Predict the sign of $\Delta$S for the reaction 6CO2(g)+ 6H2O(g)$\to$ C6H12O6(g)+ 6O2(g).

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For the reaction SbCl5(g) SbCl3(g)+ Cl2(g), $\Delta$G°f (SbCl5)= -334.34 kJ/mol $\Delta$G°f (SbCl3)= -301.25 kJ/mol $\Delta$H°f (SbCl5)= -394.34 kJ/mol $\Delta$H°f (SbCl3)= -313.80 kJ/mol Will this reaction proceed spontaneously at 298 K and 1 atm pressure?

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Calculate $\Delta$S° for the reaction SO2(s)+ NO2(g)$\to$SO3(g)+ NO(g).

A) 53.6 J/K·mol B) -53.6 J/K·mol C) -22.2 J/K·mol D) 474.8 J/K·mol E) -474.8 J/K·mol A) 53.6 J/K·mol B) -53.6 J/K·mol C) -22.2 J/K·mol D) 474.8 J/K·mol E) -474.8 J/K·mol

Aluminum forms a layer of aluminum oxide when exposed to air which protects the bulk metal from further corrosion. 4Al(s)+ 3O2(g)$\to$2Al2O3(s) Calculate $\Delta$G° for this reaction, given that $\Delta$G°f of aluminum oxide is -1576.4 kJ/mol.

A) -3152.8 kJ/mol B) -1576.4 kJ/mol C) -788.2 kJ/mol D) 1576.4 kJ/mol E) 3152.8 kJ/mol A) -3152.8 kJ/mol B) -1576.4 kJ/mol C) -788.2 kJ/mol D) 1576.4 kJ/mol E) 3152.8 kJ/mol

Find the temperature at which Kp = 4.00 for the reaction N2O4(g) 2NO2(g).[Given: at 25°C, for NO2(g), $\Delta$H°f = 33.85 kJ/mol, S° = 240.46 J/mol·K; for N2O4(g), $\Delta$H°f = 9.66 kJ/mol, S° = 304.3 J/mol·K; assume that$\Delta$H° and $\Delta$S° are independent of temperature.]

A) 197 °C B) 56 °C C) 36 °C D) 79 °C E) 476°C A) 197 °C B) 56 °C C) 36 °C D) 79 °C E) 476°C

Predict the normal boiling point of triethylborane (C6H15B)using the following data:

A) 92°C B) -21°C C) 21°C D) 365°C E) 256°C A) 92°C B) -21°C C) 21°C D) 365°C E) 256°C

Arrange these reactions according to increasing $\Delta$S. 1)H2O(g)$\to$ H2O(l) 2)2NO(g)$\to$ N2(g)+ O2(g) 3)MgCO3(s)$\to$MgO(s)+ CO2(g)

A) 1 < 2 < 3 B) 2 < 3 < 1 C) 3 < 2 < 1 D) 2 < 1 < 3 E) 1 < 3 < 2 A) 1 < 2 < 3 B) 2 < 3 < 1 C) 3 < 2 < 1 D) 2 < 1 < 3 E) 1 < 3 < 2

For the reaction HCONH2(g) NH3(g)+ CO(g), Kc = 4.84 at 400 K. If $\Delta$H° for this reaction is 29 kJ/mol, find Kc at 500 K.

A) 5.8 B) 0.17 C) 27 D) 0.88 E) 10.3 A) 5.8 B) 0.17 C) 27 D) 0.88 E) 10.3

Calculate Kp at 298 K for the reaction SO2(g)+ NO2(g)$\to$ SO3(g)+ NO(g).

