LT 5.0 Review Test

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LT 5.0 Review Test

Use this test to study for your summative assessments

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1 point

LT 5.1 I can describe the heat flow between system and surroundings in terms of direction and sign of ‘q’.

A chemical reaction that absorbs heat from the surroundings is said to be __________ and has a __________ ΔH at constant pressur,

1 point

endothermic; positive

endothermic; negative

exothermic; negative

exothermic; positive

exothermic; neutral

Clear selection

5.2 I can calculate ‘q’ for a reaction from calorimetric data.

A sample of aluminum metal absorbs 9.86 J of heat, upon which the temperature of the sample increases from 23.2°C to 30.5°, Since the specific heat capacity of aluminum is 0.90 J/g-K, the mass of the sample is __________ g.

1 point

1.5

8.1

6.6

Clear selection

21. The molar heat capacity of a compound with the formula C₂H₆SO is 88.0 J/mol-K. The specific heat of this substance is __________ J/g-K.

1 point

88.0

1.13

4.89

6.88 × 10³

-88.0

Clear selection

5.3 I can calculate the heat of a reaction using thermochemical equations and stoichiometry.

1. The value of ΔH° for the reaction below is -72 kJ. __________ kJ of heat are released when 1.0 mol of HBr is formed in this reaction.

H₂ (g) + Br₂ (g) → 2HBr (g)

1 point

144

0.44

-72

Clear selection

2. The value of ΔH° for the reaction below is -126 kJ. __________ kJ are released when 2.00 mol of NaOH is formed in the reaction?

2Na₂O₂ (s) + 2H₂O (l) → 4NaOH (s) + O₂ (g)

1 point

252

3.9

7.8

-126

Clear selection

3. The value of ΔH° for the reaction below is -126 kJ. The amount of heat that is released by the reaction of 25.0 g of Na₂O₂ with water is __________ kJ.

2Na₂O₂ (s) + 2H₂O (l) → 4NaOH (s) + O₂ (g)

1 point

20.2

40.4

67.5

80.8

-126

Clear selection

4. The value of ΔH° for the reaction below is -790 kJ. The enthalpy change accompanying the reaction of 0.95 g of S is __________ kJ.

2S (s) + 3O₂ (g) → 2SO₃ (g)

1 point

-23

-12

-790

Clear selection

5. The value of ΔH° for the reaction below is -6535 kJ. __________ kJ of heat are released in the combustion of 16.0 g of C₆H₆ (l)?

2C₆H₆ (l) + 15O₂ (g) → 12CO₂ (g) + 6₆H₂O (l)

1 point

1.34 × 10³

5.23 × 104

669

2.68 × 10³

-6535

Clear selection

6. The value of ΔH° for the reaction below is -482 kJ. Calculate the heat (kJ) released to the surroundings when 12.0 g of CO (g) reacts completely.

2CO (g) + O₂ (g) → 2CO₂ (g)

1 point

2.89 × 10³

207

103

65.7

-482

Clear selection

7. The value of ΔH° for the reaction below is -336 kJ. Calculate the heat (kJ) released to the surroundings when 23.0 g of HCl is formed.

CH₄ (g) + 3Cl₂ (g) → CHCl₃ (l) + 3HCl (g)

1 point

177

2.57 × 10³

70.7

211

-336

Clear selection

8. The value of ΔH° for the reaction below is -186 kJ. Calculate the heat (kJ) released from the reaction of 25 g of Cl₂.

H₂ (g) + Cl₂ (g) → 2HCl (g)

1 point

5.3 × 10²

-186

Clear selection

9. The enthalpy change for the following reaction is -483.6 kJ. Therefore, the enthalpy change for the following reaction is __________ kJ:

4H₂ (g) + 2O₂ (g) → 4H₂O (g)

1 point

-483.6

-967.2

2.34 × 10⁵

483.6

967.2

Clear selection

10. The value of ΔH° for the reaction below is +128.1 kJ. How many kJ of heat are consumed when 15.5 g of CH₃OH (l) decomposes as shown in the equation?

