Determine the normal melting point of benzoic acid in degrees centigrade given the following data: $\Delta$H $\begin{array} { l } \circ\\ \text { fus } \end{array}$ = 18.02 kJ/mol $\Delta$S $\begin{array} { l } \circ\\ \text { fus } \end{array}$ = 45.56 J/mol . K

The answer of Determine the normal melting point of benzoic...

The symbol $\Delta$G $\circ$ $f$ (CH4, g) refers to which of the following reactions?

A) CH4(l) $\rightarrow$CH4(g) B) CH4(g)$\rightarrow$CH4(l) C) CH4(g) $\rightarrow$C(g) + 4H(g) D) C(g) + 4H(g) $\rightarrow$CH4(g) E) C(s, graphite) + 2H2(g) $\rightarrow$ CH4(g) A) CH4(l) $\rightarrow$CH4(g) B) CH4(g)$\rightarrow$CH4(l) C) CH4(g) $\rightarrow$C(g) + 4H(g) D) C(g) + 4H(g) $\rightarrow$CH4(g) E) C(s, graphite) + 2H2(g) $\rightarrow$ CH4(g)

If 3.500 g of Ni are reacted with excess oxygen to form nickel oxide (NiO) under standard state conditions, what is the entropy change for the reaction? 2Ni(s) + O2 $\leftrightarrow$ 2NiO(s) $\begin{array}{lr} \text { Substance } & S^{\circ}(\mathbf{J} / \mathbf{m o l} \cdot \mathbf{K}) \\ \mathrm{Ni} & 182.1 \\ \mathrm{O}_{2} & 205.0 \\ \mathrm{NiO} &37.99 \end{array}$

A) -49.3 J/K B) -24.7 J/K C) -14.7 J/K D) +49.3 J/K E) -10.4 J/K A) -49.3 J/K B) -24.7 J/K C) -14.7 J/K D) +49.3 J/K E) -10.4 J/K

Which statement characterizes the following table? Temperature Dependence of Reaction Spontaneity \[\begin{array} { | l | l | l | } \hline & { \Delta S 0 } \\ \hline \Delta H 0 & \begin{array} { l } \text { Never spontaneous at any } \\ \text { temperature. } \end{array} & \begin{array} { l } \text { Spontaneous only at a sufficiently } \\ \text { low temperature. } \end{array} \\ \hline \end{array}\]

A) All entries are correct B) All entries are incorrect. C) One entry is incorrect. D) Two entries are incorrect. E) Three entries are incorrect. A) All entries are correct B) All entries are incorrect. C) One entry is incorrect. D) Two entries are incorrect. E) Three entries are incorrect.

Alcohols for use as biofuels can be produced from glucose that is obtained from starch and cellulose in plants. Use the information in the table below to determine the temperature range, if any, at which this reaction is spontaneous. C6H12O6(s) $\longrightarrow$2CH3CH2OH(l) + 2CO2(g) \[\begin{array} { | c | c | c | } \hline \text { Compound } & & \boldsymbol { S } ^ { \circ } \\ & \Delta H _ { \mathrm { f } } ^ { \circ } & { [ \mathbf { J } / ( \mathbf { m o l } \cdot \mathbf { K } ) ] } \\ \hline \text { Glucose } ( s ) & ( \mathrm { kJ } / \mathbf { m o l } ) & 212 \\ \hline \text { Ethanol } ( l ) & - 1,274 & 161 \\ \hline \text { Carbon dioxide } ( g ) & - 278 & 214 \\ \hline \end{array}\]

A) Reaction is spontaneous at high temperatures. B) Reaction is spontaneous at low temperatures. C) Reaction is spontaneous at all temperatures. D) Reaction is not spontaneous at any temperature. E) Whether the reaction is spontaneous or not cannot be predicted from the information provided. A) Reaction is spontaneous at high temperatures. B) Reaction is spontaneous at low temperatures. C) Reaction is spontaneous at all temperatures. D) Reaction is not spontaneous at any temperature. E) Whether the reaction is spontaneous or not cannot be predicted from the information provided.

