Name: ________________________ Class: ___________________ Date: __________
CHEMISTRY
Grade 11 Midsemester 1 Evaluation
Matching (0.5 Mark each)
Match each item with the correct statement below.
a. calorimeter
d. enthalpy
b. calorie
e. specific heat
c. joule
f. heat capacity
____
1. quantity of heat needed to raise the temperature of 1 g of water by 1C
____
2. heat content of a system
____
3. quantity of heat needed to change the temperature of an object by 1C
____
4. quantity of heat needed to change the temperature of 1 g of a substance by 1 C
____
5. SI unit of energy
____
6. device used to measure the heat absorbed or released during a chemical or physical process
Match each item with the correct statement below.
a. heat of reaction
d. heat of fusion
b. heat of formation
e. heat of solution
c. Hess's law of heat summation
____
7. the energy required to melt a solid at its melting point
____
8. the enthalpy change caused by dissolving a substance
____
9. the enthalpy change for a chemical reaction
____ 10. the change in enthalpy that accompanies making a compound from its elements
Multiple Choice (1.5 Marks each)
Identify the choice that best completes the statement or answers the question.
____ 11. A 100 gram piece of heated iron cools from 50° to 20°C. How much heat is released to the surroundings?
(cp of Iron = 0.449)
a. 300 J of heat are released to the surroundings.
b. 300 cal of heat are released to the surroundings.
c. The amount of heat cannot be calculated because the heat capacity is not known.
d. The amount of heat cannot be calculated because there is no closed system.
1
____ 12. What is the heat of solution?
a. the amount of heat released when a vapor changes into a liquid
b. the amount of heat required to change a solid into a liquid
c. the amount of heat required to change a vapor into a liquid
d. the amount of heat absorbed or released when a solid dissolves
____ 13. What do you know about a chemical reaction if the value of H is positive?
a. The reaction cannot occur at room temperature.
b. The reaction is exothermic.
c. The reaction occurs without the addition of energy.
d. The reaction is endothermic.
____ 14. Calculate H for the reaction of sulfur dioxide with oxygen.
2SO 2 (g) + O 2 (g)  2SO 3 (g)
(H 0f SO 2 (g) = –296.8 kJ/mol; H 0f SO 3 (g) = –395.7 kJ/mol)
a.
b.
c.
d.
197.8 kJ
–197.8 kJ
–98.9 kJ
98.9 kJ
____ 15. The specific heat of silver is 0.24
J
. How many joules of energy are needed to warm 4.37 g of silver
gC
from 25.0C to 27.5C?
a. 0.022 J
b. 2.62 J
c. 45.5 J
d. 0.14 J
____ 16. A process that absorbs heat is a(n) ____.
a. polythermic process
b. endothermic process
c. ectothermic process
d. exothermic process
____ 17. What is the amount of heat required to raise the temperature of 200.0 g of aluminum by 10 C? (specific
heat of aluminum = 0.21
a.
b.
c.
d.
cal
)
gC
420 cal
42,000 cal
420,000 cal
4200 cal
2
____ 18. Calculate the energy required to produce 7.00 mol Cl 2 O 7 on the basis of the following balanced equation.
2Cl 2 (g) + 7O 2 (g) + 130 kcal  2Cl 2 O 7 (g)
a.
b.
c.
d.
65 kcal
455 kcal
7.00 kcal
130 kcal
____ 19. How can energy change during a chemical reaction?
a. change in the mass of the reactants or thermal energy
b. transfer of heat and/or work
c. increase in heat and/or destruction of matter
d. increase or decrease in total energy of a system
____ 20. What is the specific heat of a substance if 1560 cal are required to raise the temperature of a 312-g sample
by 15C?
cal
gC
cal
0.99
gC
cal
0.33
gC
cal
1.33
gC
a. 0.033
b.
c.
d.
____ 21. How can you describe the specific heat of olive oil if it takes approximately 420 J of heat to raise the
temperature of 7 g of olive oil by 30C?
a. equal to the specific heat of water
b. less than the specific heat of water
c. Not enough information is given.
d. greater than the specific heat of water
____ 22. During an endothermic chemical reaction, what is the source of energy that causes the reaction to continue?
a. materials that are part of the system
b. chemical bonds of the reaction products
c. reactants involved in the reaction
d. materials in the surroundings of the system
____ 23. What does the symbol H stand for?
a. the specific heat of a substance
b. one Calorie given off by a reaction
c. the heat capacity of a substance
d. the heat of reaction for a chemical reaction
3
____ 24. The amount of heat needed to melt one mole of a solid at a constant temperature is called ____.
a. molar heat of solidification
b. molar heat of fusion
c. heat of reaction
d. enthalpy of fusion
____ 25. How much ice at 0°C could be melted by the addition of 15 kJ of heat? ( Hfus = 6.01kJ/mol)(molar mass of
water=18)
a. 7.2 g
b. 45 g
c. 2.5 g
d. 0.4 g
____ 26. What three factors do you need to know in order to calculate the heat change of a chemical reaction in a
calorimeter?
a. mass of reactants, mass of material that absorbs the heat, temperature change
b. heat capacity of reactants, mass of material that absorbs the heat, temperature change
c. heat capacity and mass of material that absorbs the heat, temperature change
d. heat capacity and mass of reactants in the chemical reaction, temperature change
____ 27. Using a table that lists standard heats of formation, you can calculate the change in enthalpy for a given
chemical reaction. The change in enthalpy is equal to
a. H 0f of products divided by H 0f of reactants.
b. H 0f of products minus H 0f of reactants.
c. H 0f of products plus H 0f of reactants.
d. H 0f of reactants minus H 0f of products.
