Back Questions on Heat, Temperature, and Calorimetery
1.
A temperature scale based on human body temperature and an Ammonium Chloride solution
was first developed by
a) Anders Celsius.
b) Lord Kelvin.
2.
Fahrenheit's original temperature scale was based on
a)
b)
c)
d)
3.
c) Gabriel Fahrenheit.
d) Benjamin Thompson.
the boiling and freezing points of water.
the boiling and freezing points of Ammonium Chloride.
the freezing point of an Ammonium Chloride solution and human body temperature.
the boiling point of water and the freezing point of an Ammonium Chloride solution.
A popular science fiction book is Fahrenheit 451 by Ray Bradbury. The title refers to the
(Fahrenheit) temperature at which paper burns (451F). If Mr. Bradbury were writing in the
Celsius scale, the name of the book would be
a) Celsius 451
b) Celsius 724
4.
c) Celsius 233
d) Celsius 178
In degrees Fahrenheit, absolute zero would be
a) 273.15F.
b) 459.67F.
5.
The amount of heat necessary to melt one gram of a certain substance (at its melting point) is
generally _________ the amount of heat necessary to boil one gram of the same substance (at
its boiling point).
a) greater than
6.
b) less than
c) equal to
The amount of heat necessary to change one gram of a liquid into one gram of a gas is the
a) heat of condensation.
b) heat of vaporization.
7.
c) 0F.
d) 25.6F.
c) heat of boiling.
d) inverse heat of fusion.
The amount of heat necessary to melt one gram of a substance is known as the
a) heat of sublimation.
b) heat of fusion.
c) heat of regelation.
d) heat of condensation.
8.
The amount of heat necessary to raise the temperature one unit mass of a substance by one
degree is the
a) specific heat.
b) heat of vaporization.
9.
The amount of heat that must be removed from one gram of a gas so that it condenses into one
gram of a liquid is the
a) specific heat.
b) heat of vaporization.
10.
melt one gram of ice.
raise the temperature of one gram of water one degree Centigrade.
increase the vapor pressure of one gram of water by one Torr.
the difference between water's heat of vaporization and heat of fusion.
80 calories of heat are added to 5 grams of water at 40 C. The final temperature of the water is
a) 45 C.
b) 56 C.
12.
c) 47.0 C.
d) 76.7 C.
The amount of heat necessary to boil 40 grams of liquid water at 100 C would melt
_______ grams of ice at 0 C.
a) 270
b) 100
14.
c) 120 C.
d) 80 C.
If the material in the previous question had been Beryllium (c = 0.436 cal/g C) instead of
water, the final temperature would have been
a) 45 C.
b) 92.7 C.
13.
c) heat of fusion.
d) heat of condensation.
The specific heat of water is defined as the amount of heat necessary to
a)
b)
c)
d)
11.
c) heat of fusion.
d) heat of sublimation.
c) 40
d) 140
40 calories of heat is added to 2 grams of water at 30 C. The final temperature of the water is
a) 70 C.
b) 50 C.
c) 32 C.
d) 10 C.
15.
If, in the previous question, we have 2 grams of Aluminum (cAl = 0.215 cal/g C) instead of 2
grams of water, the final temperature of the Al will be
a) 70 C.
b) 63.0 C.
16.
The amount of heat necessary to melt 40 grams of ice will raise the temperature of how much
water from 25 C to 45 C?
a) 160 grams.
b) 800 grams.
17.
c) a high melting point.
d) a high boiling point.
In the northern hemisphere's mid-latitude temperate zone, a large body of water to the west
generally results in
a) awful weather.
b) tornadoes.
21.
c) 200 calories
d) 217 calories
Compared to most metals, water has
a) a rather large specific heat.
b) a rather small specific heat.
20.
c) 20 calories
d) 200 calories
What quantity of heat must be removed from 20 g of aluminum (c = 0.217 cal/g C) in order
to reduce its temperature from 50 C to 40 C?
a) 43.4 calories
b) 921.7 calories
19.
c) 1080 grams
d) There is not enough information.
What quantity of heat must be removed from 20 g of water in order to reduce its temperature from 50 C to 40 C?
a) 2 calories
b) 20 B.T.U.'s
18.
c) 123.0 C.
d) 895.3 C.
c) the Coriolis force.
d) moderate weather.