Exam 18: Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

The values of $\Delta$ H°_rxn and $\Delta$ S°_rxn are shown for the following equilibrium reaction. What makes the equilibrium constant larger at low temperature? 2NO₂(g) $\leftrightarrows$ N₂O₄(g) $\Delta$ H $\degree$ = -58.02 kJ/mol, $\Delta$ S°=-176.5 J/mol .K

(Multiple Choice)

4.7/5

(27)

Question 61

The equilibrium vapor pressure for benzene is 94.4 mm Hg. When liquid benzene is in equilibrium with its vapor, we must have ________

(Multiple Choice)

4.9/5

(50)

Question 62

Determine the normal melting point of benzoic acid in degrees centigrade given the following data: $\Delta$ H \circ fus = 18.02 kJ/mol $\Delta$ S \circ fus = 45.56 J/mol . K

(Short Answer)

4.9/5

(44)

Question 63

Dinitrogen tetroxide (N₂O₄) decomposes to nitrogen dioxide (NO₂). If $\Delta$ H° = 58.02 kJ/mol and $\Delta$ S° = 176.1 J/mol · K, at what temperature are reactants and products in their standard states at equilibrium?

(Multiple Choice)

4.9/5

(37)

Question 64

Which of the following must be true for a reaction to proceed to form products?

(Multiple Choice)

4.8/5

(47)

Question 65

The heat of fusion for water is 333.6 J/g. What is the entropy change for the universe when 1.00 L of water at 0°C freezes at +5°C? Comment on the sign.

(Essay)

4.7/5

(37)

Question 66

The symbol $\Delta$ G $\circ$ $f$ (CH₄, g) refers to which of the following reactions?

(Multiple Choice)

4.7/5

(25)

Question 67

The standard free energy of formation, $\Delta G _ { f } ^ { 0 }$ , of atomic oxygen is 230.1 kJ/mol. Determine the equilibrium constant for the following reaction at standard thermodynamic conditions. O₂(g) $\leftrightarrows$ 2O(g)

(Multiple Choice)

4.7/5

(44)

Question 68

Draw a graph of entropy versus temperature for a typical substance. Be sure to clearly label phases and phase transitions on the graph.

(Essay)

4.8/5

(34)

Question 69

A sketch of the free energy versus Q for a hypothetical chemical equilibrium is shown here. The stress to the equilibrium by adding more reactants is shown by which arrow?

(Multiple Choice)

4.9/5

(38)

Question 70

Indicate which one of the following reactions results in a positive $\Delta$ S_sys.

(Multiple Choice)

4.9/5

(28)

Question 71

In a spontaneous process, the entropy of the universe ________

(Multiple Choice)

4.7/5

(28)

Question 72

Which of the following statements about equilibrium are true? I. $\Delta$ G_sys = 0 II. $\Delta$ S_sys = 0 III. $\Delta$ S_universe = 0

(Multiple Choice)

4.9/5

(36)

Question 73

The standard entropy of nitrogen gas in air is 192 J/(mol . K). Estimate how many states are accessible to a nitrogen molecule in air.

(Multiple Choice)

4.9/5

(36)

Question 74

If 3.500 g of Ni are reacted with excess oxygen to form nickel oxide (NiO) under standard state conditions, what is the entropy change for the reaction? 2Ni(s) + O₂ $\leftrightarrow$ 2NiO(s) Substance (/\cdot) 182.1 205.0 37.99

(Multiple Choice)

4.9/5

(33)

Question 75

A perturbation or stress to a chemical reaction at equilibrium ________

(Multiple Choice)

4.9/5

(38)

Question 76

Which statement characterizes the following table? Temperature Dependence of Reaction Spontaneity \DeltaS<0 \DeltaS>0 \DeltaH<0 Spontaneous only at a sufficiently high temperature. Always spontaneous at any temperature. \DeltaH>0 Never spontaneous at any temperature. Spontaneous only at a sufficiently low temperature.