____ 28. When 45 g of an alloy, at 25C, are dropped into 100.0 g of water, the alloy absorbs 956 J of heat. If the
final temperature of the alloy is 37C, what is its specific heat?
cal
a. 1.77
gC
cal
b. 48.8
gC
cal
c. 0.423
gC
cal
d. 9.88
gC
4
____ 29. One mole of hydrogen is burned in oxygen to produce water in the gas phase, H = 285.8 kJ. What is the
energy change when 1 mole of water, in the gas phase, decomposes to form hydrogen and oxygen?
a. 142.9 kJ of heat is absorbed.
b. 285.8 kJ of heat is released.
c. 285.8 kJ of heat is absorbed.
d. 142.9 kJ of heat is released.
____ 30. The quantity of heat required to change the temperature of 1 g of a substance by 1 C is defined as ____.
a. specific heat
b. a joule
c. a calorie
d. density
____ 31. How is thermal energy transferred between two objects that are at different temperatures?
a. Heat flows from the object that has more thermal energy to the object that has less
thermal energy.
b. The object at a lower temperature pulls heat energy from the warmer object.
c. Heat flows from the warmer object to the cooler object until they reach the same
d.
temperature.
Heat flows back and forth between the two objects until they reach the same temperature.
____ 32. Which of these phase changes is an endothermic process?
a. All phase changes are endothermic.
b. condensation
c. evaporation
d. freezing
____ 33. Which of the following substances has the highest specific heat?
a. mercury
b. steel
c. liquid water
d. ice
____ 34. What is the standard heat of reaction for the following reaction?
Zn(s) + Cu 2  (aq)  Zn 2  (aq) + Cu(s)
(H 0f for Cu 2  = +64.4 kJ/mol; H 0f for Zn 2  = –152.4 kJ/mol)
a.
b.
c.
d.
216.8 kJ absorbed per mole
88.0 kJ absorbed per mole
88.0 kJ released per mole
216.8 kJ released per mole
5
ID: A
CHEMISTRY
Answer Section
Grade 11 Midsemester 1 Evaluation
MATCHING
1. ANS:
OBJ:
BLM:
2. ANS:
OBJ:
BLM:
3. ANS:
OBJ:
BLM:
4. ANS:
OBJ:
BLM:
5. ANS:
OBJ:
BLM:
6. ANS:
OBJ:
BLM:
B
PTS: 1
DIF: L1
REF: p. 558
17.1.1 Explain the ways in which energy changes can occur.
knowledge
D
PTS: 1
DIF: L1
REF: p. 562
17.2.1 Describe how you measure the change in enthalpy of a reaction.
knowledge
F
PTS: 1
DIF: L1
REF: p. 559
17.1.3 Identify two factors on which the heat capacity of an object depends.
knowledge
E
PTS: 1
DIF: L1
REF: p. 559
17.1.3 Identify two factors on which the heat capacity of an object depends.
knowledge
C
PTS: 1
DIF: L1
REF: p. 559
17.1.1 Explain the ways in which energy changes can occur.
knowledge
A
PTS: 1
DIF: L1
REF: p. 562
17.2.1 Describe how you measure the change in enthalpy of a reaction.
knowledge
7. ANS: D
PTS: 1
DIF: L1
REF: p. 569
OBJ: 17.3.1 Compare the quantity of heat absorbed by a melting solid to the quantity of
heat released when the liquid solidifies.
BLM: knowledge
8. ANS: E
PTS: 1
DIF: L1
REF: p. 574
OBJ: 17.3.3 Describe thermochemical changes that occur when a solution forms.
BLM: knowledge
9. ANS: A
PTS: 1
DIF: L1
REF: p. 565
OBJ: 17.2.2 Describe how you express the enthalpy change for a reaction in a chemical
equation.
BLM: knowledge
10. ANS: B
PTS: 1
DIF: L1
REF: p. 530
OBJ: 17.4.1 Identify two ways that you can determine the heat of reaction when it cannot
be directly measured.
BLM: knowledge
1
ID: A
MULTIPLE CHOICE
11. ANS: C
PTS: 1
DIF: L2
REF: p. 559
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: application
12. ANS: D
PTS: 1
DIF: L1
REF: p. 574
OBJ: 17.3.3 Describe thermochemical changes that occur when a solution forms.
BLM: knowledge
13. ANS: D
PTS: 1
DIF: L2
REF: p. 566
OBJ: 17.2.2 Describe how you express the enthalpy change for a reaction in a chemical
equation.
BLM: knowledge
14. ANS: B
PTS: 1
DIF: L2
REF: p. 581
OBJ: 17.4.1 Identify two ways that you can determine the heat of reaction when it cannot
be directly measured.