A) 6.99 $\times$ 10-7 B) 5.71 $\times$ 10-8 C) 14.2 D) 475 E) 1.42 $\times$ 106 A) 6.99 $\times$ 10-7 B) 5.71 $\times$ 10-8 C) 14.2 D) 475 E) 1.42 $\times$ 106

Exam 18: Entropy, Free Energy, and Equilibrium

For the reaction CuS(s)+ H₂(g) $For the reaction CuS(s)+ H2(g) H2S(g)+ Cu(s), \Delta G°f (CuS)= -53.6 kJ/mol \Delta G°f (H2S)= -33.6 kJ/mol \Delta H°f (CuS)= -53.1 kJ/mol \Delta H°f (H2S)= - 20.6 kJ/mol Will this reaction proceed spontaneously at 298 K and 1 atm pressure?$ H₂S(g)+ Cu(s), $\Delta$ G°_f (CuS)= -53.6 kJ/mol $\Delta$ G°_f (H₂S)= -33.6 kJ/mol $\Delta$ H°_f (CuS)= -53.1 kJ/mol $\Delta$ H°_f (H₂S)= - 20.6 kJ/mol Will this reaction proceed spontaneously at 298 K and 1 atm pressure?

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Question 1

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The entropy change on vaporization ( $\Delta$ S_vap)of a compound or element is

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The element oxygen was prepared by Joseph Priestley in 1774 by heating mercury(II)oxide: HgO(s)\9\to\) Hg(l)+ ¹/₂O₂(g), $\Delta$ H° = 90.84 kJ/mol. Estimate the temperature at which this reaction will become spontaneous under standard state conditions. S°(Hg)= 76.02 J/K·mol S°(O₂)= 205.0 J/K·mol S°(HgO)= 70.29 J/K·mol

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Rubidium has a heat of vaporization of 69.0 kJ/mol at its boiling point (686°C).Calculate $\Delta$ S for this process, Rb(l) $\to$ Rb(g), at 1 atm and 686°C.

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Question 4

Predict the sign of $\Delta$ S for the reaction 6CO₂(g)+ 6H₂O(g) $\to$ C₆H₁₂O₆(g)+ 6O₂(g).

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Question 5

For the reaction SbCl₅(g) $For the reaction SbCl5(g) SbCl3(g)+ Cl2(g), \Delta G°f (SbCl5)= -334.34 kJ/mol \Delta G°f (SbCl3)= -301.25 kJ/mol \Delta H°f (SbCl5)= -394.34 kJ/mol \Delta H°f (SbCl3)= -313.80 kJ/mol Will this reaction proceed spontaneously at 298 K and 1 atm pressure?$ SbCl₃(g)+ Cl₂(g), $\Delta$ G°_f (SbCl₅)= -334.34 kJ/mol $\Delta$ G°_f (SbCl₃)= -301.25 kJ/mol $\Delta$ H°_f (SbCl₅)= -394.34 kJ/mol $\Delta$ H°_f (SbCl₃)= -313.80 kJ/mol Will this reaction proceed spontaneously at 298 K and 1 atm pressure?

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Question 6

Calculate $\Delta$ S° for the reaction SO₂(s)+ NO₂(g) $\to$ SO₃(g)+ NO(g). $Calculate \Delta S° for the reaction SO2(s)+ NO2(g) \to SO3(g)+ NO(g).$

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Question 7

Choose the substance with the higher entropy per mole at a given temperature: 1 mole of N₂(g)in a 22.4 L container or 1 mole of N₂(g)in a 2.24 L container.

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Question 8

A sample of solid naphthalene is introduced into an evacuated flask. Use the data below to calculate the equilibrium vapor pressure of naphthalene (C₁₀H₈)in the flask at 35°C.

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Question 9

The heat of vaporization of water is 2.27 kJ/g. What is $\Delta$ S_vap per mole at the normal boiling point?

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Question 10

For a given substance the entropy always increases in the following order: S (gas)< S (liq)< S (solid).

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Question 11

$\Delta$ H_vap for ethanol is 38.7 kJ/mol at its boiling point (78°C).What is $\Delta$ S_surr when 1.00 mole of ethanol is boiled?

