Using the thermodynamic data provided below, calculate Ka2 for H2CO3(aq) at 25$\circ$. $\begin{array}{|l|c|c|} \hline & \Delta \mathrm{H}_{\mathrm{f}}^{\circ}(\mathrm{kJ} / \mathrm{mol}) & \mathrm{S}^{\circ}(\mathrm{J} / \mathrm{K} \cdot \mathrm{~mol}) \\ \hline \mathrm{H}^{+}(a q) & 0 & 0 \\ \hline \mathrm{H}_{2} \mathrm{CO}_{3}(a q) & -698.7 & 191 \\ \hline \mathrm{HCO}_{3}^{-}(a q) & -691.11 & 95.0 \\ \hline \mathrm{CO}_{3}^{2-}(a q) & -676.26 & -53.1 \\ \hline \end{array}$

A) 4.09 * 10-11 B) 4.39 * 10-9 C) 4.59 * 10-10 D) 4.59 * 10-11 E) None of the above A) 4.09 * 10-11 B) 4.39 * 10-9 C) 4.59 * 10-10 D) 4.59 * 10-11 E) None of the above

Which response includes all of the following processes that are accompanied by an increase in entropy 1) I2(s) $\rarr$I2(g) 2) 2I(g) $\rarr$ I2(g) 3) 2NH3(g) $\rarr$ N2(g) + 3H2(g) 4) Mg2+(aq) + 2OH-(aq) $\rarr$Mg(OH)2(s)

A) 1, 2 B) 1, 3 C) 3, 4 D) 3 E) 2, 4 A) 1, 2 B) 1, 3 C) 3, 4 D) 3 E) 2, 4

Given the following data, estimate the boiling point of carbon disulfide, CS2, assuming that $\Delta$S$\circ$ and $\Delta$H$\circ$ are temperature-independent. $\begin{array}{|l|c|c|} \hline & \Delta \mathrm{H}^{\circ}_f(\mathrm{kJ} / \mathrm{mol}) & \mathrm{S}^{\circ}(\mathrm{J} / \mathrm{K} \cdot \mathrm{~mol}) \\ \hline \mathrm{CS}_{2}(g) & 115.3 & 237.8 \\ \hline \mathrm{CS}_{2}(l) & 87.3 & 151.0 \\ \hline \end{array}$

A) 47.4$\circ$C B) 49.4$\circ$C C) 51.4$\circ$C D) 53.4$\circ$C E) None of the above A) 47.4$\circ$C B) 49.4$\circ$C C) 51.4$\circ$C D) 53.4$\circ$C E) None of the above

Using the thermodynamic data provided below, determine the temperature in $\circ$C at which the decomposition of solid calcium carbonate to form solid calcium oxide and oxygen becomes spontaneous. $\begin{array}{|l|c|c|} \hline & \Delta \mathrm{H}_{\mathrm{f}}^{\circ}(\mathrm{kJ} / \mathrm{mol}) & \mathrm{S}^{\circ}(\mathrm{J} / \mathrm{K} \cdot \mathrm{~mol}) \\ \hline \mathrm{CO}_{2}(\mathrm{g}) & -393.5 & 213.6 \\ \hline \mathrm{CaO}(\mathrm{s}) & -635.6 & 39.8 \\ \hline \mathrm{CaCO}_{3}(\mathrm{s}) & -1206.9 & 92.9 \\ \hline \end{array}$

A) 834.6$\circ$C B) 814.6$\circ$C C) 794.6$\circ$C D) 774.6$\circ$C E) None of the above A) 834.6$\circ$C B) 814.6$\circ$C C) 794.6$\circ$C D) 774.6$\circ$C E) None of the above

Exam 17: Entropy Free Energy and Equilibrium

Using the thermodynamic data provided below, calculate K_a2 for H₂CO₃(aq) at 25^$\circ$. \Delta(/) (/\cdot) (aq) 0 0 (aq) -698.7 191 (aq) -691.11 95.0 (aq) -676.26 -53.1

(Multiple Choice)

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Question 121

Which response includes all of the following processes that are accompanied by an increase in entropy 1) I₂(s) $\rarr$ I₂(g) 2) 2I(g) $\rarr$ I₂(g) 3) 2NH₃(g) $\rarr$ N₂(g) + 3H₂(g) 4) Mg²⁺(aq) + 2OH^-(aq) $\rarr$ Mg(OH)₂(s)

(Multiple Choice)

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Question 122

Given the following data, estimate the boiling point of carbon disulfide, CS₂, assuming that $\Delta$ S^$\circ$ and $\Delta$ H^$\circ$ are temperature-independent. \Delta(/) (/\cdot) (g) 115.3 237.8 (l) 87.3 151.0

(Multiple Choice)

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Question 123

Which one of the following reactions would you expect to have highest $\Delta$ S^$\circ$

(Multiple Choice)

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Question 124

The following reaction is spontaneous under standard state conditions at 25^$\circ$C: AgCl(s) $\rarr$ Ag⁺(aq) + Cl^-(aq) ( $\Delta$ G^$\circ$ = 55 kJ/mol).

(True/False)

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Question 125

The standard entropy of any pure substance is 0 J/mol.