BLM: analysis
15. ANS: B
PTS: 1
DIF: L2
REF: p. 560
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: analysis
16. ANS: B
PTS: 1
DIF: L1
REF: p. 557
OBJ: 17.1.2 Explain how the energy of the universe before a chemical or physical process
is related to the energy of the universe after a chemical or physical process.
BLM: knowledge
17. ANS: A
PTS: 1
DIF: L2
REF: p. 560
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: analysis
18. ANS: B
PTS: 1
DIF: L2
REF: p. 566
OBJ: 17.2.2 Describe how you express the enthalpy change for a reaction in a chemical
equation.
BLM: analysis
19. ANS: B
PTS: 1
DIF: L1
REF: p. 556
OBJ: 17.1.1 Explain the ways in which energy changes can occur.
BLM: knowledge
20. ANS: C
PTS: 1
DIF: L2
REF: p. 561
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: analysis
21. ANS: B
PTS: 1
DIF: L2
REF: p. 560
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: application
22. ANS: D
PTS: 1
DIF: L2
REF: p. 557
OBJ: 17.1.2 Explain how the energy of the universe before a chemical or physical process
is related to the energy of the universe after a chemical or physical process.
BLM: comprehension
2
ID: A
23. ANS: D
PTS: 1
DIF: L1
REF: p. 563
OBJ: 17.2.1 Describe how you measure the change in enthalpy of a reaction.
BLM: knowledge
24. ANS: B
PTS: 1
DIF: L1
REF: p. 569
OBJ: 17.3.1 Compare the quantity of heat absorbed by a melting solid to the quantity of
heat released when the liquid solidifies.
BLM: knowledge
25. ANS: B
PTS: 1
DIF: L2
REF: p. 570
OBJ: 17.3.1 Compare the quantity of heat absorbed by a melting solid to the quantity of
heat released when the liquid solidifies.
BLM: analysis
26. ANS: C
PTS: 1
DIF: L2
REF: p. 563
OBJ: 17.2.1 Describe how you measure the change in enthalpy of a reaction.
BLM: comprehension
27. ANS: B
PTS: 1
DIF: L1
REF: p. 580
OBJ: 17.4.1 Identify two ways that you can determine the heat of reaction when it cannot
be directly measured.
BLM: knowledge
28. ANS: A
PTS: 1
DIF: L2
REF: p. 560
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: analysis
29. ANS: C
PTS: 1
DIF: L2
REF: p. 566
OBJ: 17.2.2 Describe how you express the enthalpy change for a reaction in a chemical
equation.
BLM: comprehension
30. ANS: A
PTS: 1
DIF: L1
REF: p. 559
OBJ: 17.1.2 Explain how the energy of the universe before a chemical or physical process
is related to the energy of the universe after a chemical or physical process.
BLM: knowledge
31. ANS: C
PTS: 1
DIF: L1
REF: p. 556
OBJ: 17.1.1 Explain the ways in which energy changes can occur.
BLM: knowledge
32. ANS: C
PTS: 1
DIF: L2
REF: p. 558
OBJ: 17.1.2 Explain how the energy of the universe before a chemical or physical process
is related to the energy of the universe after a chemical or physical process.
BLM: application
33. ANS: C
PTS: 1
DIF: L2
REF: p. 559
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: comprehension
34. ANS: D
PTS: 1
DIF: L3
REF: p. 567
OBJ: 17.2.2 Describe how you express the enthalpy change for a reaction in a chemical
equation.
BLM: analysis
3
Name: ________________________ Class: ___________________ Date: __________
CHEMISTRY
Grade 11 Midsemester 1 Evaluation
Matching (0.5 Mark each)
Match each item with the correct statement below.
a. heat of reaction
d. heat of fusion
b. heat of formation
e. heat of solution
c. Hess's law of heat summation
____
1. the change in enthalpy that accompanies making a compound from its elements
____
2. the energy required to melt a solid at its melting point
____
3. the enthalpy change caused by dissolving a substance
____
4. the enthalpy change for a chemical reaction
Match each item with the correct statement below.
a. calorimeter
d. enthalpy
b. calorie
e. specific heat
c. joule
f. heat capacity
____
5. quantity of heat needed to raise the temperature of 1 g of water by 1C
____
6. device used to measure the heat absorbed or released during a chemical or physical process
____
7. quantity of heat needed to change the temperature of an object by 1C
____
8. quantity of heat needed to change the temperature of 1 g of a substance by 1 C
____
9. SI unit of energy
____ 10. heat content of a system
Multiple Choice (1.5 Marks each)
Identify the choice that best completes the statement or answers the question.
____ 11. The specific heat of silver is 0.24
J
. How many joules of energy are needed to warm 4.37 g of silver
gC
from 25.0C to 27.5C?
a. 0.022 J
b. 0.14 J
c. 45.5 J
d. 2.62 J
1
____ 12. What three factors do you need to know in order to calculate the heat change of a chemical reaction in a
calorimeter?
a. mass of reactants, mass of material that absorbs the heat, temperature change
b. heat capacity and mass of material that absorbs the heat, temperature change
c. heat capacity of reactants, mass of material that absorbs the heat, temperature change
d. heat capacity and mass of reactants in the chemical reaction, temperature change
____ 13. How is thermal energy transferred between two objects that are at different temperatures?
a. Heat flows from the object that has more thermal energy to the object that has less
b.
c.
d.
thermal energy.
