Hydrogen reacts with nitrogen to form ammonia (NH3) according to the reaction 3H2(g) + N2(g) $\leftrightarrow$ 2NH3(g) The value of $\Delta$H° is -92.38 kJ/mol, and that of $\Delta$S° is -198.2 J/(mol . K). Determine $\Delta$G° at 25°C.

A) +5.897 * 104 kJ/mol B) +297.8 kJ/mol C) -33.32 kJ/mol D) -16.66 kJ/mol E) +49.5 kJ/mol A) +5.897 * 104 kJ/mol B) +297.8 kJ/mol C) -33.32 kJ/mol D) -16.66 kJ/mol E) +49.5 kJ/mol

What is the overall standard free-energy change for the following two reactions? A + B $\rightarrow$ 2C $\Delta$G $\begin{array} { l } \circ\\ \text { rxn } \end{array}$ = $\Delta$G1 C + D $\rightarrow$ E $\Delta$G $\begin{array} { l } \circ\\ \text { rxn } \end{array}$ = $\Delta$G2

A) ($\Delta$G1 + $\Delta$G2) B) ($\Delta$G1 + 2$\Delta$G2) C) ($\Delta$G2 - $\Delta$G1) D) (2$\Delta$G2 - $\Delta$G1) E) ($\Delta$G1$\Delta$G22) A) ($\Delta$G1 + $\Delta$G2) B) ($\Delta$G1 + 2$\Delta$G2) C) ($\Delta$G2 - $\Delta$G1) D) (2$\Delta$G2 - $\Delta$G1) E) ($\Delta$G1$\Delta$G22)

Determine the entropy change for the reaction SO2(g) + \[\frac { 1 } { 2 }\] O2(g)$\rightarrow$SO3(g) given the following information: \[\begin{array} { l c } \text { Substance } & \boldsymbol { S } ^ { \circ } ( \mathbf { J } / \mathbf { m o l } \cdot \mathbf { K } ) \\ \mathrm { SO } _ { 2 } ( g ) & 248.2 \\ \mathrm { O } _ { 2 } ( g ) & 205.0 \\ \mathrm { SO } _ { 3 } ( g ) & 256.8 \end{array}\]

A) -196.4 J/K B) +196.4 J/K C) -93.9 J/K D) +93.9 J/K E) +401.4 J/K A) -196.4 J/K B) +196.4 J/K C) -93.9 J/K D) +93.9 J/K E) +401.4 J/K

Exam 18: Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Care must be taken when dissolving solid pellets of sodium hydroxide (NaOH) in water, because the temperature of the water can rise dramatically. Taking NaOH as the system, what can you deduce about the signs of the entropy change of the system ( $\Delta$ S_sys) and surroundings ( $\Delta$ S_surr) from this?

(Multiple Choice)

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Question 121

In the equation relating equilibrium to thermodynamics, a = -RTb,

(Multiple Choice)

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Question 122

Which of the following must be true for a spontaneous exothermic process?

(Multiple Choice)

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Question 123

Which of the following is in the correct order of standard state entropy? I.Diamond < graphite II.Liquid water < solid water III.NH₃ < H₂

(Multiple Choice)

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Question 124

Processes are always spontaneous when ________ (H and S refer to the system).

(Multiple Choice)

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Question 125

The equilibrium constant for a given reaction ________

(Multiple Choice)

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Question 126

A sketch of the free energy for a hypothetical chemical equilibrium is shown here. What part of the plot on the axis representing the relative quantities of reactants and products corresponds to a value of Q that is less than K?

(Multiple Choice)

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Question 127

The following figures represent distributions of two types of gas molecules between two containers connected by an open tube. In which figure is the entropy of the system maximized?

(Multiple Choice)

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Question 128

Several groups of general chemistry lab students measured the equilibrium constant for the same chemical equilibrium. In comparing their results, they found that they had different values because the temperatures of the experiments were different. Everyone was disappointed by the inconsistency, except for Dexter when he realized the measurements were made at different measured temperatures: "My esteemed colleagues," he said, "together we have sufficient data to determine two additional thermodynamic parameters and show the lab instructor what we know!" What two parameters did Dexter have in mind?

(Multiple Choice)

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Question 129

Which of the following statements is/are correct? A large negative free-energy change for a reaction means that ________ I. the equilibrium constant for the reaction is large. II. the equilibrium constant for the reaction is small. III. the reaction greatly favors formation of the products. IV. only a small amount of product is produced at equilibrium.

(Multiple Choice)

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Question 130

Suppose $\Delta$ G° is 25.0 kJ/mol for a hypothetical reaction in which A converts into B. Which of the following statements describes an equilibrium mixture of A and B?

(Multiple Choice)

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Question 131

Hydrogen reacts with nitrogen to form ammonia (NH₃) according to the reaction 3H₂(g) + N₂(g) $\leftrightarrow$ 2NH₃(g) The value of $\Delta$ H° is -92.38 kJ/mol, and that of $\Delta$ S° is -198.2 J/(mol . K). Determine $\Delta$ G° at 25°C.

