Question 1

Given the following table of thermodynamic data,
 
Complete the following sentence. The vaporization of TiCl4 is _ .

Accepted Answer

A)  nonspontaneous at low temperature and spontaneous at high temperature 
B)  spontaneous at low temperature and nonspontaneous at high temperature 
C)  spontaneous at all temperatures 
D)  nonspontaneous at all temperatures 
E)  not enough information given to draw a conclusion 
A)  nonspontaneous at low temperature and spontaneous at high temperature 
B)  spontaneous at low temperature and nonspontaneous at high temperature 
C)  spontaneous at all temperatures 
D)  nonspontaneous at all temperatures 
E)  not enough information given to draw a conclusion

Question 2

Phosphorous and chlorine gases combine to produce phosphorous trichloride:
 
ΔG° at 298 oK for this reaction is - 642.9 kJ/mol. The value of ΔG at 298 K for a reaction mixture that consists of 1.5 atm P2, 1.6 atm Cl2, and 0.65 atm PCl3 is _ .

Accepted Answer

A)  - 7.28 × 103 
B)  - 3.88 × 103 
C)  - 649.5 
D)  - 44.2 
E)  - 708.4 
A)  - 7.28 × 103 
B)  - 3.88 × 103 
C)  - 649.5 
D)  - 44.2 
E)  - 708.4

Question 3

A system that doesn't exchange matter or energy with its surroundings is called an system.

Accepted Answer

A)  isotonic 
B)  adiabatic 
C)  isothermal 
D)  isobaric 
E)  isolated 
A)  isotonic 
B)  adiabatic 
C)  isothermal 
D)  isobaric 
E)  isolated

Question 4

Use the table below to answer the questions that follow.
   Thermodynamic Quantities for Selected Substances at 298.15 K (25°C)  
-The value of ΔS° for the catalytic hydrogenation of acetylene to ethane,   is J/K.

Accepted Answer

A)  +28.7 
B)  +232.5 
C)  - 232.5 
D)  +440.9 
E)  - 76.0 
A)  +28.7 
B)  +232.5 
C)  - 232.5 
D)  +440.9 
E)  - 76.0

Question 5

The value of ΔG° at 100.0 °C for the formation of calcium chloride from its constituent elements:
 
Is kJ/mol. At 25.0 oC for this reaction, ΔH° is - 795.8 kJ/mol, ΔG° is - 748.1 kJ/mol, and
ΔS° is - 159.8 J/K.

Accepted Answer

A)  5.88 × 104  
B)  - 855.4 
C)  1.52 × 104  
D)  - 779.8 
E)  - 736.2 
A)  5.88 × 104  
B)  - 855.4 
C)  1.52 × 104  
D)  - 779.8 
E)  - 736.2

Question 6

Use the table below to answer the questions that follow.
   Thermodynamic Quantities for Selected Substances at 298.15 K (25°C)
-  The combustion of acetylene in the presence of excess oxygen yields carbon dioxide  
The value of ΔSo for this reaction is J/K.

Accepted Answer

A)  +432.4 
B)  +689.3 
C)  - 122.3 
D)  +122.3 
E)  - 432.4 
A)  +432.4 
B)  +689.3 
C)  - 122.3 
D)  +122.3 
E)  - 432.4

Question 7

Calculate OG○(in kJ/mol) for the following reaction at 1 atm and 25○C:   
OHf○C2H6 (g) = - 84.7 kJ/mol; S○C2H6 (g) = 229.5 J/K · mol; OHf○CO2 (g) = - 393.5
kJ/mol; S○CO2 (g) = 213.6 J/K · mol; OHf○H2O (l) = - 285.8 kJ/mol; S○H2O (l) = 69.9 J/K ·
mol

Accepted Answer

Question 8

For a given reaction, OH = +35.5 kJ/mol and OS = +83.6 J/K- mol. The reaction is spontaneous
) Assume that OH and OS do not vary with temperature.

