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Online Study Guide - Chem 2 - Energy



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 ´ 10energy_files/i0080000.jpg J
c.
2.2 ´ 10energy_files/i0080001.jpg J
b.
9.2 ´ 10energy_files/i0080002.jpg J
d.
5.5 ´ 10energy_files/i0080003.jpg J
 

 8. 

Rice contains 245 nutritional Calories. Calculate the energy in joules.
a.
energy_files/i0090000.jpg J
c.
energy_files/i0090001.jpg J
b.
energy_files/i0090002.jpg J
d.
energy_files/i0090003.jpg J
 

 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 energy_files/i0210000.jpg. How many joules of energy are needed to warm 4.37 g of silver from 25.0energy_files/i0210001.jpgC to 27.5energy_files/i0210002.jpgC?
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 106 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 103
d.
1.3 x 102
b.
66
e.
7.3
c.
2.4 x 103
 

 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 103
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 106
d.
12.0
b.
1.20 x 104
e.
80.0
c.
3.60 x 103
 

 25. 

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

 26. 

One Joule equals __________.
a.
1 kgm2/s2
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 103
b.
100 x 102
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 = 1/2mv2
b.
a negative DH corresponds to an exothermic process
c.
DE = Efinal - Einitial
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 107
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 107
 

 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/g-K, the mass of the sample was _____ g.
a.
72
d.
8.1
b.
1.5
e.
6.6
c.
65
 

 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/g-K) of the metal?  The specific heat of H2O(l) is 4.18 J/g-K.
a.
0.46
d.
2.0
b.
2.8
e.
4.18
c.
0.35
 

 40. 

Calculate the heat capacity (in J/g-K) 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/g-K.  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/g-K.  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 103
b.
20.9
e.
387
c.
1.36 x 103
 

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
 



 
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