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Major Examination in Thermodynamics

Total questions: 50

Worksheet time: 2hrs 40mins

Name
Class
Date
1.

What is the First Law of Thermodynamics?

a)

Energy cannot be created or destroyed; it can only change forms.

b)

Energy can be created, but it cannot be destroyed.

c)

Energy cannot be created, but it can be destroyed.

d)

Energy can be created, destroyed, or change forms.

2.

Can energy be created or destroyed?

a)

Yes

b)

No

3.

A metal spoon placed in a cup of hot cocoa will become hot to the touch. This is an example of _____.

a)

conduction

b)

convection

c)

radiation

4.

_____ is a form of energy transport consisting of electromagnetic waves traveling at the speed of light. It does not require matter to transfer heat.

a)

Conduction

b)

Convection

c)

Radiation

5.

Warm air and steam will rise above a pot of boiling water. This is an example of _____.

a)

conduction

b)

convection

c)

radiation

6.

The amount of energy required to raise the temperature of 1 gram of a substance by 1oC is known as:

a)

Specific heat capacity (C)

b)

Heat (q)

c)

Change in temperature (ΔT)

d)

Mass (m)

7.
A(n) _____________ is a device for measuring temperature.
a)
thermometer
b)
barometer
c)
anemometer
d)
psychrometer 
8.
Temperature is a measure of the...
a)
total energy in a substance
b)
total kinetic energy in a substance
c)
average potential energy in a substance
d)
average kinetic energy of molecules in a substance
9.
A slower particle has a lower energy than an identical, faster particle.
a)
True
b)
False
10.
The transfer of thermal energy between objects of different temperatures is called...
a)
temperature
b)
heat
c)
internal energy
d)
none of these
11.
When thermal energy is added to a substance, the substance's particles move:
a)
More rapidly at an increased diestance from each other.
b)
More rapidly with less distance between each other.
c)
More slowly with a greater distance between each other.
d)
More slowly with a reduced distance between each other.
12.
Thermal energy always moves:
a)
From a high temperature object to a lower temperature object.
b)
From a lower temperature object to a higher temperature object.
c)
From an object with lower kinetic energy to an object with higher kinetic energy.
d)
From an object of higher mass to an object of lower mass.
13.
The second  law of thermodynamics states that entropy of a system  tends to ______________. 
a)
increase
b)
decrease
c)
stay constant
d)
fluctuate wildly
14.
The temperature of a glass of cold water will eventually...
a)
Match the temperature of the surrounding environment.
b)
Always be colder than the surrounding environment.
c)
Become warmer than the surrounding environment.
d)
Never change temperature.
15.
Which law of thermodynamics states that absolute zero cannot be reached?
a)
1st
b)
2nd
c)
3rd
16.
The first law of thermodynamics states that energy is
a)
created
b)
destroyed
c)
conserved
d)
created and destroyed
17.

As the temperature of an abject increases, its molecules

a)

move faster

b)

get samller (condense)

c)

move farther apart (expand)

d)

move faster and farther apart (expand)

18.
Which best describes ENTROPY?
a)
Useful heat energy needed to drive an engine
b)
Heat that can be stored to be used at a later date
c)
  Random energy that escapes from the system
d)
A state of order in a physical system
19.
The first law of thermodynamics states that the change in the internal energy of a system is equal to the difference in energy transferred to or from the system as heat and
a)
mass
b)
work done
c)
force
d)
pressure
20.
Which statement is true about the ENTROPY?
a)
Entropy refers to DISORDER, the unusable energy that escapes a system.
b)
Entropy refers to the balance of temperature among two or more systems.
c)
Entropy refers to the average kinetic energy of the molecules.
d)
Entropy refers to the inability to destroy or create energy. 
21.
Rank the following samples from greatest kinetic energy of the molecules to least kinetic energy of the molecules:
a)
A > B > C > D
b)
B > A > C > D
c)
B > A > D > C
d)
D > C > B > A
22.
Two identical blocks of iron, one at 10 degrees C and the other at 20 degrees C, are put in contact. Suppose the cooler block cools to 5 degrees C and the warmer block warms to 25 degrees C. This would violate the
a)
first law of thermodynamics.
b)
second law of thermodynamics.
c)
both of the above
d)
none of the above
23.

Do molecules generally move faster at 45 C or 106 C?

a)

45 C because molecules have more energy than in 106C

b)

106 C because molecules have more energy than in 45C

c)

106 C because molecules have less energy than in 45C

d)

45C because molecules have less energy than in 106 C

24.

When you place the metal in boiling water, heat flows from the _________ to the _______.

a)

metal to the boiling water

b)

bottom of the metal to the top half of the metal

c)

bottom of the water to the top of the water

d)

boiling water to the metal

25.

DON'T RUSH, YOU HAVE TIME.

Water droplets condensing on the inside of a window on a cold day. Is this process exothermic or endothermic?

a)

Gases condense to form liquids. Gases are moving faster than liquids, the air around the window has a higher temperature/kinetic energy. Releasing energy to get water droplets, which is is Exothermic

b)

Gases condense to form liquids. Gases are moving faster than liquids, the air around the window has a higher temperature/kinetic energy. Releasing energy to get water droplets, which is is Endothermic

c)

Gases condense to form liquids. Gases particles are moving slower than liquids. Releasing energy to get water droplets, which is is Endothermic

d)

Gases condense to form liquids. Gases particles are moving slower than liquids. Releasing energy to get water droplets, which is is Exothermic

26.

DON'T RUSH, YOU HAVE TIME.