Accepted Answer

A)  at all temperatures 
B)  at T  425 K 
E)  at T > 298 K 
A)  at all temperatures 
B)  at T  425 K 
E)  at T > 298 K

Question 9

Use the table below to answer the questions that follow.
Thermodynamic Quantities for Selected Substances at 298.15 K (25°C)  
-The value of ΔS° for the decomposition of phosphorous trichloride into its constituent elements,   is J/K.

Accepted Answer

A)  +311.7 
B)  +129.4 
C)  +263.7 
D)  - 129.4 
E)  - 311.7 
A)  +311.7 
B)  +129.4 
C)  +263.7 
D)  - 129.4 
E)  - 311.7

Question 10

Which reaction produces a decrease in the entropy of the system?

Accepted Answer

A)  2C (s) + O2 (g) - 2CO (g) 
B)  CO2 (s) -CO2 (g) 
C)  H2O (l) -H2O (g) 
D)  2H2 (g) + O2 (g) - 2H2O (l) 
E)  CaCO3 (s) - CaO (s) + CO2 (g) 
A)  2C (s) + O2 (g) - 2CO (g) 
B)  CO2 (s) -CO2 (g) 
C)  H2O (l) -H2O (g) 
D)  2H2 (g) + O2 (g) - 2H2O (l) 
E)  CaCO3 (s) - CaO (s) + CO2 (g)

Question 11

Consider the reaction:
 
Given the following table of thermodynamic data,  
Determine the temperature (in °C) above which the reaction is nonspontaneous.

Accepted Answer

A)  756.3 
B)  2439 
C)  This reaction is spontaneous at all temperatures. 
D)  618.1 
E)  1235 
A)  756.3 
B)  2439 
C)  This reaction is spontaneous at all temperatures. 
D)  618.1 
E)  1235

Question 12

Use the table below to answer the questions that follow.
Thermodynamic Quantities for Selected Substances at 298.15 K (25°C)  
-The value of ΔG° at 25 °C for the oxidation of solid elemental sulfur to gaseous sulfur trioxide,   is kJ/mol.

Accepted Answer

A)  +370.4 
B)  - 740.8 
C)  +740.8 
D)  +185.2 
E)  - 370.4 
A)  +370.4 
B)  - 740.8 
C)  +740.8 
D)  +185.2 
E)  - 370.4

Question 13

Use the table below to answer the questions that follow.
Thermodynamic Quantities for Selected Substances at 298.15 K (25°C)  
-The value of ΔG° at 25 °C for the decomposition of gaseous sulfur dioxide to solid elemental sulfur and gaseous oxygen,   is kJ/mol.

Accepted Answer

A)  - 269.9 
B)  +395.2 
C)  +300.4 
D)  - 300.4 
E)  +269.9 
A)  - 269.9 
B)  +395.2 
C)  +300.4 
D)  - 300.4 
E)  +269.9

Question 14

Use the table below to answer the questions that follow.
   Thermodynamic Quantities for Selected Substances at 298.15 K (25°C)
-The value of ΔS° for the catalytic hydrogenation of ethene to ethane,   is J/K.

Accepted Answer

A)  +101.9 
B)  +112.0 
C)  - 101.9 
D)  - 120.5 
E)  - 232.5 
A)  +101.9 
B)  +112.0 
C)  - 101.9 
D)  - 120.5 
E)  - 232.5

Question 15

A reversible process is one that _ _.

Accepted Answer

A)  must be carried out at high temperature 
B)  can be reversed with no net change in either system or surroundings 
C)  must be carried out at low temperature 
D)  happens spontaneously 
E)  is spontaneous in both directions 
A)  must be carried out at high temperature 
B)  can be reversed with no net change in either system or surroundings 
C)  must be carried out at low temperature 
D)  happens spontaneously 
E)  is spontaneous in both directions

Question 16

The second law of thermodynamics states that .