CH₃OH (l) → CO (g) + 2H₂ (g)

1 point

0.48

62.0

1.3 × 10²

8.3

Clear selection

11. How many kJ of heat are consumed when 5.10 g of H2 (g) is formed as shown in the equation? The value of ΔH° for the reaction below is +128.1 kJ:

CH₃OH (l) → CO (g) + 2H₂ (g)

1 point

162

62.0

128

653

326

Clear selection

12. How many kJ of heat are consumed when 5.10 g of CO (g) is formed as shown in the equation? The value of ΔH° for the reaction below is +128.1 kJ:

CH₃OH (l) → CO (g) + 2H₂ (g)

1 point

0.182

162

8.31

23.3

62.0

Clear selection

13. How many kJ of heat are consumed when 5.75 g of CO (g) is formed as shown in the equation? The value of ΔH° for the reaction below is +128.1 kJ:

CH₃OH (l) → CO (g) + 2H₂ (g)

1 point

23.3

62.0

26.3

162

8.3

Clear selection

14. How many kJ of heat are released when 5.75 g of Ba (s) reacts completely with oxygen to form BaO (s)? The value of ΔH° for the reaction below is -1107 kJ:

2Ba (s) + O₂ (g) → 2BaO (s)

1 point

96.3

26.3

46.4

23.2

193

Clear selection

15. How many kJ of heat are released when 5.75 g of BaO (s) is produced? The value of ΔH° for the reaction below is -1107 kJ:

2Ba (s) + O₂ (g) → 2BaO (s)

1 point

56.9

23.2

20.8

193

96.3

Clear selection

16. How many kJ of heat are released when 15.75 g of Ba (s) reacts completely with oxygen to form BaO (s)? The value of ΔH° for the reaction below is -1107 kJ:

2Ba (s) + O₂ (g) → 2BaO (s)

1 point

20.8

63.5

114

70.3

35.1

Clear selection

19. In the presence of excess oxygen, methane gas burns in a constant-pressure system to yield carbon dioxide and water. Calculate the value of q (kJ) in this exothermic reaction when 1.70 g of methane is combusted at constant pressure,

CH₄ (g) + 2O₂ (g) → CO₂ (g) + 2H₂O (l) ΔH = -890.0 kJ

1 point

-94.6

0.0306

-0.0106

32.7

-9.46 × 10⁴

Clear selection

20. Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction. Calculate the value of q (kJ) in this exothermic reaction when 4.00 g of hydrogen peroxide decomposes at constant pressure.

2H₂O₂ (l) → 2H₂O (l) + O₂ (g) ΔH = -196 kJ

1 point

-23.1

-11.5

-0.0217

1.44

-2.31 × 10⁴

Clear selection

The specific heat capacity of lead is 0.13 J/g-K. How much heat (in J) is required to raise the temperature of 15 g of lead from 22°C to 37°C?

1 point

2.0

-0.13

5.8 × 10⁻⁴

0.13

Clear selection

24. The temperature of a 15-g sample of lead metal increases from 22°C to 37°C upon the addition of 29.0 J of heat. The specific heat capacity of the lead is __________ J/g-K.

1 point

7.8

1.9

0.13

-29

Clear selection

25. The specific heat of bromine liquid is 0.226 J/g • K. The molar heat capacity (in J/mol-K) of bromine liquid is __________.

1 point

707

36.1

18.1

9.05

0.226

Clear selection

26. The specific heat of liquid bromine is 0.226 J/g-K. How much heat (J) is required to raise the temperature of 10.0 mL of bromine from 25.00°C to 27.30°C? The density of liquid bromine: 3.12 g/mL.

1 point

5.20

16.2

300

32.4

10.4

Clear selection

27. The ΔH for the solution process when solid sodium hydroxide dissolves in water is 44.4 kJ/mol. When a 13.9-g sample of NaOH dissolves in 250.0 g of water in a coffee-cup calorimeter, the temperature increases from 23.0°C to __________°, Assume that the solution has the same specific heat as liquid water, 4.184 J/g-K.

1 point

35.2°C

24.0°C

37.8°C

37.0°C

40.2°C

Clear selection

28. A sample of calcium carbonate [CaCO₃ (s)] absorbs 45.5 J of heat, upon which the temperature of the sample increases from 21.1°C to 28.5°, If the specific heat of calcium carbonate is 0.82 J/g-K, what is the mass (in grams) of the sample?