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Question 12

Aluminum forms a layer of aluminum oxide when exposed to air which protects the bulk metal from further corrosion. 4Al(s)+ 3O₂(g) $\to$ 2Al₂O₃(s) Calculate $\Delta$ G° for this reaction, given that $\Delta$ G°_f of aluminum oxide is -1576.4 kJ/mol.

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Question 13

Find the temperature at which K_p = 4.00 for the reaction N₂O₄(g) $Find the temperature at which Kp = 4.00 for the reaction N2O4(g) 2NO2(g).[Given: at 25°C, for NO2(g), \Delta H°f = 33.85 kJ/mol, S° = 240.46 J/mol·K; for N2O4(g), \Delta H°f = 9.66 kJ/mol, S° = 304.3 J/mol·K; assume that \Delta H° and \Delta S° are independent of temperature.]$ 2NO₂(g).[Given: at 25°C, for NO₂(g), $\Delta$ H°_f = 33.85 kJ/mol, S° = 240.46 J/mol·K; for N₂O₄(g), $\Delta$ H°_f = 9.66 kJ/mol, S° = 304.3 J/mol·K; assume that $\Delta$ H° and $\Delta$ S° are independent of temperature.]

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Question 14

Predict the normal boiling point of triethylborane (C₆H₁₅B)using the following data:

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Question 15

Arrange these reactions according to increasing $\Delta$ S. 1)H₂O(g) $\to$ H₂O(l) 2)2NO(g) $\to$ N₂(g)+ O₂(g) 3)MgCO₃(s) $\to$ MgO(s)+ CO₂(g)

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Question 16

The entropy change $\times$ S° for the reaction NH₄Cl(s) $\to$ NH₃(g)+ HCl(g)will be negative.

(True/False)

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Question 17

For the reaction HCONH₂(g) $For the reaction HCONH2(g) NH3(g)+ CO(g), Kc = 4.84 at 400 K. If \Delta H° for this reaction is 29 kJ/mol, find Kc at 500 K.$ NH₃(g)+ CO(g), K_c = 4.84 at 400 K. If $\Delta$ H° for this reaction is 29 kJ/mol, find K_c at 500 K.

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Question 18

Calculate K_p at 298 K for the reaction SO₂(g)+ NO₂(g) $\to$ SO₃(g)+ NO(g). $Calculate Kp at 298 K for the reaction SO2(g)+ NO2(g) \to SO3(g)+ NO(g).$

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Question 19

Using the thermodynamic data provided below, calculate K_a2 for H₂CO₃(aq)at 25°.

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Question 20

Showing 1 - 20 of 112

The entropy change on vaporization ( $\Delta$ S_vap)of a compound or element is

Rubidium has a heat of vaporization of 69.0 kJ/mol at its boiling point (686°C).Calculate $\Delta$ S for this process, Rb(l) $\to$ Rb(g), at 1 atm and 686°C.

Predict the sign of $\Delta$ S for the reaction 6CO₂(g)+ 6H₂O(g) $\to$ C₆H₁₂O₆(g)+ 6O₂(g).

Calculate $\Delta$ S° for the reaction SO₂(s)+ NO₂(g) $\to$ SO₃(g)+ NO(g). $Calculate \Delta S° for the reaction SO<sub>2</sub>(s)+ NO<sub>2</sub>(g) \to SO<sub>3</sub>(g)+ NO(g).$

Choose the substance with the higher entropy per mole at a given temperature: 1 mole of N₂(g)in a 22.4 L container or 1 mole of N₂(g)in a 2.24 L container.

A sample of solid naphthalene is introduced into an evacuated flask. Use the data below to calculate the equilibrium vapor pressure of naphthalene (C₁₀H₈)in the flask at 35°C.

The heat of vaporization of water is 2.27 kJ/g. What is $\Delta$ S_vap per mole at the normal boiling point?

For a given substance the entropy always increases in the following order: S (gas)< S (liq)< S (solid).

$\Delta$ H_vap for ethanol is 38.7 kJ/mol at its boiling point (78°C).What is $\Delta$ S_surr when 1.00 mole of ethanol is boiled?