(Multiple Choice)

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Question 132

What is the overall standard free-energy change for the following two reactions? A + B $\rightarrow$ 2C $\Delta$ G \circ rxn = $\Delta$ G₁ C + D $\rightarrow$ E $\Delta$ G \circ rxn = $\Delta$ G₂

(Multiple Choice)

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Question 133

Calcium sulfate is a desiccant used for storage of samples and equipment in a dry atmosphere because it absorbs water from air. The relevant thermodynamic reaction equation is given below. At what temperature will this reaction reverse to release the water and regenerate the dry desiccant? CaSO₄(s) + 2H₂O(g) $\rightarrow$ CaSO₄.H₂O(s) $\Delta$ H° = -104.9 kJ/mol, $\Delta$ S° = -291.2 J/(mol K)

(Multiple Choice)

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Question 134

Which of the following relationships are sufficient to ensure that reactants and products will be in their standard state at equilibrium? I. $\Delta$ G = 0 II. $\Delta$ G° = 0 III. K = 1

(Multiple Choice)

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Question 135

Determine the entropy change for the reaction SO₂(g) + $\frac { 1 } { 2 }$ O₂(g) $\rightarrow$ SO₃(g) given the following information: Substance (/\cdot) (g) 248.2 (g) 205.0 (g) 256.8

(Multiple Choice)

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Question 136

Values for $\Delta$ H° and $\Delta$ S° for a reaction can be determined experimentally by fitting a linear equation to a plot of on the x-axis and on the y-axis. The slope of this equation is equal to and the intercept allows us to calculate .

(Essay)

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Question 137

Because the triple point of water is 273 K, what must be true of the change in enthalpy and the change in entropy for ice converting to water at this temperature?

(Multiple Choice)

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Question 138

As T approaches infinity, ln K approaches ________

(Multiple Choice)

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Question 139

Hydrochloric acid (HCl) reacts with sodium hydroxide (NaOH) to form sodium chloride (NaCl) And water. If $\Delta$ H° = -56.13 kJ/mol and $\Delta$ S° = 79.11 J/mol . K, what is $\Delta$ G° for this reaction at 20°C?

(Multiple Choice)

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Question 140

Showing 121 - 140 of 157

In the equation relating equilibrium to thermodynamics, a = -RTb,

Which of the following must be true for a spontaneous exothermic process?

Which of the following is in the correct order of standard state entropy? I.Diamond < graphite II.Liquid water < solid water III.NH₃ < H₂

Processes are always spontaneous when ________ (H and S refer to the system).

The equilibrium constant for a given reaction ________

A sketch of the free energy for a hypothetical chemical equilibrium is shown here. What part of the plot on the axis representing the relative quantities of reactants and products corresponds to a value of Q that is less than K?

The following figures represent distributions of two types of gas molecules between two containers connected by an open tube. In which figure is the entropy of the system maximized?

Suppose $\Delta$ G° is 25.0 kJ/mol for a hypothetical reaction in which A converts into B. Which of the following statements describes an equilibrium mixture of A and B?

Hydrogen reacts with nitrogen to form ammonia (NH₃) according to the reaction 3H₂(g) + N₂(g) $\leftrightarrow$ 2NH₃(g) The value of $\Delta$ H° is -92.38 kJ/mol, and that of $\Delta$ S° is -198.2 J/(mol . K). Determine $\Delta$ G° at 25°C.

What is the overall standard free-energy change for the following two reactions? A + B $\rightarrow$ 2C $\Delta$ G \circ rxn = $\Delta$ G₁ C + D $\rightarrow$ E $\Delta$ G \circ rxn = $\Delta$ G₂

Which of the following relationships are sufficient to ensure that reactants and products will be in their standard state at equilibrium? I. $\Delta$ G = 0 II. $\Delta$ G° = 0 III. K = 1

Determine the entropy change for the reaction SO₂(g) + $\frac { 1 } { 2 }$ O₂(g) $\rightarrow$ SO₃(g) given the following information: Substance (/\cdot) (g) 248.2 (g) 205.0 (g) 256.8

Values for $\Delta$ H° and $\Delta$ S° for a reaction can be determined experimentally by fitting a linear equation to a plot of on the x-axis and on the y-axis. The slope of this equation is equal to and the intercept allows us to calculate .

Because the triple point of water is 273 K, what must be true of the change in enthalpy and the change in entropy for ice converting to water at this temperature?

As T approaches infinity, ln K approaches ________

Hydrochloric acid (HCl) reacts with sodium hydroxide (NaOH) to form sodium chloride (NaCl) And water. If $\Delta$ H° = -56.13 kJ/mol and $\Delta$ S° = 79.11 J/mol . K, what is $\Delta$ G° for this reaction at 20°C?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: the Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Structures and Applications

Organic Chemistry: Fuels, Pharmaceuticals, Materials, and Life

Chemical Kinetics: Reactions in the Air We Breathe

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acid-Base and Solubility Equilibria: Reactions in Soil and Water

Metal Ions: Colorful and Essential

Electrochemistry: the Quest for Clean Energy

Biochemistry: the Compounds of Life

Nuclear Chemistry: Applications to Energy and Medicine

Life and the Periodic Table

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Exam 18: Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

In the equation relating equilibrium to thermodynamics, a = -RTb,

Which of the following must be true for a spontaneous exothermic process?