1 point

3.7

5.0

7.5

410

5.0 x 10³

Clear selection

29. An 8.29 g sample of calcium carbonate [CaCO₃ (s)] absorbs 50.3 J of heat, upon which the temperature of the sample increases from 21.1°C to 28.5°, What is the specific heat of calcium carbonate?

1 point

0.63

0.82

1.1

2.2

4.2

Clear selection

30. A sample of iron absorbs 67.5 J of heat, upon which the temperature of the sample increases from 21.5°C to 28.5°, If the specific heat of iron is 0.450 J/g-K, what is the mass (in grams) of the sample?

1 point

4.3

1100

1.1 x 10³

Clear selection

31. A 22.44 g sample of iron absorbs 180.8 J of heat, upon which the temperature of the sample increases from 21.1°C to 39.0°, What is the specific heat of iron?

1 point

0.140

0.450

0.820

0.840

0.900

Clear selection

32. The specific heat capacity of liquid water is 4.18 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of water from 25.1°C to 65.3°C?

1 point

48.1

840

1.89 × 10³

2.08 × 10⁻²

54.4

Clear selection

33. The specific heat capacity of methane gas is 2.20 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of methane from 36.0°C to 75.0°C?

1 point

88.6

429

1221

0.0113

22.9

Clear selection

34. The specific heat capacity of liquid mercury is 0.14 J/g-K. How many joules of heat are needed to raise the temperature of 5.00 g of mercury from 15.0°C to 36.5°C?

1 point

7.7 × 102

0.0013

1.7

Clear selection

35. The specific heat capacity of solid copper metal is 0.385 J/g-K. How many joules of heat are needed to raise the temperature of a 1.55-kg block of copper from 33.0°C to 77.5°C?

1 point

1.79 × 10⁵

26.6

2.66 × 10⁴

5.58 × 10⁻⁶

0.00558

Clear selection

36. A 5.00-g sample of liquid water at 25.0 C is heated by the addition of 84.0 J of energy. The final temperature of the water is __________ °, The specific heat capacity of liquid water is

1 point

95.2

25.2

-21.0

29.0

4.02

Clear selection

37. A 50.0-g sample of liquid water at 25.0 C is mixed with 29.0 g of water at 45.0°, The final temperature of the water is __________.

1 point

102

27.6

35.0

142

32.3

Clear selection

38. A 6.50-g sample of copper metal at 25.0°C is heated by the addition of 84.0 J of energy. The final temperature of the copper is ________°, The specific heat capacity of copper is 0.38 J/g°,

1 point

29.9

25.0

9.0

59.0

34.0

Clear selection

39. What is the enthalpy change (in kJ) of a chemical reaction that raises the temperature of 250.0 ml of solution having a density of 1.25 g/ml by 7.80°C? (The specific heat of the solution is 3.74 joules/gram-K.)

1 point

-7.43

-12.51

8.20

-9.12

6.51

Clear selection

5.4 I can calculate ‘q’ for a reaction from Hess’s Law.

1 point

355

-1135

+1135

+35

-35

Clear selection

1 point

-59.0

40.5

-15.5

-109

+109

Clear selection

1 point

180.6

-47.8

47.8

90.3

-180.6

Clear selection

1 point

-68

-292

292

-146

Clear selection

1 point

196

-196

1087

-1384

-543

Clear selection

1 point

215.4

571.6

-215.4

-571.6

7.01 × 10⁴

Clear selection

1 point

-395.62

-527.65

439.63

571.66

527.65

Clear selection

1 point

67.6

-67.6

293.8

-293.8

45.5

Clear selection

1 point

67.6

45.5

-293.8

-45.5

293.8

Clear selection

1 point

145.7

343.9

-343.9

17.5

-145.7

Clear selection

5.5 I can calculate ‘q’ for a reaction from enthalpies of formation.

50. The value of ΔH° for the reaction below is -186 kJ. The value of ΔHf° for HCl (g) is __________ kJ/mol.

H₂ (g) + Cl₂ (g) → 2HCl (g)

1 point

-3.72 × 10²

-1.27 × 10²

-93.0

-186

+186

Clear selection

51. The value of ΔH° for the following reaction is -3351 kJ. The value of ΔHf° for Al2O3 (s) is __________ kJ. *

2Al (s) + 3O₂ (g) → 2Al₂O₃ (s)

1 point

-3351

-1676

-32.86

-16.43

+3351

1 point

-744.9

-4519

-4219

-130.4

-76.4

Clear selection

1 point

-1172

-150

-1540

-1892

The ΔHf° of O₂ (g) is needed for the calculation.