Frying an egg on a skillet. Referring to the egg, would the Enthalpy change be positive or negative?

a)

Skillet is absorbing heat energy from the egg. Absorbing energy is Endothermic. Endothermic has a positive Enthalpy

b)

Egg absorbing heat energy from the skillet. Absorbing energy is Endothermic. Endothermic has a positive Enthalpy

c)

Egg absorbing heat energy from the skillet. Releasing energy is Exothermic. Exothermic has a positive Enthalpy

d)

Egg absorbing heat energy from the skillet. Releasing energy is Exothermic. Exothermic has a negative Enthalpy

27.

Define ΔH

a)

Change in Specific Heat; Heat by one Degree Celsius

b)

Change in Temperature; the energy we calculate; Degree Celsius

c)

Change in Enthalpy; the energy/heat we calculate

d)

Change in Time; time travel

28.

Define Exothermic

a)

Energy is released; ΔH is negative; Going from Gas to Liquid, Liquid to Solid

b)

Energy is absorbed; ΔH is positive; Going from Gas to Liquid, Liquid to Solid

c)

Energy is released; ΔH is positive; Going from Solid to Liquid, Liquid to Gas

d)

Energy is absorbed; ΔH is negative; Going from Gas to Liquid, Liquid to Solid

29.

Define Endothermic

a)

Energy is absorbed; ΔH is negative; Going from Liquid to Gas, and Gas to Liquid

b)

Energy is released; ΔH is negative; Going from Solid to Liquid, and Liquid to Gas

c)

Energy is released; ΔH is positive; Going from Solid to Liquid, and Liquid to Gas

d)

Energy is absorbed; ΔH is positive; Going from Solid to Liquid, and Liquid to Gas

30.

YOU HAVE TIME!

How much energy is needed to raise the temperature of a 20.0g piece of copper from 15.0 degrees Celsius to 25.0 degrees Celsius? (The specific heat of copper is 0.385 J/g C)

a)

20 X (25-15) =70 J

b)

20 X .385 X (25-15)= 77 J

c)

20 X .385 X (15-25)= 62 J

d)

20 X .385 X (15-0)= 77 J

31.
The diagram represents which type of reaction
a)
endothermic
b)
exothermic
32.
What kind of graph is this?
a)
endothermic
b)
exothermic
33.
 How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22°C to 55°C, if the specific heat of aluminum is 0.90 J/gx°C?    
a)
297 Joules
b)
0.003 Joules
c)
297 J/gx°C
d)
0.003 J/gx°C
34.
The symbol for specific heat is .......
a)
c
b)
Q
c)
m
d)
t
35.
What  is the formula to calculate heat energy required to raise the temperature of any substance?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ½mv
d)
m=QC
36.
How many Joules of energy are required to change 10 gram of liquidwater from 20 C to 90 C?
a)
1400 J
b)
2800 J
c)
210,000 J
d)
1,400,000 J
37.
20 g of water. specific heat of water is 4.18 J/x°C.  temperature changes from 25° C to 20° C, how much heat energy (Q) moves from the water to the surroundings?
a)
418 Joules
b)
209 J
c)
83 J
d)
4.18 J
38.
The specific heat of aluminum is 0.21 J/g°C.  How much heat(Q) is released when a 10 g piece of aluminum foil is taken out of the oven and cools from 100° to 50°?
a)
105 J
b)
10.5 J
c)
1.05 J
39.
The first law of thermodynamics states that the change in the internal energy of a system is equal to the difference in energy transferred to or from the system as heat and
a)
mass
b)
work done
c)
force
d)
pressure
40.
Which best describes ENTROPY?
a)
Useful heat energy needed to drive an engine
b)
Heat that can be stored to be used at a later date
c)
  Random energy that escapes from the system
d)
A state of order in a physical system
41.
Which state of H2O  has the greatest entropy?
a)
Ice
b)
Water
c)
Vapor
42.
Which statement is true about the ENTROPY?
a)
Entropy refers to DISORDER, the unusable energy that escapes a system.
b)
Entropy refers to the balance of temperature among two or more systems.
c)
Entropy refers to the average kinetic energy of the molecules.
d)
Entropy refers to the inability to destroy or create energy. 
43.
As a system becomes more disordered, entropy
a)
remains the same
b)
increases
c)
decreases
d)
cannot be determined
44.
The first law of thermodynamics is a restatement of the
a)
Zeroth law of thermodynamics
b)
law of heat addition
c)
principle of entropy
d)
conservation of energy
45.

Which is an example of decreasing entropy in a closed system?

a)

Boiling water

b)

Freezing water

c)

Cells in a body coming together

d)

Ice melting

46.

The picture shows two completely identical mason jars. They're both filled with the same gas, only one of them has more in it (more molecules). What can you say about the pressures of both jars?

a)

P1 > P2 (greater pressure in jar 1)

b)

P1< P2 (greater pressure in jar 2)

c)

P1 = P2 (same pressure in both)

d)

There's not enough info to tell

47.
Which would have more entropy?
a)
Frozen ice cream
b)
Liquid Ice cream
48.
Rank the following samples from greatest kinetic energy of the molecules to least kinetic energy of the molecules:
a)
A > B > C > D
b)
B > A > C > D
c)
B > A > D > C
d)
D > C > B > A
49.
A slower particle has a lower energy than an identical, faster particle.
a)
True
b)
False
50.
Two identical blocks of iron, one at 10 degrees C and the other at 20 degrees C, are put in contact. Suppose the cooler block cools to 5 degrees C and the warmer block warms to 25 degrees C. This would violate the
a)
first law of thermodynamics.
b)
second law of thermodynamics.
c)
both of the above
d)
none of the above

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