Download stations - Harrison High School

1. During the phase change from solid to liquid, the
temperature of the sample
a)
b)
c)
d)
e)
increases
decreases
doubles
halves
does not change
• a) increases
2. The process of melting the solid sample is an
________________ process.
a) endothermic
b) exothermic
c)
neither, energy is not created nor
destroyed
2. The process of melting the solid sample is an
________________ process.
a) endothermic
b) exothermic
c)
neither, energy is not created nor
destroyed
3. During the condensation of the water vapor
to water, heat is _________ by the system.
a)
b)
c)
gained
lost
neither
• 3. During the condensation of the water vapor to
water, heat is _________ by the system.
•
• a) gained
• b) lost
• c) neither
•
4. The vaporization of water is a
_______________________ process.
a)
b)
c)
d)
slow
exothermic
endothermic
boring
• 4. The vaporization of water is a
_______________________ process.
•
• a) slow
• b) exothermic
• c) endothermic
• d) boring
5. Which of the following is an exothermic
process?
a) Candle wax melting
b) A puddle evaporating
c)
Dry ice (solid CO2) subliming to form
gaseous CO2
d) Water freezing to form ice
• 5. Which of the following is an exothermic
process?
• a) Candle wax melting
• b) A puddle evaporating
• c) Dry ice (solid CO2) subliming to form
gaseous CO2
• d) Water freezing to form ice
6. A measure of the average kinetic energy of
the particles in a sample of matter is
a.
b.
c.
d.
e.
heat
enthalpy
temperature
energy
both
• 6. A measure of the average kinetic energy of
the particles in a sample of matter is
•
• a. heat
• b. enthalpy
• c. temperature
• d. energy
• e. both
7. As ice cools from 0oC to -10oC, the average kinetic
energy of its molecules will
________________________.
a. decrease
b. increase
c. remain the same
• 7. As ice cools from 0oC to -10oC, the average
kinetic energy of its molecules will
________________________.
•
• a. decrease
• b. increase
• c. remain the same
•
•
8. Water has a ____________________ specific
heat, which allows it to heat and cool slowly.
a.
b.
high
low
• 8. Water has a ____________________
specific heat, which allows it to heat and cool
slowly.
•
• a. high
• b. low
9. Solid X is placed in contact with solid Y. Heat
will flow spontaneously from X to Y when
_______________________.
a. X is 20°C and Y is 20°C
b. X is 10°C and Y is 5°C
c. X is -25°C and Y is -10°C
d. X is 25°C and Y is 30°C
• 9. Solid X is placed in contact with solid Y.
Heat will flow spontaneously from X to Y when
_______________________.
• a. X is 20°C and Y is 20°C
• b. X is 10°C and Y is 5°C
• c. X is -25°C and Y is -10°C
• d. X is 25°C and Y is 30°C
10. Compared to 100 g of iron, a 10-g sample of
iron has ____________.
a. a higher specific heat
b. a lower specific heat
c. the same specific heat
• 10. Compared to 100 g of iron, a 10-g sample
of iron has ____________.
• a. a higher specific heat
• b. a lower specific heat
• c. the same specific heat
•
11. When a 37.5 gram sample of an unknown
metal cools from 77 ˚C to 23 ˚C, 560 J of energy is
released. Find the specific heat capacity of the
unknown metal.
a)
b)
c)
d)
0.149 J/g˚C
2.28 J/g˚C
0.277 J/g˚C
16.1 J/g˚C
• 11. When a 37.5 gram sample of an unknown
metal cools from 77 ˚C to 23 ˚C, 560 J of energy is
released. Find the specific heat capacity of the
unknown metal.
•
•
•
•
a)
b)
c)
d)
0.149 J/g˚C
2.28 J/g˚C
0.277 J/g˚C
16.1 J/g˚C
12. How much heat is absorbed when a 15.8 g
sample of potassium with c = 0.75 J/g˚C changes
temperature by 14˚C?
a)
b)
c)
d)
51.7 J
165.9 J
106.6 J
4.245 J
• 12. How much heat is absorbed when a 15.8 g
sample of potassium with c = 0.75 J/g˚C changes
temperature by 14˚C?