Clear selection

1 point

-79.0

-1048.0

-476.4

-492.6

The value of ΔHf° of O₂ (g) is required for the calculation.

Clear selection

1 point

140

-140

-508

-64

Clear selection

1 point

1801

-1801

121

-121

-101

Clear selection

1 point

-566.4

-283.2

283.2

-677.0

The ΔH°f of O₂ (g) is needed for the calculation.

Clear selection

1 point

-1600

-813.4

-635.5

813.4

177.8

Clear selection

1 point

-1.6

+1.6

-3.2

+3.2

The ΔH°f of S (s) and of O₂ (g) are needed for the calculation.

Clear selection

1 point

-267

-370

-202

-308

More data are needed to complete the calculation.

Clear selection

1 point

-99

-198

198

The ΔH°f of O₂ (g) is needed for the calculation.

Clear selection

1 point

-132

1496

704

-704

-2.16 × 10³

Clear selection

1 point

-385.77

-570.37

570.37

385.77

The ΔH°f of Cl₂ (g) is needed for the calculation.

Clear selection

1 point

-570.37

-385.77

570.37

385.77

The ΔH°f of Cl₂ (g) is needed for the calculation.

Clear selection

65. For which one of the following reactions is ΔH°rxn equal to the heat of formation of the product?

1 point

N₂ (g) + 3H₂ (g) → 2NH₃ (g)

(1/2)N₂ (g) + O₂ (g) → NO₂ (g)

6C (s) + 6H (g) → C₆H₆ (l)

P (g) + 4H (g) + Br (g) → PH₄Br (l)

12C (g) + 11H₂ (g) + 11O (g) → C₆H₂₂O₁₁ (g)

Clear selection

66. Of the following, ΔHf° is not zero for __________.

1 point

O₂ (g)

C (graphite)

N₂ (g)

F₂ (s)

Cl₂ (g)

Clear selection

67. Consider the following two reactions: A → 2B ΔH°rxn = 456.7 kJ/mol; A → C ΔH°rxn = -22.1kJ/mol

Determine the enthalpy change for the process, 2B → C

1 point

-478.8 kJ/mol

-434.6 kJ/mol

434.6 kJ/mol

478.8 kJ/mol

More information is needed to solve the problem.

Clear selection

68. In the reaction below, ΔHf° is zero for __________.

Ni (s) + 2CO (g) + 2PF₃ (g) → Ni(CO)₂(PF₃)₂ (l)

1 point

Ni (s)

CO (g)

PF₃ (g)

Ni(CO)₂(PF₃)₂ (l)

both CO (g) and PF₃ (g)

Clear selection

69. For the species in the reaction below, ΔHf° is zero for __________.

2Co (s) + H₂ (g) + 8PF₃ (g) → 2HCo(PF₃)₄ (l)

1 point

Co (s)

H₂ (g)

PF₃ (g)

HCo(PF₃)₄ (l)

both Co(s) and H₂ (g)

Clear selection

70. For which one of the following equations is ΔH°rxn equal to ΔHf° for the product?

1 point

Xe (g) + 2F₂ (g) → XeF₄ (g)

CH₄ (g) + 2Cl₂ (g) → CH₂Cl₂ (l) + 2HCl (g)

N₂ (g) + O₃ (g) → N₂O₃ (g)

2CO (g) + O₂ (g) → 2CO₂ (g)

C (diamond) + O₂ (g) → CO₂ (g)

Clear selection

71. For which one of the following reactions is the value of ΔH°rxn equal to ΔHf° for the product?

1 point

2Ca (s) + O₂ (g) → 2CaO (s)

C₂H₂ (g) + H₂ (g) → C₂H₄ (g)

2C (graphite) + O₂ (g) → 2CO (g)

3Mg (s) + N₂ (g) → Mg₃N₂ (s)

C (diamond) + O₂ (g) → CO₂ (g)

Clear selection

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