(True/False)

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Question 126

The reaction rates of many spontaneous reactions are actually very slow. Which of these statements is the best explanation for this observation

(Multiple Choice)

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Question 127

Using the thermodynamic data provided below, determine the temperature in ^$\circ$C at which the decomposition of solid calcium carbonate to form solid calcium oxide and oxygen becomes spontaneous. \Delta(/) (/\cdot) () -393.5 213.6 () -635.6 39.8 () -1206.9 92.9

(Multiple Choice)

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Question 128

Using the thermodynamic data provided below, calculate K_a2 for H₂CO₃(aq) at 25^$\circ$. \Delta(/) (/\cdot) (aq) 0 0 (aq) -698.7 191 (aq) -691.11 95.0 (aq) -676.26 -53.1

Which response includes all of the following processes that are accompanied by an increase in entropy 1) I₂(s) $\rarr$ I₂(g) 2) 2I(g) $\rarr$ I₂(g) 3) 2NH₃(g) $\rarr$ N₂(g) + 3H₂(g) 4) Mg²⁺(aq) + 2OH^-(aq) $\rarr$ Mg(OH)₂(s)

Given the following data, estimate the boiling point of carbon disulfide, CS₂, assuming that $\Delta$ S^$\circ$ and $\Delta$ H^$\circ$ are temperature-independent. \Delta(/) (/\cdot) (g) 115.3 237.8 (l) 87.3 151.0

Which one of the following reactions would you expect to have highest $\Delta$ S^$\circ$

The following reaction is spontaneous under standard state conditions at 25^$\circ$C: AgCl(s) $\rarr$ Ag⁺(aq) + Cl^-(aq) ( $\Delta$ G^$\circ$ = 55 kJ/mol).

The standard entropy of any pure substance is 0 J/mol.

The reaction rates of many spontaneous reactions are actually very slow. Which of these statements is the best explanation for this observation

Using the thermodynamic data provided below, determine the temperature in ^$\circ$C at which the decomposition of solid calcium carbonate to form solid calcium oxide and oxygen becomes spontaneous. \Delta(/) (/\cdot) () -393.5 213.6 () -635.6 39.8 () -1206.9 92.9

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Chemical Kinetics

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Acid-Base Equilibria and Solubility Equilibria

Electrochemistry

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Exam 17: Entropy Free Energy and Equilibrium

Using the thermodynamic data provided below, calculate Ka2 for H2CO3(aq) at 25 ∘\circ∘ . \Delta(/) (/\cdot) (aq) 0 0 (aq) -698.7 191 (aq) -691.11 95.0 (aq) -676.26 -53.1

Which response includes all of the following processes that are accompanied by an increase in entropy 1) I2(s) →\rarr→ I2(g) 2) 2I(g) →\rarr→ I2(g) 3) 2NH3(g) →\rarr→ N2(g) + 3H2(g) 4) Mg2+(aq) + 2OH-(aq) →\rarr→ Mg(OH)2(s)

Given the following data, estimate the boiling point of carbon disulfide, CS2, assuming that Δ\DeltaΔ S ∘\circ∘ and Δ\DeltaΔ H ∘\circ∘ are temperature-independent. \Delta(/) (/\cdot) (g) 115.3 237.8 (l) 87.3 151.0

Which one of the following reactions would you expect to have highest Δ\DeltaΔ S ∘\circ∘

The following reaction is spontaneous under standard state conditions at 25 ∘\circ∘ C: AgCl(s) →\rarr→ Ag+(aq) + Cl-(aq) ( Δ\DeltaΔ G ∘\circ∘ = 55 kJ/mol).

The standard entropy of any pure substance is 0 J/mol.

The reaction rates of many spontaneous reactions are actually very slow. Which of these statements is the best explanation for this observation

Using the thermodynamic data provided below, determine the temperature in ∘\circ∘ C at which the decomposition of solid calcium carbonate to form solid calcium oxide and oxygen becomes spontaneous. \Delta(/) (/\cdot) () -393.5 213.6 () -635.6 39.8 () -1206.9 92.9

Chemistry: The Study of Change

Atoms Molecules and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solutions

Gases

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Periodic Relationships Among the Elements

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Hybridization of Atomic

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Electrochemistry

Nuclear Chemistry

Chemistry in the Atmosphere

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Transition Metals Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

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Using the thermodynamic data provided below, calculate K_a2 for H₂CO₃(aq) at 25^$\circ$. \Delta(/) (/\cdot) (aq) 0 0 (aq) -698.7 191 (aq) -691.11 95.0 (aq) -676.26 -53.1

Which response includes all of the following processes that are accompanied by an increase in entropy 1) I₂(s) $\rarr$ I₂(g) 2) 2I(g) $\rarr$ I₂(g) 3) 2NH₃(g) $\rarr$ N₂(g) + 3H₂(g) 4) Mg²⁺(aq) + 2OH^-(aq) $\rarr$ Mg(OH)₂(s)

Given the following data, estimate the boiling point of carbon disulfide, CS₂, assuming that $\Delta$ S^$\circ$ and $\Delta$ H^$\circ$ are temperature-independent. \Delta(/) (/\cdot) (g) 115.3 237.8 (l) 87.3 151.0

Which one of the following reactions would you expect to have highest $\Delta$ S^$\circ$

The following reaction is spontaneous under standard state conditions at 25^$\circ$C: AgCl(s) $\rarr$ Ag⁺(aq) + Cl^-(aq) ( $\Delta$ G^$\circ$ = 55 kJ/mol).

Using the thermodynamic data provided below, determine the temperature in ^$\circ$C at which the decomposition of solid calcium carbonate to form solid calcium oxide and oxygen becomes spontaneous. \Delta(/) (/\cdot) () -393.5 213.6 () -635.6 39.8 () -1206.9 92.9