Accepted Answer

A)  ΔH°rxn = 3 nΔH°f (products) - 3 mΔH°f (reactants) 
B)  for any spontaneous process, the entropy of the universe increases 
C)  ΔS = qrev/T at constant temperature 
D)  ΔE = q + w 
E)  the entropy of a pure crystalline substance is zero at absolute zero 
A)  ΔH°rxn = 3 nΔH°f (products) - 3 mΔH°f (reactants) 
B)  for any spontaneous process, the entropy of the universe increases 
C)  ΔS = qrev/T at constant temperature 
D)  ΔE = q + w 
E)  the entropy of a pure crystalline substance is zero at absolute zero

Question 17

Use the table below to answer the questions that follow.
Thermodynamic Quantities for Selected Substances at 298.15 K (25°C)  
-The value of ΔG° at 373 K for the oxidation of solid elemental sulfur to gaseous sulfur trioxide,   is kJ/mol.

Accepted Answer

A)  +740.8 
B)  - 728.3 
C)  - 740.8 
D)  - 61.3 
E)  +61.3 
A)  +740.8 
B)  - 728.3 
C)  - 740.8 
D)  - 61.3 
E)  +61.3

Question 18

When a system is at equilibrium, _.

Accepted Answer

A)  the process is not spontaneous in either direction 
B)  the forward and the reverse processes are both spontaneous 
C)  both forward and reverse processes have stopped 
D)  the reverse process is spontaneous but the forward process is not 
E)  the forward process is spontaneous but the reverse process is not 
A)  the process is not spontaneous in either direction 
B)  the forward and the reverse processes are both spontaneous 
C)  both forward and reverse processes have stopped 
D)  the reverse process is spontaneous but the forward process is not 
E)  the forward process is spontaneous but the reverse process is not

Question 19

Which one of the following processes produces a decrease of the entropy of the system?

Accepted Answer

A)  dissolving sodium chloride in water 
B)  sublimation of naphthalene 
C)  dissolving oxygen in water 
D)  explosion of nitroglycerine 
E)  boiling of alcohol 
A)  dissolving sodium chloride in water 
B)  sublimation of naphthalene 
C)  dissolving oxygen in water 
D)  explosion of nitroglycerine 
E)  boiling of alcohol

Question 20

The value of ΔG° at 100.0 °C for the oxidation of solid elemental sulfur to gaseous sulfur dioxide,
 S (s,rhombic) + O2 (g) →SO2 (g)
Is kJ/mol. At 25.0 oC for this reaction, ΔH° is - 269.9 kJ/mol, ΔG° is - 300.4 kJ/mol, and
ΔS° is +11.6 J/K.

Accepted Answer

A)  - 274.2 
B)  - 1,430 
C)  - 4,598 
D)  - 271.1 
E)  - 265.6 
A)  - 274.2 
B)  - 1,430 
C)  - 4,598 
D)  - 271.1 
E)  - 265.6

Exam 19: Chemical Thermodynamics

Given the following table of thermodynamic data, Complete the following sentence. The vaporization of TiCl4 is _ .

Phosphorous and chlorine gases combine to produce phosphorous trichloride: ΔG° at 298 oK for this reaction is - 642.9 kJ/mol. The value of ΔG at 298 K for a reaction mixture that consists of 1.5 atm P2, 1.6 atm Cl2, and 0.65 atm PCl3 is _ .

A system that doesn't exchange matter or energy with its surroundings is called an system.

Use the table below to answer the questions that follow. Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) -The value of ΔS° for the catalytic hydrogenation of acetylene to ethane, is J/K.

The value of ΔG° at 100.0 °C for the formation of calcium chloride from its constituent elements: Is kJ/mol. At 25.0 oC for this reaction, ΔH° is - 795.8 kJ/mol, ΔG° is - 748.1 kJ/mol, and ΔS° is - 159.8 J/K.

Use the table below to answer the questions that follow. Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) - The combustion of acetylene in the presence of excess oxygen yields carbon dioxide The value of ΔSo for this reaction is J/K.