Which of the following is in the correct order of standard state entropy? I.Diamond < graphite II.Liquid water < solid water III.NH3 < H2

Processes are always spontaneous when ________ (H and S refer to the system).

The equilibrium constant for a given reaction ________

A sketch of the free energy for a hypothetical chemical equilibrium is shown here. What part of the plot on the axis representing the relative quantities of reactants and products corresponds to a value of Q that is less than K?

The following figures represent distributions of two types of gas molecules between two containers connected by an open tube. In which figure is the entropy of the system maximized?

Suppose Δ\DeltaΔ G° is 25.0 kJ/mol for a hypothetical reaction in which A converts into B. Which of the following statements describes an equilibrium mixture of A and B?

Hydrogen reacts with nitrogen to form ammonia (NH3) according to the reaction 3H2(g) + N2(g) ↔\leftrightarrow↔ 2NH3(g) The value of Δ\DeltaΔ H° is -92.38 kJ/mol, and that of Δ\DeltaΔ S° is -198.2 J/(mol . K). Determine Δ\DeltaΔ G° at 25°C.

What is the overall standard free-energy change for the following two reactions? A + B →\rightarrow→ 2C Δ\DeltaΔ G \circ rxn = Δ\DeltaΔ G1 C + D →\rightarrow→ E Δ\DeltaΔ G \circ rxn = Δ\DeltaΔ G2

Which of the following relationships are sufficient to ensure that reactants and products will be in their standard state at equilibrium? I. Δ\DeltaΔ G = 0 II. Δ\DeltaΔ G° = 0 III. K = 1

Determine the entropy change for the reaction SO2(g) + 12\frac { 1 } { 2 }21​ O2(g) →\rightarrow→ SO3(g) given the following information: Substance (/\cdot) (g) 248.2 (g) 205.0 (g) 256.8

Values for Δ\DeltaΔ H° and Δ\DeltaΔ S° for a reaction can be determined experimentally by fitting a linear equation to a plot of ________ on the x-axis and ________ on the y-axis. The slope of this equation is equal to ________ and the intercept allows us to calculate ________.

Because the triple point of water is 273 K, what must be true of the change in enthalpy and the change in entropy for ice converting to water at this temperature?

As T approaches infinity, ln K approaches ________

Hydrochloric acid (HCl) reacts with sodium hydroxide (NaOH) to form sodium chloride (NaCl) And water. If Δ\DeltaΔ H° = -56.13 kJ/mol and Δ\DeltaΔ S° = 79.11 J/mol . K, what is Δ\DeltaΔ G° for this reaction at 20°C?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: the Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Structures and Applications

Organic Chemistry: Fuels, Pharmaceuticals, Materials, and Life

Chemical Kinetics: Reactions in the Air We Breathe

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acid-Base and Solubility Equilibria: Reactions in Soil and Water

Metal Ions: Colorful and Essential

Electrochemistry: the Quest for Clean Energy

Biochemistry: the Compounds of Life

Nuclear Chemistry: Applications to Energy and Medicine

Life and the Periodic Table

Filters

Which of the following is in the correct order of standard state entropy? I.Diamond < graphite II.Liquid water < solid water III.NH₃ < H₂

Suppose $\Delta$ G° is 25.0 kJ/mol for a hypothetical reaction in which A converts into B. Which of the following statements describes an equilibrium mixture of A and B?

Hydrogen reacts with nitrogen to form ammonia (NH₃) according to the reaction 3H₂(g) + N₂(g) $\leftrightarrow$ 2NH₃(g) The value of $\Delta$ H° is -92.38 kJ/mol, and that of $\Delta$ S° is -198.2 J/(mol . K). Determine $\Delta$ G° at 25°C.

What is the overall standard free-energy change for the following two reactions? A + B $\rightarrow$ 2C $\Delta$ G \circ rxn = $\Delta$ G₁ C + D $\rightarrow$ E $\Delta$ G \circ rxn = $\Delta$ G₂

Which of the following relationships are sufficient to ensure that reactants and products will be in their standard state at equilibrium? I. $\Delta$ G = 0 II. $\Delta$ G° = 0 III. K = 1

Determine the entropy change for the reaction SO₂(g) + $\frac { 1 } { 2 }$ O₂(g) $\rightarrow$ SO₃(g) given the following information: Substance (/\cdot) (g) 248.2 (g) 205.0 (g) 256.8

Values for $\Delta$ H° and $\Delta$ S° for a reaction can be determined experimentally by fitting a linear equation to a plot of on the x-axis and on the y-axis. The slope of this equation is equal to and the intercept allows us to calculate .

Hydrochloric acid (HCl) reacts with sodium hydroxide (NaOH) to form sodium chloride (NaCl) And water. If $\Delta$ H° = -56.13 kJ/mol and $\Delta$ S° = 79.11 J/mol . K, what is $\Delta$ G° for this reaction at 20°C?