  5,155  c.  1.91 x 10^{7}     


38.

When
a sample of aluminum absorbed 9.86 J of heat, its temperature increased from 23.2°C to
30.5°C. Since the specific heat of aluminum is 0.90 J/gK, the mass of the sample was
_____ g.


39.

When
72 g of a metal at 97.0°C is added to 100.0 g of water at 25.0°C, the final temperature is
29.1°C. What is the heat capacity (in J/gK) of the metal? The specific heat of
H2O(l) is 4.18 J/gK. a.  0.46  d.  2.0  b.  2.8  e.  4.18  c.  0.35     


40.

Calculate the heat capacity (in J/gK) for metal X from the following
information. A sample of the metal (95 g) at 75.0°C is placed in 50.0 g of water at
18.0°C. The specific heat of H2O(l) is 4.18 J/gK. The final temperature of the
water is 23.0°C. a.  23  d.  3.6  b.  0.21  e.  4.2  c.  0.76     


41.

The
specific heat of copper metal is 0.38 J/gK. Assume you had a 75 g cube of copper at
25.0°C. What would the final temperature of the copper be (in °C) if it absorbed
150.0 J of heat? a.  19.7  d.  25.8  b.  5.3  e.  5.3  c.  30.3     


42.

How
much energy (in kJ) is required to raise the temperature of 500.0 g of water from 20.00°C to
20.15°C? a.  2.092  d.  0.3138  b.  331.8  e.  209.2  c.  75.00     


43.

If
73.51 J of heat were added to 25.6 g of water at 25.3°C, what would be the final temperature of
the water? a.  26.0°C  d.  13.8°C  b.  39.1°C  e.  13.8°C  c.  98.8°C     


44.

How
many grams of water can be heated from 20.0°C to 25.0°C by the addition of 324 J of
energy? a.  15.5  d.  6.78 x
10^{3}  b.  20.9  e.  387  c.  1.36 x 10^{3}     

Matching



Match the
terms below with their correct definitions. a.  system  e.  kinetic energy  b.  calorimeter  f.  potential
energy  c.  thermochemistry  g.  surroundings  d.  universe     


45.

An insulated
device used to measure the amount of heat absorbed or released during a chemical or physical
process


46.

The study of
heat changes that accompany chemical reactions and phase changes


47.

The specific
part of the universe that contains the reaction or process you wish to study


48.

A system
plus its surroundings


49.

Everything
in the universe except the system being studied


50.

energy of motion