Heat flows back and forth between the two objects until they reach the same temperature.
The object at a lower temperature pulls heat energy from the warmer object.
Heat flows from the warmer object to the cooler object until they reach the same
temperature.
____ 14. How can you describe the specific heat of olive oil if it takes approximately 420 J of heat to raise the
temperature of 7 g of olive oil by 30C?
a. greater than the specific heat of water
b. Not enough information is given.
c. less than the specific heat of water
d. equal to the specific heat of water
____ 15. A 100 gram piece of heated iron cools from 50° to 20°C. How much heat is released to the surroundings?
(cp of Iron = 0.449)
a. 300 cal of heat are released to the surroundings.
b. The amount of heat cannot be calculated because there is no closed system.
c. The amount of heat cannot be calculated because the heat capacity is not known.
d. 300 J of heat are released to the surroundings.
____ 16. What is the heat of solution?
a. the amount of heat required to change a vapor into a liquid
b. the amount of heat released when a vapor changes into a liquid
c. the amount of heat required to change a solid into a liquid
d. the amount of heat absorbed or released when a solid dissolves
____ 17. How can energy change during a chemical reaction?
a. increase in heat and/or destruction of matter
b. change in the mass of the reactants or thermal energy
c. transfer of heat and/or work
d. increase or decrease in total energy of a system
2
____ 18. Calculate H for the reaction of sulfur dioxide with oxygen.
2SO 2 (g) + O 2 (g)  2SO 3 (g)
(H 0f SO 2 (g) = –296.8 kJ/mol; H 0f SO 3 (g) = –395.7 kJ/mol)
a.
b.
c.
d.
197.8 kJ
98.9 kJ
–98.9 kJ
–197.8 kJ
____ 19. What does the symbol H stand for?
a. the heat capacity of a substance
b. the specific heat of a substance
c. one Calorie given off by a reaction
d. the heat of reaction for a chemical reaction
____ 20. One mole of hydrogen is burned in oxygen to produce water in the gas phase, H = 285.8 kJ. What is the
energy change when 1 mole of water, in the gas phase, decomposes to form hydrogen and oxygen?
a. 285.8 kJ of heat is absorbed.
b. 285.8 kJ of heat is released.
c. 142.9 kJ of heat is released.
d. 142.9 kJ of heat is absorbed.
____ 21. Which of the following substances has the highest specific heat?
a. mercury
b. ice
c. liquid water
d. steel
____ 22. The quantity of heat required to change the temperature of 1 g of a substance by 1 C is defined as ____.
a. a joule
b. a calorie
c. specific heat
d. density
____ 23. How much ice at 0°C could be melted by the addition of 15 kJ of heat? ( Hfus = 6.01kJ/mol)(molar mass of
water=18)
a. 0.4 g
b. 7.2 g
c. 2.5 g
d. 45 g
3
____ 24. What is the amount of heat required to raise the temperature of 200.0 g of aluminum by 10 C? (specific
heat of aluminum = 0.21
a.
b.
c.
d.
cal
)
gC
420,000 cal
4200 cal
42,000 cal
420 cal
____ 25. What do you know about a chemical reaction if the value of H is positive?
a. The reaction cannot occur at room temperature.
b. The reaction is exothermic.
c. The reaction occurs without the addition of energy.
d. The reaction is endothermic.
____ 26. A process that absorbs heat is a(n) ____.
a. polythermic process
b. endothermic process
c. exothermic process
d. ectothermic process
____ 27. What is the specific heat of a substance if 1560 cal are required to raise the temperature of a 312-g sample
by 15C?
cal
gC
cal
1.33
gC
cal
0.33
gC
cal
0.99
gC
a. 0.033
b.
c.
d.
____ 28. When 45 g of an alloy, at 25C, are dropped into 100.0 g of water, the alloy absorbs 956 J of heat. If the
final temperature of the alloy is 37C, what is its specific heat?
cal
a. 0.423
gC
cal
b. 1.77
gC
cal
c. 9.88
gC
cal
d. 48.8
gC
4
____ 29. What is the standard heat of reaction for the following reaction?
Zn(s) + Cu 2  (aq)  Zn 2  (aq) + Cu(s)
(H 0f for Cu 2  = +64.4 kJ/mol; H 0f for Zn 2  = –152.4 kJ/mol)
a.
b.
c.
d.
216.8 kJ released per mole
88.0 kJ absorbed per mole
88.0 kJ released per mole
216.8 kJ absorbed per mole
____ 30. During an endothermic chemical reaction, what is the source of energy that causes the reaction to continue?
a. materials that are part of the system
b. chemical bonds of the reaction products
c. reactants involved in the reaction
d. materials in the surroundings of the system
____ 31. Which of these phase changes is an endothermic process?
a. freezing
b. All phase changes are endothermic.
c. condensation
d. evaporation
____ 32. The amount of heat needed to melt one mole of a solid at a constant temperature is called ____.
a. molar heat of solidification
b. enthalpy of fusion
c. heat of reaction
d. molar heat of fusion
____ 33. Calculate the energy required to produce 7.00 mol Cl 2 O 7 on the basis of the following balanced equation.
2Cl 2 (g) + 7O 2 (g) + 130 kcal  2Cl 2 O 7 (g)
a.
b.
c.
d.