(Multiple Choice)

4.9/5

(41)

Question 77

Alcohols for use as biofuels can be produced from glucose that is obtained from starch and cellulose in plants. Use the information in the table below to determine the temperature range, if any, at which this reaction is spontaneous. C₆H₁₂O₆(s) $\longrightarrow$ 2CH₃CH₂OH(l) + 2CO₂(g) Compound \Delta [/(\cdot)] Glucose (s) (/) 212 Ethanol (l) -1,274 161 Carbon dioxide (g) -278 214

(Multiple Choice)

4.8/5

(32)

Question 78

The entropy of vaporization of water is 109.0 J/mol · K. What is the enthalpy of vaporization of water at its normal boiling point?

(Multiple Choice)

4.7/5

(40)

Question 79

What types of motion does a molecule of chlorine have?

(Multiple Choice)

4.8/5

(43)

Question 80

Showing 61 - 80 of 157

The values of $\Delta$ H°_rxn and $\Delta$ S°_rxn are shown for the following equilibrium reaction. What makes the equilibrium constant larger at low temperature? 2NO₂(g) $\leftrightarrows$ N₂O₄(g) $\Delta$ H $\degree$ = -58.02 kJ/mol, $\Delta$ S°=-176.5 J/mol .K

The equilibrium vapor pressure for benzene is 94.4 mm Hg. When liquid benzene is in equilibrium with its vapor, we must have ________

Determine the normal melting point of benzoic acid in degrees centigrade given the following data: $\Delta$ H \circ fus = 18.02 kJ/mol $\Delta$ S \circ fus = 45.56 J/mol . K

Dinitrogen tetroxide (N₂O₄) decomposes to nitrogen dioxide (NO₂). If $\Delta$ H° = 58.02 kJ/mol and $\Delta$ S° = 176.1 J/mol · K, at what temperature are reactants and products in their standard states at equilibrium?

Which of the following must be true for a reaction to proceed to form products?

The heat of fusion for water is 333.6 J/g. What is the entropy change for the universe when 1.00 L of water at 0°C freezes at +5°C? Comment on the sign.

The symbol $\Delta$ G $\circ$ $f$ (CH₄, g) refers to which of the following reactions?

The standard free energy of formation, $\Delta G _ { f } ^ { 0 }$ , of atomic oxygen is 230.1 kJ/mol. Determine the equilibrium constant for the following reaction at standard thermodynamic conditions. O₂(g) $\leftrightarrows$ 2O(g)

Draw a graph of entropy versus temperature for a typical substance. Be sure to clearly label phases and phase transitions on the graph.

A sketch of the free energy versus Q for a hypothetical chemical equilibrium is shown here. The stress to the equilibrium by adding more reactants is shown by which arrow?

Indicate which one of the following reactions results in a positive $\Delta$ S_sys.

In a spontaneous process, the entropy of the universe ________

Which of the following statements about equilibrium are true? I. $\Delta$ G_sys = 0 II. $\Delta$ S_sys = 0 III. $\Delta$ S_universe = 0

The standard entropy of nitrogen gas in air is 192 J/(mol . K). Estimate how many states are accessible to a nitrogen molecule in air.

If 3.500 g of Ni are reacted with excess oxygen to form nickel oxide (NiO) under standard state conditions, what is the entropy change for the reaction? 2Ni(s) + O₂ $\leftrightarrow$ 2NiO(s) Substance (/\cdot) 182.1 205.0 37.99

A perturbation or stress to a chemical reaction at equilibrium ________

The entropy of vaporization of water is 109.0 J/mol · K. What is the enthalpy of vaporization of water at its normal boiling point?

What types of motion does a molecule of chlorine have?

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

Exam 18: Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

The values of Δ\DeltaΔ H°rxn and Δ\DeltaΔ S°rxn are shown for the following equilibrium reaction. What makes the equilibrium constant larger at low temperature? 2NO2(g) ⇆\leftrightarrows ⇆ N2O4(g) Δ\DeltaΔ H °\degree° = -58.02 kJ/mol, Δ\DeltaΔ S°=-176.5 J/mol .K

The equilibrium vapor pressure for benzene is 94.4 mm Hg. When liquid benzene is in equilibrium with its vapor, we must have ________

Determine the normal melting point of benzoic acid in degrees centigrade given the following data: Δ\DeltaΔ H \circ fus = 18.02 kJ/mol Δ\DeltaΔ S \circ fus = 45.56 J/mol . K

Dinitrogen tetroxide (N2O4) decomposes to nitrogen dioxide (NO2). If Δ\DeltaΔ H° = 58.02 kJ/mol and Δ\DeltaΔ S° = 176.1 J/mol · K, at what temperature are reactants and products in their standard states at equilibrium?