Aluminum forms a layer of aluminum oxide when exposed to air which protects the bulk metal from further corrosion. 4Al(s)+ 3O₂(g) $\to$ 2Al₂O₃(s) Calculate $\Delta$ G° for this reaction, given that $\Delta$ G°_f of aluminum oxide is -1576.4 kJ/mol.

Predict the normal boiling point of triethylborane (C₆H₁₅B)using the following data:

Arrange these reactions according to increasing $\Delta$ S. 1)H₂O(g) $\to$ H₂O(l) 2)2NO(g) $\to$ N₂(g)+ O₂(g) 3)MgCO₃(s) $\to$ MgO(s)+ CO₂(g)

The entropy change $\times$ S° for the reaction NH₄Cl(s) $\to$ NH₃(g)+ HCl(g)will be negative.

Calculate K_p at 298 K for the reaction SO₂(g)+ NO₂(g) $\to$ SO₃(g)+ NO(g). $Calculate K<sub>p</sub> at 298 K for the reaction SO<sub>2</sub>(g)+ NO<sub>2</sub>(g) \to SO<sub>3</sub>(g)+ NO(g).$

Using the thermodynamic data provided below, calculate K_a2 for H₂CO₃(aq)at 25°.

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Exam 18: Entropy, Free Energy, and Equilibrium

For the reaction CuS(s)+ H2(g) H2S(g)+ Cu(s), Δ\DeltaΔ G°f (CuS)= -53.6 kJ/mol Δ\DeltaΔ G°f (H2S)= -33.6 kJ/mol Δ\DeltaΔ H°f (CuS)= -53.1 kJ/mol Δ\DeltaΔ H°f (H2S)= - 20.6 kJ/mol Will this reaction proceed spontaneously at 298 K and 1 atm pressure?

The entropy change on vaporization ( Δ\DeltaΔ Svap)of a compound or element is

Rubidium has a heat of vaporization of 69.0 kJ/mol at its boiling point (686°C).Calculate Δ\DeltaΔ S for this process, Rb(l) →\to→ Rb(g), at 1 atm and 686°C.

Predict the sign of Δ\DeltaΔ S for the reaction 6CO2(g)+ 6H2O(g) →\to→ C6H12O6(g)+ 6O2(g).

For the reaction SbCl5(g) SbCl3(g)+ Cl2(g), Δ\DeltaΔ G°f (SbCl5)= -334.34 kJ/mol Δ\DeltaΔ G°f (SbCl3)= -301.25 kJ/mol Δ\DeltaΔ H°f (SbCl5)= -394.34 kJ/mol Δ\DeltaΔ H°f (SbCl3)= -313.80 kJ/mol Will this reaction proceed spontaneously at 298 K and 1 atm pressure?

Calculate Δ\DeltaΔ S° for the reaction SO2(s)+ NO2(g) →\to→ SO3(g)+ NO(g).

Choose the substance with the higher entropy per mole at a given temperature: 1 mole of N2(g)in a 22.4 L container or 1 mole of N2(g)in a 2.24 L container.

A sample of solid naphthalene is introduced into an evacuated flask. Use the data below to calculate the equilibrium vapor pressure of naphthalene (C10H8)in the flask at 35°C.

The heat of vaporization of water is 2.27 kJ/g. What is Δ\DeltaΔ Svap per mole at the normal boiling point?

For a given substance the entropy always increases in the following order: S (gas)< S (liq)< S (solid).

Δ\DeltaΔ Hvap for ethanol is 38.7 kJ/mol at its boiling point (78°C).What is Δ\DeltaΔ Ssurr when 1.00 mole of ethanol is boiled?

Aluminum forms a layer of aluminum oxide when exposed to air which protects the bulk metal from further corrosion. 4Al(s)+ 3O2(g) →\to→ 2Al2O3(s) Calculate Δ\DeltaΔ G° for this reaction, given that Δ\DeltaΔ G°f of aluminum oxide is -1576.4 kJ/mol.