455 kcal
130 kcal
65 kcal
7.00 kcal
____ 34. Using a table that lists standard heats of formation, you can calculate the change in enthalpy for a given
chemical reaction. The change in enthalpy is equal to
a. H 0f of products divided by H 0f of reactants.
b. H 0f of reactants minus H 0f of products.
c. H 0f of products minus H 0f of reactants.
d. H 0f of products plus H 0f of reactants.
5
ID: B
CHEMISTRY
Answer Section
Grade 11 Midsemester 1 Evaluation
MATCHING
1. ANS: B
PTS: 1
DIF: L1
REF: p. 530
OBJ: 17.4.1 Identify two ways that you can determine the heat of reaction when it cannot
be directly measured.
BLM: knowledge
2. ANS: D
PTS: 1
DIF: L1
REF: p. 569
OBJ: 17.3.1 Compare the quantity of heat absorbed by a melting solid to the quantity of
heat released when the liquid solidifies.
BLM: knowledge
3. ANS: E
PTS: 1
DIF: L1
REF: p. 574
OBJ: 17.3.3 Describe thermochemical changes that occur when a solution forms.
BLM: knowledge
4. ANS: A
PTS: 1
DIF: L1
REF: p. 565
OBJ: 17.2.2 Describe how you express the enthalpy change for a reaction in a chemical
equation.
BLM: knowledge
5. ANS:
OBJ:
BLM:
6. ANS:
OBJ:
BLM:
7. ANS:
OBJ:
BLM:
8. ANS:
OBJ:
BLM:
9. ANS:
OBJ:
BLM:
10. ANS:
OBJ:
BLM:
B
PTS: 1
DIF: L1
REF: p. 558
17.1.1 Explain the ways in which energy changes can occur.
knowledge
A
PTS: 1
DIF: L1
REF: p. 562
17.2.1 Describe how you measure the change in enthalpy of a reaction.
knowledge
F
PTS: 1
DIF: L1
REF: p. 559
17.1.3 Identify two factors on which the heat capacity of an object depends.
knowledge
E
PTS: 1
DIF: L1
REF: p. 559
17.1.3 Identify two factors on which the heat capacity of an object depends.
knowledge
C
PTS: 1
DIF: L1
REF: p. 559
17.1.1 Explain the ways in which energy changes can occur.
knowledge
D
PTS: 1
DIF: L1
REF: p. 562
17.2.1 Describe how you measure the change in enthalpy of a reaction.
knowledge
1
ID: B
MULTIPLE CHOICE
11. ANS: D
PTS: 1
DIF: L2
REF: p. 560
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: analysis
12. ANS: B
PTS: 1
DIF: L2
REF: p. 563
OBJ: 17.2.1 Describe how you measure the change in enthalpy of a reaction.
BLM: comprehension
13. ANS: D
PTS: 1
DIF: L1
REF: p. 556
OBJ: 17.1.1 Explain the ways in which energy changes can occur.
BLM: knowledge
14. ANS: C
PTS: 1
DIF: L2
REF: p. 560
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: application
15. ANS: C
PTS: 1
DIF: L2
REF: p. 559
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: application
16. ANS: D
PTS: 1
DIF: L1
REF: p. 574
OBJ: 17.3.3 Describe thermochemical changes that occur when a solution forms.
BLM: knowledge
17. ANS: C
PTS: 1
DIF: L1
REF: p. 556
OBJ: 17.1.1 Explain the ways in which energy changes can occur.
BLM: knowledge
18. ANS: D
PTS: 1
DIF: L2
REF: p. 581
OBJ: 17.4.1 Identify two ways that you can determine the heat of reaction when it cannot
be directly measured.
BLM: analysis
19. ANS: D
PTS: 1
DIF: L1
REF: p. 563
OBJ: 17.2.1 Describe how you measure the change in enthalpy of a reaction.
BLM: knowledge
20. ANS: A
PTS: 1
DIF: L2
REF: p. 566
OBJ: 17.2.2 Describe how you express the enthalpy change for a reaction in a chemical
equation.
BLM: comprehension
21. ANS: C
PTS: 1
DIF: L2
REF: p. 559
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: comprehension
22. ANS: C
PTS: 1
DIF: L1
REF: p. 559
OBJ: 17.1.2 Explain how the energy of the universe before a chemical or physical process
is related to the energy of the universe after a chemical or physical process.
BLM: knowledge
2
ID: B
23. ANS: D
PTS: 1
DIF: L2
REF: p. 570
OBJ: 17.3.1 Compare the quantity of heat absorbed by a melting solid to the quantity of
heat released when the liquid solidifies.
BLM: analysis
24. ANS: D
PTS: 1
DIF: L2
REF: p. 560
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: analysis
25. ANS: D
PTS: 1
DIF: L2
REF: p. 566
OBJ: 17.2.2 Describe how you express the enthalpy change for a reaction in a chemical
equation.