•
•
•
•
•
a)
b)
c)
d)
51.7 J
165.9 J
106.6 J
4.245 J
13. A chunk of iron (CFe = 0.46 J/g˚C) at 90˚C is
added to a calorimeter containing 150 g of water at
23˚C. The final temperature of the system is 31˚C.
What was the mass of the iron?
a)
b)
c)
d)
189.1 g
1.005 g
166.5 g
124.0 g
• 13. A chunk of iron (CFe = 0.46 J/g˚C) at 90˚C is
added to a calorimeter containing 150 g of water
at 23˚C. The final temperature of the system is
31˚C. What was the mass of the iron?
•
•
•
•
•
a)
b)
c)
d)
189.1 g
1.005 g
166.5 g
124.0 g
14. A sample of 2.8 grams of water is cooled from 105°C to -6°C. How
much heat is lost from the sample?
∆H fusion = 333.5 J/g
∆H vap = 2260 J/g
C solid = 2.1 J/g°C
C liquid = 4.184 J/g°C
C vapor = 1.7 J/g°C
a)1299.144 J
b)1632.76 J
c)2259.04 J
d)8492.4 J
• 14. A sample of 2.8 grams of water is cooled from 105°C to -6°C.
How much heat is lost from the sample?
•
•
•
•
•
∆H fusion = 333.5 J/g
∆H vap = 2260 J/g
C solid = 2.1 J/g°C
C liquid = 4.184 J/g°C
C vapor = 1.7 J/g°C
•
•
•
•
a)1299.144 J
b)1632.76 J
c)2259.04 J
d)8492.4 J
15. A light bulb filament made of tungsten has a mass of
1 g and has a temperature of 1500 C. Calculate the
amount of heat released when the filament is cooled to
20 C. The specific heat capacity of tungsten is 0.142 J/g C.
a) 210.16 J
b) 10563.4 J
c) 1500.142
d) 20.142
• 15. A light bulb filament made of tungsten has a mass
of 1 g and has a temperature of 1500 C. Calculate the
amount of heat released when the filament is cooled
to 20 C. The specific heat capacity of tungsten is 0.142
J/g C.
•
• a) 210.16 J
• b) 10563.4 J
• c) 1500.142
• d) 20.142
16. When natural gas (methane, CH4) is burned,
891.2 kJ of heat is produced as follows:
CH4 + 2 O2 ----> CO2 + 2 H2O + 891.2 kJ
How much heat will be produced by the burning of
454 grams of natural gas?
a) 404604.8 kJ
b) 25287.8 kJ
c) 1.96 kJ
d) 1345.2 kJ
• 16. When natural gas (methane, CH4) is burned,
891.2 kJ of heat is produced as follows:
•
CH4 + 2 O2 ----> CO2 + 2 H2O + 891.2 kJ
• How much heat will be produced by the burning
of 454 grams of natural gas?
•
• a) 404604.8 kJ
• b) 25287.8 kJ
• c) 1.96 kJ
• d) 1345.2 kJ
17. When baking soda decomposes, the reaction is
2NaHCO3 (s) ----> Na2CO3 (s) + H2O (g) + CO2
(g) H = 129 kJ
Determine the mass of baking soda that will decompose
when 65.3 kJ of energy are applied to the system.
a)
b)
c)
d)
63.7 g
184 g
85 g
1.98 g
• 17. When baking soda decomposes, the reaction is
•
2NaHCO3 (s) ----> Na2CO3 (s) + H2O (g) + CO2 (g)
H = 129 kJ
• Determine the mass of baking soda that will decompose
when 65.3 kJ of energy are applied to the system.
•
•
•
•
•
a)
b)
c)
d)
63.7 g
184 g
85 g
1.98 g