The concept of a “sea breeze” can be explained using
a) the relatively high specific heat of water.
b) the relatively low specific heat of water.
c) the heat of regelation of water.
d) Friday afternoon happy hours.
22.
Water’s overall moderating influence on climate can be seen in
a) San Francisco, CA.
b) Bermuda.
23.
c) Northern Europe.
d) all of the above.
If the earth spun on its axis in the opposite direction, which of these pairs of U.S. cities would
be most likely to change climates:
a) New York City and Orlando, FA
b) New York City and San Francisco, CA
c) Orlando, FA and San Francisco, CA
d) (b) and (c) but not (a).
e) none of the above.
Answer Key:
1. C
2. C
3. C
4. B
5. B
6. B
7. B
8. A
9. B
10. B
11. B
12. D
13. A
14. B
15. C
16. A
17. D
18. A
19. A
20. D
21. A
22. D
23. B (think carefully about why
C doesn’t work as well!)
Back Short Answer Questions on Heat, Temperature and Calorimetry
1.
How much energy is necessary to change 30 grams of ice at 30 C to steam at 140 C? Take
cice = 0.55 cal/g C and csteam = 0.50 cal/g C. (Ans. 22695 cal)
2.
100 grams of ice at 10 C is added to 200 grams of water at 50 C. What is the final temperature of the mixture? Take cice = 0.55 cal/g C. (Hint: what has to be done to the ice before it
will melt??) Two extra points if your final answer is in Kelvins instead of C. (Ans 4.83C =
278 K)
3.
The specific heat of solid aluminum (Al) is 0.215 cal/g C; the heat of fusion of Al is
94.8 cal/g; and the melting point of Al is 660 C. How much heat energy is required to take
100 grams of Al at room temperature (you are responsible for defining a “reasonable” room
temperature) and melt it, leaving 100 grams of liquid Al at 660 C? Obviously, your answer
will depend on your initial room temperature, so there is no one “absolutely correct” answer to
this problem; I am more interested in the process you use to get the answer. An absurd initial
room temperature, however, will result in a loss of 2 points. (Ans. With room temperature =
20C, total heat energy necessary is 23, 240 cal)
4.
Assume that Earth’s seas and oceans were filled with alcohol instead of water. Alcohol has a
specific heat equal to 0.58 cal/g C. How would this affect sea breezes and land breezes?
Would they still exist? If not, why not? If so, would they be stronger or weaker than we
experience now? Or, would sea and land breezes remain exactly the same as they are today?
Be sure your explanations are very clear – answers without explanations will get no credit. (I
claim that because the breezes exist due to the large difference between the specific heats of
water and land, and since c(alcohol) < c(water), the breezes would not be as strong, since the
difference between c(land) and c(alcohol) is less than the difference between c(land) and
c(water).)
5.
Calculate the minimum amount of heat necessary to completely vaporize 100 g of Aluminum
originally at 60C. Let cAl (solid) = 0.215 cal/gC; cAl (liquid) = 0.400 cal/gC; the heat of
fusion of Al = 94.8 cal/g; the heat of vaporization of Al = 2720 cal/g; the freezing point of
Aluminum = 660C, and the boiling point of liquid Aluminum = 2450C. This problem is
actually pretty easy  it's very similar to the ice  steam problem that I did in class! (Ans.
365980 cal)
6.
This should sound familiar. 100 grams of Aluminum originally at 95C is dumped into
180 grams of water initially at 10C. Assuming the mixture is well insulated (like in the
calorimeters used in lab), what is the final temperature of the mixture? You should ignore the
presence of the calorimeter in this problem (unlike in lab!), but you can still assume that the
aluminum and water come to the same final temperature. (Ans. 19.07C)
7.
Another familiar one. 50 grams of ice initially at 0C is dumped into 180 grams of water
initially at 45C. Assuming the mixture is well insulated (like in the calorimeters used in lab),
what is the final temperature of the mixture? You should ignore the presence of the calorimeter
in this problem (unlike in lab!), but you can still assume everything comes to the same final
temperature. (Ans. 17.8C)