BLM: knowledge
26. ANS: B
PTS: 1
DIF: L1
REF: p. 557
OBJ: 17.1.2 Explain how the energy of the universe before a chemical or physical process
is related to the energy of the universe after a chemical or physical process.
BLM: knowledge
27. ANS: C
PTS: 1
DIF: L2
REF: p. 561
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: analysis
28. ANS: B
PTS: 1
DIF: L2
REF: p. 560
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: analysis
29. ANS: A
PTS: 1
DIF: L3
REF: p. 567
OBJ: 17.2.2 Describe how you express the enthalpy change for a reaction in a chemical
equation.
BLM: analysis
30. ANS: D
PTS: 1
DIF: L2
REF: p. 557
OBJ: 17.1.2 Explain how the energy of the universe before a chemical or physical process
is related to the energy of the universe after a chemical or physical process.
BLM: comprehension
31. ANS: D
PTS: 1
DIF: L2
REF: p. 558
OBJ: 17.1.2 Explain how the energy of the universe before a chemical or physical process
is related to the energy of the universe after a chemical or physical process.
BLM: application
32. ANS: D
PTS: 1
DIF: L1
REF: p. 569
OBJ: 17.3.1 Compare the quantity of heat absorbed by a melting solid to the quantity of
heat released when the liquid solidifies.
BLM: knowledge
33. ANS: A
PTS: 1
DIF: L2
REF: p. 566
OBJ: 17.2.2 Describe how you express the enthalpy change for a reaction in a chemical
equation.
BLM: analysis
34. ANS: C
PTS: 1
DIF: L1
REF: p. 580
OBJ: 17.4.1 Identify two ways that you can determine the heat of reaction when it cannot
be directly measured.
BLM: knowledge
3
Name: ________________________ Class: ___________________ Date: __________
CHEMISTRY
Grade 11 Midsemester 1 Evaluation
Matching (0.5 Mark each)
Match each item with the correct statement below.
a. heat of reaction
d. heat of fusion
b. heat of formation
e. heat of solution
c. Hess's law of heat summation
____
1. the enthalpy change for a chemical reaction
____
2. the enthalpy change caused by dissolving a substance
____
3. the change in enthalpy that accompanies making a compound from its elements
____
4. the energy required to melt a solid at its melting point
Match each item with the correct statement below.
a. calorimeter
d. enthalpy
b. calorie
e. specific heat
c. joule
f. heat capacity
____
5. quantity of heat needed to raise the temperature of 1 g of water by 1C
____
6. heat content of a system
____
7. quantity of heat needed to change the temperature of an object by 1C
____
8. device used to measure the heat absorbed or released during a chemical or physical process
____
9. quantity of heat needed to change the temperature of 1 g of a substance by 1 C
____ 10. SI unit of energy
Multiple Choice (1.5 Marks each)
Identify the choice that best completes the statement or answers the question.
____ 11. A process that absorbs heat is a(n) ____.
a. endothermic process
b. ectothermic process
c. polythermic process
d. exothermic process
1
____ 12. How is thermal energy transferred between two objects that are at different temperatures?
a. Heat flows back and forth between the two objects until they reach the same temperature.
b. Heat flows from the object that has more thermal energy to the object that has less
thermal energy.
c. The object at a lower temperature pulls heat energy from the warmer object.
d. Heat flows from the warmer object to the cooler object until they reach the same
temperature.
____ 13. Using a table that lists standard heats of formation, you can calculate the change in enthalpy for a given
chemical reaction. The change in enthalpy is equal to
a. H 0f of products minus H 0f of reactants.
b. H 0f of reactants minus H 0f of products.
c. H 0f of products plus H 0f of reactants.
d. H 0f of products divided by H 0f of reactants.
____ 14. A 100 gram piece of heated iron cools from 50° to 20°C. How much heat is released to the surroundings?
(cp of Iron = 0.449)
a. 300 cal of heat are released to the surroundings.
b. 300 J of heat are released to the surroundings.
c. The amount of heat cannot be calculated because there is no closed system.
d. The amount of heat cannot be calculated because the heat capacity is not known.
____ 15. The quantity of heat required to change the temperature of 1 g of a substance by 1 C is defined as ____.
a. a calorie
b. specific heat
c. a joule
d. density
____ 16. The specific heat of silver is 0.24
J
. How many joules of energy are needed to warm 4.37 g of silver
gC
from 25.0C to 27.5C?
a. 2.62 J
b. 45.5 J
c. 0.022 J
d. 0.14 J
____ 17. The amount of heat needed to melt one mole of a solid at a constant temperature is called ____.
a. heat of reaction
b. molar heat of solidification
c. enthalpy of fusion
d. molar heat of fusion
2
____ 18. What do you know about a chemical reaction if the value of H is positive?
a. The reaction cannot occur at room temperature.
b. The reaction occurs without the addition of energy.
c. The reaction is exothermic.
d. The reaction is endothermic.