Predict the normal boiling point of triethylborane (C6H15B)using the following data:

Arrange these reactions according to increasing Δ\DeltaΔ S. 1)H2O(g) →\to→ H2O(l) 2)2NO(g) →\to→ N2(g)+ O2(g) 3)MgCO3(s) →\to→ MgO(s)+ CO2(g)

The entropy change ×\times× S° for the reaction NH4Cl(s) →\to→ NH3(g)+ HCl(g)will be negative.

For the reaction HCONH2(g) NH3(g)+ CO(g), Kc = 4.84 at 400 K. If Δ\DeltaΔ H° for this reaction is 29 kJ/mol, find Kc at 500 K.

Calculate Kp at 298 K for the reaction SO2(g)+ NO2(g) →\to→ SO3(g)+ NO(g).

Using the thermodynamic data provided below, calculate Ka2 for H2CO3(aq)at 25°.

Chemistry: The Study of Change

Atoms, Molecules, and Ions

Mass Relationships in Chemical Reactions

Reactions in Aqueous Solution

Gases

Thermo-Chemistry

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 Orbitals

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Chemistry in the Atmosphere

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The entropy change on vaporization ( $\Delta$ S_vap)of a compound or element is

Rubidium has a heat of vaporization of 69.0 kJ/mol at its boiling point (686°C).Calculate $\Delta$ S for this process, Rb(l) $\to$ Rb(g), at 1 atm and 686°C.

Predict the sign of $\Delta$ S for the reaction 6CO₂(g)+ 6H₂O(g) $\to$ C₆H₁₂O₆(g)+ 6O₂(g).

Calculate $\Delta$ S° for the reaction SO₂(s)+ NO₂(g) $\to$ SO₃(g)+ NO(g). $Calculate \Delta S° for the reaction SO<sub>2</sub>(s)+ NO<sub>2</sub>(g) \to SO<sub>3</sub>(g)+ NO(g).$

Choose the substance with the higher entropy per mole at a given temperature: 1 mole of N₂(g)in a 22.4 L container or 1 mole of N₂(g)in a 2.24 L container.

A sample of solid naphthalene is introduced into an evacuated flask. Use the data below to calculate the equilibrium vapor pressure of naphthalene (C₁₀H₈)in the flask at 35°C.

The heat of vaporization of water is 2.27 kJ/g. What is $\Delta$ S_vap per mole at the normal boiling point?

$\Delta$ H_vap for ethanol is 38.7 kJ/mol at its boiling point (78°C).What is $\Delta$ S_surr when 1.00 mole of ethanol is boiled?

Aluminum forms a layer of aluminum oxide when exposed to air which protects the bulk metal from further corrosion. 4Al(s)+ 3O₂(g) $\to$ 2Al₂O₃(s) Calculate $\Delta$ G° for this reaction, given that $\Delta$ G°_f of aluminum oxide is -1576.4 kJ/mol.

Predict the normal boiling point of triethylborane (C₆H₁₅B)using the following data:

Arrange these reactions according to increasing $\Delta$ S. 1)H₂O(g) $\to$ H₂O(l) 2)2NO(g) $\to$ N₂(g)+ O₂(g) 3)MgCO₃(s) $\to$ MgO(s)+ CO₂(g)

The entropy change $\times$ S° for the reaction NH₄Cl(s) $\to$ NH₃(g)+ HCl(g)will be negative.

Calculate K_p at 298 K for the reaction SO₂(g)+ NO₂(g) $\to$ SO₃(g)+ NO(g). $Calculate K<sub>p</sub> at 298 K for the reaction SO<sub>2</sub>(g)+ NO<sub>2</sub>(g) \to SO<sub>3</sub>(g)+ NO(g).$

Using the thermodynamic data provided below, calculate K_a2 for H₂CO₃(aq)at 25°.