Calculate OG○(in kJ/mol) for the following reaction at 1 atm and 25○C: OHf○C2H6 (g) = - 84.7 kJ/mol; S○C2H6 (g) = 229.5 J/K · mol; OHf○CO2 (g) = - 393.5 kJ/mol; S○CO2 (g) = 213.6 J/K · mol; OHf○H2O (l) = - 285.8 kJ/mol; S○H2O (l) = 69.9 J/K · mol

For a given reaction, OH = +35.5 kJ/mol and OS = +83.6 J/K- mol. The reaction is spontaneous ) Assume that OH and OS do not vary with temperature.

Use the table below to answer the questions that follow. Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) -The value of ΔS° for the decomposition of phosphorous trichloride into its constituent elements, is J/K.

Which reaction produces a decrease in the entropy of the system?

Consider the reaction: Given the following table of thermodynamic data, Determine the temperature (in °C) above which the reaction is nonspontaneous.

Use the table below to answer the questions that follow. Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) -The value of ΔG° at 25 °C for the oxidation of solid elemental sulfur to gaseous sulfur trioxide, is kJ/mol.

Use the table below to answer the questions that follow. Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) -The value of ΔG° at 25 °C for the decomposition of gaseous sulfur dioxide to solid elemental sulfur and gaseous oxygen, is kJ/mol.

Use the table below to answer the questions that follow. Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) -The value of ΔS° for the catalytic hydrogenation of ethene to ethane, is J/K.

A reversible process is one that _ _.

The second law of thermodynamics states that .

Use the table below to answer the questions that follow. Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) -The value of ΔG° at 373 K for the oxidation of solid elemental sulfur to gaseous sulfur trioxide, is kJ/mol.

When a system is at equilibrium, _.

Which one of the following processes produces a decrease of the entropy of the system?

The value of ΔG° at 100.0 °C for the oxidation of solid elemental sulfur to gaseous sulfur dioxide, S (s,rhombic) + O2 (g) →SO2 (g) Is kJ/mol. At 25.0 oC for this reaction, ΔH° is - 269.9 kJ/mol, ΔG° is - 300.4 kJ/mol, and ΔS° is +11.6 J/K.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

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Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Gases

Intermolecular Forces, Liquids, and Solids

Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

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Additional Aspects of Equilibria

Chemistry of the Environment

Electrochemistry

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Filters

Given the following table of thermodynamic data, Complete the following sentence. The vaporization of TiCl₄is _ .

Phosphorous and chlorine gases combine to produce phosphorous trichloride: ΔG° at 298 ^oK for this reaction is - 642.9 kJ/mol. The value of ΔG at 298 K for a reaction mixture that consists of 1.5 atm P₂, 1.6 atm Cl₂, and 0.65 atm PCl₃is _ .

The value of ΔG° at 100.0 °C for the formation of calcium chloride from its constituent elements: Is kJ/mol. At 25.0 ^oC for this reaction, ΔH° is - 795.8 kJ/mol, ΔG° is - 748.1 kJ/mol, and ΔS° is - 159.8 J/K.

Use the table below to answer the questions that follow. Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) - The combustion of acetylene in the presence of excess oxygen yields carbon dioxide The value of ΔS^ofor this reaction is J/K.

Calculate OG^○(in kJ/mol) for the following reaction at 1 atm and 25^○C: OH_f^○C₂H₆(g) = - 84.7 kJ/mol; S^○C₂H₆(g) = 229.5 J/K · mol; OH_f^○CO₂(g) = - 393.5 kJ/mol; S^○CO₂(g) = 213.6 J/K · mol; OH_f^○H₂O (l) = - 285.8 kJ/mol; S^○H₂O (l) = 69.9 J/K · mol

The value of ΔG° at 100.0 °C for the oxidation of solid elemental sulfur to gaseous sulfur dioxide, S (s,rhombic) + O₂(g) →SO₂(g) Is kJ/mol. At 25.0 ^oC for this reaction, ΔH° is - 269.9 kJ/mol, ΔG° is - 300.4 kJ/mol, and ΔS° is +11.6 J/K.