____ 19. How can you describe the specific heat of olive oil if it takes approximately 420 J of heat to raise the
temperature of 7 g of olive oil by 30C?
a. greater than the specific heat of water
b. less than the specific heat of water
c. Not enough information is given.
d. equal to the specific heat of water
____ 20. One mole of hydrogen is burned in oxygen to produce water in the gas phase, H = 285.8 kJ. What is the
energy change when 1 mole of water, in the gas phase, decomposes to form hydrogen and oxygen?
a. 285.8 kJ of heat is released.
b. 142.9 kJ of heat is absorbed.
c. 142.9 kJ of heat is released.
d. 285.8 kJ of heat is absorbed.
____ 21. Which of the following substances has the highest specific heat?
a. steel
b. liquid water
c. mercury
d. ice
____ 22. What is the specific heat of a substance if 1560 cal are required to raise the temperature of a 312-g sample
by 15C?
cal
gC
cal
0.99
gC
cal
0.033
gC
cal
1.33
gC
a. 0.33
b.
c.
d.
3
____ 23. What is the amount of heat required to raise the temperature of 200.0 g of aluminum by 10 C? (specific
heat of aluminum = 0.21
a.
b.
c.
d.
cal
)
gC
420,000 cal
4200 cal
42,000 cal
420 cal
____ 24. How can energy change during a chemical reaction?
a. change in the mass of the reactants or thermal energy
b. transfer of heat and/or work
c. increase in heat and/or destruction of matter
d. increase or decrease in total energy of a system
____ 25. What does the symbol H stand for?
a. the specific heat of a substance
b. one Calorie given off by a reaction
c. the heat of reaction for a chemical reaction
d. the heat capacity of a substance
____ 26. When 45 g of an alloy, at 25C, are dropped into 100.0 g of water, the alloy absorbs 956 J of heat. If the
final temperature of the alloy is 37C, what is its specific heat?
cal
a. 9.88
gC
cal
b. 48.8
gC
cal
c. 1.77
gC
cal
d. 0.423
gC
____ 27. Calculate H for the reaction of sulfur dioxide with oxygen.
2SO 2 (g) + O 2 (g)  2SO 3 (g)
(H 0f SO 2 (g) = –296.8 kJ/mol; H 0f SO 3 (g) = –395.7 kJ/mol)
a.
b.
c.
d.
98.9 kJ
197.8 kJ
–197.8 kJ
–98.9 kJ
4
____ 28. What is the heat of solution?
a. the amount of heat required to change a solid into a liquid
b. the amount of heat required to change a vapor into a liquid
c. the amount of heat absorbed or released when a solid dissolves
d. the amount of heat released when a vapor changes into a liquid
____ 29. What is the standard heat of reaction for the following reaction?
Zn(s) + Cu 2  (aq)  Zn 2  (aq) + Cu(s)
(H 0f for Cu 2  = +64.4 kJ/mol; H 0f for Zn 2  = –152.4 kJ/mol)
a.
b.
c.
d.
88.0 kJ absorbed per mole
216.8 kJ released per mole
216.8 kJ absorbed per mole
88.0 kJ released per mole
____ 30. How much ice at 0°C could be melted by the addition of 15 kJ of heat? ( Hfus = 6.01kJ/mol)(molar mass of
water=18)
a. 7.2 g
b. 2.5 g
c. 45 g
d. 0.4 g
____ 31. Calculate the energy required to produce 7.00 mol Cl 2 O 7 on the basis of the following balanced equation.
2Cl 2 (g) + 7O 2 (g) + 130 kcal  2Cl 2 O 7 (g)
a.
b.
c.
d.
130 kcal
455 kcal
65 kcal
7.00 kcal
____ 32. What three factors do you need to know in order to calculate the heat change of a chemical reaction in a
calorimeter?
a. mass of reactants, mass of material that absorbs the heat, temperature change
b. heat capacity and mass of reactants in the chemical reaction, temperature change
c. heat capacity and mass of material that absorbs the heat, temperature change
d. heat capacity of reactants, mass of material that absorbs the heat, temperature change
____ 33. Which of these phase changes is an endothermic process?
a. condensation
b. evaporation
c. All phase changes are endothermic.
d. freezing
5
____ 34. During an endothermic chemical reaction, what is the source of energy that causes the reaction to continue?
a. reactants involved in the reaction
b. materials that are part of the system
c. chemical bonds of the reaction products
d. materials in the surroundings of the system
6
ID: C
CHEMISTRY
Answer Section
Grade 11 Midsemester 1 Evaluation
MATCHING
1. ANS: A
PTS: 1
DIF: L1
REF: p. 565
OBJ: 17.2.2 Describe how you express the enthalpy change for a reaction in a chemical
equation.
BLM: knowledge
2. ANS: E
PTS: 1
DIF: L1
REF: p. 574
OBJ: 17.3.3 Describe thermochemical changes that occur when a solution forms.
BLM: knowledge
3. ANS: B
PTS: 1
DIF: L1
REF: p. 530
OBJ: 17.4.1 Identify two ways that you can determine the heat of reaction when it cannot
be directly measured.
BLM: knowledge
4. ANS: D
PTS: 1
DIF: L1
REF: p. 569
OBJ: 17.3.1 Compare the quantity of heat absorbed by a melting solid to the quantity of
heat released when the liquid solidifies.