Which of the following must be true for a reaction to proceed to form products?

The heat of fusion for water is 333.6 J/g. What is the entropy change for the universe when 1.00 L of water at 0°C freezes at +5°C? Comment on the sign.

The symbol Δ\DeltaΔ G ∘\circ∘ fff (CH4, g) refers to which of the following reactions?

The standard free energy of formation, ΔGf0\Delta G _ { f } ^ { 0 }ΔGf0​ , of atomic oxygen is 230.1 kJ/mol. Determine the equilibrium constant for the following reaction at standard thermodynamic conditions. O2(g) ⇆\leftrightarrows⇆ 2O(g)

Draw a graph of entropy versus temperature for a typical substance. Be sure to clearly label phases and phase transitions on the graph.

A sketch of the free energy versus Q for a hypothetical chemical equilibrium is shown here. The stress to the equilibrium by adding more reactants is shown by which arrow?

Indicate which one of the following reactions results in a positive Δ\DeltaΔ Ssys.

In a spontaneous process, the entropy of the universe ________

Which of the following statements about equilibrium are true? I. Δ\DeltaΔ Gsys = 0 II. Δ\DeltaΔ Ssys = 0 III. Δ\DeltaΔ Suniverse = 0

The standard entropy of nitrogen gas in air is 192 J/(mol . K). Estimate how many states are accessible to a nitrogen molecule in air.

If 3.500 g of Ni are reacted with excess oxygen to form nickel oxide (NiO) under standard state conditions, what is the entropy change for the reaction? 2Ni(s) + O2 ↔\leftrightarrow↔ 2NiO(s) Substance (/\cdot) 182.1 205.0 37.99

A perturbation or stress to a chemical reaction at equilibrium ________

The entropy of vaporization of water is 109.0 J/mol · K. What is the enthalpy of vaporization of water at its normal boiling point?

What types of motion does a molecule of chlorine have?

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

The values of $\Delta$ H°_rxn and $\Delta$ S°_rxn are shown for the following equilibrium reaction. What makes the equilibrium constant larger at low temperature? 2NO₂(g) $\leftrightarrows$ N₂O₄(g) $\Delta$ H $\degree$ = -58.02 kJ/mol, $\Delta$ S°=-176.5 J/mol .K

Determine the normal melting point of benzoic acid in degrees centigrade given the following data: $\Delta$ H \circ fus = 18.02 kJ/mol $\Delta$ S \circ fus = 45.56 J/mol . K

Dinitrogen tetroxide (N₂O₄) decomposes to nitrogen dioxide (NO₂). If $\Delta$ H° = 58.02 kJ/mol and $\Delta$ S° = 176.1 J/mol · K, at what temperature are reactants and products in their standard states at equilibrium?

The symbol $\Delta$ G $\circ$ $f$ (CH₄, g) refers to which of the following reactions?

The standard free energy of formation, $\Delta G _ { f } ^ { 0 }$ , of atomic oxygen is 230.1 kJ/mol. Determine the equilibrium constant for the following reaction at standard thermodynamic conditions. O₂(g) $\leftrightarrows$ 2O(g)

Indicate which one of the following reactions results in a positive $\Delta$ S_sys.

Which of the following statements about equilibrium are true? I. $\Delta$ G_sys = 0 II. $\Delta$ S_sys = 0 III. $\Delta$ S_universe = 0

If 3.500 g of Ni are reacted with excess oxygen to form nickel oxide (NiO) under standard state conditions, what is the entropy change for the reaction? 2Ni(s) + O₂ $\leftrightarrow$ 2NiO(s) Substance (/\cdot) 182.1 205.0 37.99