Exam 19: Chemical Thermodynamics

Consider a pure crystalline solid that is heated from absolute zero to a temperature above the boiling point of the liquid. Which of the following processes produces the greatest increase in the entropy of the substance?

(Multiple Choice)

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Question 21

If ΔG° for a reaction is greater than zero, then .

(Multiple Choice)

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Question 22

Calculate OG^o(in kJ/mol) for the following reaction at 1 atm and 25^○C: OG_f^○C₂H₆(g) = - 32.89 kJ/mol; OG_f^○CO₂(g) = - 394.4 kJ/mol; OG_f^○H₂O (l) = - 237.2 kJ/mol

(Short Answer)

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Question 23

The value of ΔG° at 141.0 °C for the formation of phosphorous trichloride from its constituent elements, is kJ/mol. At 25.0 ^oC for this reaction, ΔH° is - 720.5 kJ/mol, ΔG° is - 642.9 kJ/mol, and ΔS° is - 263.7 J/K.

(Multiple Choice)

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Question 24

Use the table below to answer the questions that follow. Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) -The value of ΔH° for the decomposition of POCl₃into its constituent elements, is kJ/mol.

(Multiple Choice)

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Question 25

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 gaseous sulfur dioxide to solid elemental sulfur and gaseous oxygen, is J/K.

(Multiple Choice)

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Question 26

Which one of the following correctly indicates the relationship between the entropy of a system and the number of different arrangements, W, in the system?

(Multiple Choice)

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Question 27

Which reaction produces an increase in the entropy of the system?

(Multiple Choice)

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Question 28

Use the table below to answer the questions that follow. Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) -The value of ΔH° for the formation of POCl₃from its constituent elements, is kJ/mol.

(Multiple Choice)

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Question 29

The entropy of a pure crystalline substance at 0 ^oC is zero.

(True/False)

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Question 30

Of the following, only _ is not a state function.

(Multiple Choice)

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Question 31

For a given reaction, ΔH = - 19.9 kJ/mol and ΔS = - 55.5 J/K- mol. The reaction will have ΔG = 0 at------K. Assume that ΔH and ΔS do not vary with temperature.

(Multiple Choice)

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Question 32

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

(Multiple Choice)

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Question 33

The more negative OG^○is for a given reaction, the larger the value of the corresponding equilibrium constant, K.

(True/False)

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Question 34

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 ^oC for the decomposition of gaseous sulfur trioxide to solid elemental sulfur and gaseous oxygen, is kJ/mol.

(Multiple Choice)

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Question 35

With thermodynamics, one cannot determine .

(Multiple Choice)

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Question 36

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

(Multiple Choice)

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Question 37

A reaction that is not spontaneous at low temperature can become spontaneous at high temperature if OH is and OS is _ .

(Multiple Choice)

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Question 38

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

(Multiple Choice)

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Question 39

Which one of the following is always positive when a spontaneous process occurs?

(Multiple Choice)

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Question 40

Showing 21 - 40 of 101

Exam 19: Chemical Thermodynamics

Consider a pure crystalline solid that is heated from absolute zero to a temperature above the boiling point of the liquid. Which of the following processes produces the greatest increase in the entropy of the substance?

If ΔG° for a reaction is greater than zero, then .

Calculate OGo (in kJ/mol) for the following reaction at 1 atm and 25○C: OGf○C2H6 (g) = - 32.89 kJ/mol; OGf○CO2 (g) = - 394.4 kJ/mol; OGf○H2O (l) = - 237.2 kJ/mol

The value of ΔG° at 141.0 °C for the formation of phosphorous trichloride from its constituent elements, is kJ/mol. At 25.0 oC for this reaction, ΔH° is - 720.5 kJ/mol, ΔG° is - 642.9 kJ/mol, and ΔS° is - 263.7 J/K.

Use the table below to answer the questions that follow. Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) -The value of ΔH° for the decomposition of POCl3 into its constituent elements, 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 decomposition of gaseous sulfur dioxide to solid elemental sulfur and gaseous oxygen, is J/K.

Which one of the following correctly indicates the relationship between the entropy of a system and the number of different arrangements, W, in the system?

Which reaction produces an increase in the entropy of the 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 ΔH° for the formation of POCl3 from its constituent elements, is kJ/mol.

The entropy of a pure crystalline substance at 0 oC is zero.

Of the following, only _ is not a state function.

For a given reaction, ΔH = - 19.9 kJ/mol and ΔS = - 55.5 J/K- mol. The reaction will have ΔG = 0 at------K. Assume that ΔH and ΔS do not vary with temperature.

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

The more negative OG○is for a given reaction, the larger the value of the corresponding equilibrium constant, K.

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 oC for the decomposition of gaseous sulfur trioxide to solid elemental sulfur and gaseous oxygen, is kJ/mol.

With thermodynamics, one cannot determine .

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

A reaction that is not spontaneous at low temperature can become spontaneous at high temperature if OH is and OS is _ .

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

Which one of the following is always positive when a spontaneous process occurs?

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Calculate OG^o(in kJ/mol) for the following reaction at 1 atm and 25^○C: OG_f^○C₂H₆(g) = - 32.89 kJ/mol; OG_f^○CO₂(g) = - 394.4 kJ/mol; OG_f^○H₂O (l) = - 237.2 kJ/mol

The value of ΔG° at 141.0 °C for the formation of phosphorous trichloride from its constituent elements, is kJ/mol. At 25.0 ^oC for this reaction, ΔH° is - 720.5 kJ/mol, ΔG° is - 642.9 kJ/mol, and ΔS° is - 263.7 J/K.

Use the table below to answer the questions that follow. Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) -The value of ΔH° for the decomposition of POCl₃into its constituent elements, 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 ΔH° for the formation of POCl₃from its constituent elements, is kJ/mol.

The entropy of a pure crystalline substance at 0 ^oC is zero.

The more negative OG^○is for a given reaction, the larger the value of the corresponding equilibrium constant, K.

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 ^oC for the decomposition of gaseous sulfur trioxide to solid elemental sulfur and gaseous oxygen, is kJ/mol.