BLM: knowledge
5. ANS:
OBJ:
BLM:
6. ANS:
OBJ:
BLM:
7. ANS:
OBJ:
BLM:
8. ANS:
OBJ:
BLM:
9. ANS:
OBJ:
BLM:
10. ANS:
OBJ:
BLM:
B
PTS: 1
DIF: L1
REF: p. 558
17.1.1 Explain the ways in which energy changes can occur.
knowledge
D
PTS: 1
DIF: L1
REF: p. 562
17.2.1 Describe how you measure the change in enthalpy of a reaction.
knowledge
F
PTS: 1
DIF: L1
REF: p. 559
17.1.3 Identify two factors on which the heat capacity of an object depends.
knowledge
A
PTS: 1
DIF: L1
REF: p. 562
17.2.1 Describe how you measure the change in enthalpy of a reaction.
knowledge
E
PTS: 1
DIF: L1
REF: p. 559
17.1.3 Identify two factors on which the heat capacity of an object depends.
knowledge
C
PTS: 1
DIF: L1
REF: p. 559
17.1.1 Explain the ways in which energy changes can occur.
knowledge
1
ID: C
MULTIPLE CHOICE
11. ANS: A
PTS: 1
DIF: L1
REF: p. 557
OBJ: 17.1.2 Explain how the energy of the universe before a chemical or physical process
is related to the energy of the universe after a chemical or physical process.
BLM: knowledge
12. ANS: D
PTS: 1
DIF: L1
REF: p. 556
OBJ: 17.1.1 Explain the ways in which energy changes can occur.
BLM: knowledge
13. ANS: A
PTS: 1
DIF: L1
REF: p. 580
OBJ: 17.4.1 Identify two ways that you can determine the heat of reaction when it cannot
be directly measured.
BLM: knowledge
14. ANS: D
PTS: 1
DIF: L2
REF: p. 559
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: application
15. ANS: B
PTS: 1
DIF: L1
REF: p. 559
OBJ: 17.1.2 Explain how the energy of the universe before a chemical or physical process
is related to the energy of the universe after a chemical or physical process.
BLM: knowledge
16. ANS: A
PTS: 1
DIF: L2
REF: p. 560
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: analysis
17. ANS: D
PTS: 1
DIF: L1
REF: p. 569
OBJ: 17.3.1 Compare the quantity of heat absorbed by a melting solid to the quantity of
heat released when the liquid solidifies.
BLM: knowledge
18. ANS: D
PTS: 1
DIF: L2
REF: p. 566
OBJ: 17.2.2 Describe how you express the enthalpy change for a reaction in a chemical
equation.
BLM: knowledge
19. ANS: B
PTS: 1
DIF: L2
REF: p. 560
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: application
20. ANS: D
PTS: 1
DIF: L2
REF: p. 566
OBJ: 17.2.2 Describe how you express the enthalpy change for a reaction in a chemical
equation.
BLM: comprehension
21. ANS: B
PTS: 1
DIF: L2
REF: p. 559
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: comprehension
22. ANS: A
PTS: 1
DIF: L2
REF: p. 561
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: analysis
2
ID: C
23. ANS: D
PTS: 1
DIF: L2
REF: p. 560
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: analysis
24. ANS: B
PTS: 1
DIF: L1
REF: p. 556
OBJ: 17.1.1 Explain the ways in which energy changes can occur.
BLM: knowledge
25. ANS: C
PTS: 1
DIF: L1
REF: p. 563
OBJ: 17.2.1 Describe how you measure the change in enthalpy of a reaction.
BLM: knowledge
26. ANS: C
PTS: 1
DIF: L2
REF: p. 560
OBJ: 17.1.3 Identify two factors on which the heat capacity of an object depends.
BLM: analysis
27. ANS: C
PTS: 1
DIF: L2
REF: p. 581
OBJ: 17.4.1 Identify two ways that you can determine the heat of reaction when it cannot
be directly measured.
BLM: analysis
28. ANS: C
PTS: 1
DIF: L1
REF: p. 574
OBJ: 17.3.3 Describe thermochemical changes that occur when a solution forms.
BLM: knowledge
29. ANS: B
PTS: 1
DIF: L3
REF: p. 567
OBJ: 17.2.2 Describe how you express the enthalpy change for a reaction in a chemical
equation.
BLM: analysis
30. ANS: C
PTS: 1
DIF: L2
REF: p. 570
OBJ: 17.3.1 Compare the quantity of heat absorbed by a melting solid to the quantity of
heat released when the liquid solidifies.
BLM: analysis
31. ANS: B
PTS: 1
DIF: L2
REF: p. 566
OBJ: 17.2.2 Describe how you express the enthalpy change for a reaction in a chemical
equation.
BLM: analysis
32. ANS: C
PTS: 1
DIF: L2
REF: p. 563
OBJ: 17.2.1 Describe how you measure the change in enthalpy of a reaction.
BLM: comprehension
33. ANS: B
PTS: 1
DIF: L2
REF: p. 558
OBJ: 17.1.2 Explain how the energy of the universe before a chemical or physical process
is related to the energy of the universe after a chemical or physical process.
BLM: application
34. ANS: D
PTS: 1
DIF: L2
REF: p. 557
OBJ: 17.1.2 Explain how the energy of the universe before a chemical or physical process
is related to the energy of the universe after a chemical or physical process.
BLM: comprehension
3