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

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

Without reference to a table, arrange these reactions according to increasing $\Delta$S. 1)CH4(g)+ H2O(g)$\rarr$ CO(g)+ 3H2(g) 2)C(s)+ O2(g)$\rarr$CO2(g) 3)H2O2(l)$\rarr$ H2O(l)+ 1/2O2(g)

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

For the reaction 2NO(g)+ O2(g)$\rarr$ 2NO2(g)if initially P(NO)= 1.5 atm, P(O2)= 1.4 atm, and P(NO2)= 2.0 atm, calculate $\Delta$G for this reaction at 25°C.The following data is valid at 25°C:

A) -69.9 kJ/mol B) -69.2 kJ/mol C) 522.1 kJ/mol D) -79.9 kJ/mol E) -35.0 kJ/mol A) -69.9 kJ/mol B) -69.2 kJ/mol C) 522.1 kJ/mol D) -79.9 kJ/mol E) -35.0 kJ/mol

At 1500°C the equilibrium constant for the reaction CO(g)+ 2H2(g) CH3OH(g)has the value Kp = 1.4 × 10-7.Calculate $\Delta$G° for this reaction at 1500°C.

A) 105 kJ/mol B) 1.07 kJ/mol C) -233 kJ/mol D) -105 kJ/mol E) 233 kJ/mol A) 105 kJ/mol B) 1.07 kJ/mol C) -233 kJ/mol D) -105 kJ/mol E) 233 kJ/mol

Exam 17: Entropy Free Energy and Equilibrium

The solubility product constant at 25°C for AgI(s)in water has the value 8.3 × 10^-17.Calculate $\Delta$ G_rxn at 25°C for the process AgI(s) $The solubility product constant at 25°C for AgI(s)in water has the value 8.3 × 10-17.Calculate \Delta Grxn at 25°C for the process AgI(s) Ag+(aq)+ I- (aq)where [Ag+] = 9.1 × 10-9 and [I-] = 9.1 × 10-9.$ Ag⁺(aq)+ I^-(aq)where [Ag⁺] = 9.1 × 10^-9 and [I^-] = 9.1 × 10^-9.

(Multiple Choice)

5.0/5

(82)

Question 21

Predict the signs (-, +, or 0)of $\Delta$ H and $\Delta$ S, in that order, for the expansion of an ideal gas into a vacuum.

(Short Answer)

4.9/5

(88)

Question 22

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

(True/False)

4.8/5

(77)

Question 23

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.

(Multiple Choice)

4.8/5

(78)

Question 24

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

(True/False)

4.8/5

(77)

Question 25

Given the following data, estimate the boiling point of carbon disulfide, CS₂, assuming that $\Delta$ S° and $\Delta$ H° are temperature-independent. $Given the following data, estimate the boiling point of carbon disulfide, CS2, assuming that \Delta S° and \Delta H° are temperature-independent.$

(Short Answer)

4.8/5

(73)

Question 26

For the reaction CuS(s)+ H₂(g) $For the reaction CuS(s)+ H2(g) H2S(g)+ Cu(s), \Delta G°f (CuS)= -53.6 kJ/mol \Delta G°f (H2S)= -33.6 kJ/mol \Delta H°f (CuS)= -53.1 kJ/mol \Delta H°f (H2S)= -20.6 kJ/mol Calculate \Delta G at 798 K and 1 atm pressure (assume \Delta S° and \Delta H° do not change with temperature).$ 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 Calculate $\Delta$ G at 798 K and 1 atm pressure (assume $\Delta$ S°and $\Delta$ H° do not change with temperature).

(Short Answer)

4.8/5

(87)

Question 27

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.

(Multiple Choice)

4.8/5

(84)

Question 28

Melting an ionic solid always results in an increase in entropy.

(True/False)

4.9/5

(88)

Question 29

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.]

(Multiple Choice)

4.9/5

(77)

Question 30

Without reference to a table, arrange these reactions according to increasing $\Delta$ S. 1)CH₄(g)+ H₂O(g) $\rarr$ CO(g)+ 3H₂(g) 2)C(s)+ O₂(g) $\rarr$ CO₂(g) 3)H₂O₂(l) $\rarr$ H₂O(l)+ ¹/₂O₂(g)

(Multiple Choice)

4.8/5

(81)

Question 31

For the reaction SbCl₅(g) $For the reaction SbCl5(g) SbCl3(g)+ Cl2(g), \Delta G°f (SbCl5)= -334.34 kJ/mol \Delta G°f (SbCl3)= -301.25 kJ/mol \Delta H°f (SbCl5)= -394.34 kJ/mol \Delta H°f (SbCl3)= -313.80 kJ/mol Calculate the value of the equilibrium constant (Kp)at 800 K and 1 atm pressure.$ 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 Calculate the value of the equilibrium constant (K_p)at 800 K and 1 atm pressure.

(Short Answer)

4.8/5

(95)

Question 32

The equilibrium constant for the reaction AgBr(s) $The equilibrium constant for the reaction AgBr(s) Ag+(aq)+ Br- (aq)is the solubility product constant, Ksp = 7.7 × 10-13 at 25°C.Calculate \Delta G for the reaction when [Ag+] = 1.0 × 10-2 M and [Br-] = 1.0 × 10-3 M.Is the reaction spontaneous or nonspontaneous at these concentrations?$ Ag⁺(aq)+ Br^-(aq)is the solubility product constant, K_sp = 7.7 × 10^-13 at 25°C.Calculate $\Delta$ G for the reaction when [Ag⁺] = 1.0 × 10^-2 M and [Br^-] = 1.0 × 10^-3 M.Is the reaction spontaneous or nonspontaneous at these concentrations?

(Multiple Choice)

4.8/5

(86)

Question 33

Sulfur can be separated from lead in the mineral galena, PbS(s), by "roasting" the ore in the presence of oxygen as shown in the following reaction: 2PbS(s)+ 3O₂(g) $\rarr$ 2PbO(s)+ 2SO₂(g) Calculate $\Delta$ S° for this reaction using the thermodynamic data provided below. $Sulfur can be separated from lead in the mineral galena, PbS(s), by roasting the ore in the presence of oxygen as shown in the following reaction: 2PbS(s)+ 3O2(g) \rarr 2PbO(s)+ 2SO2(g) Calculate \Delta S° for this reaction using the thermodynamic data provided below.$

(Multiple Choice)

4.9/5

(80)

Question 34

Under what conditions (always, never, high temperature only, low temperature only)is the process: H₂O(l) $\rarr$ H₂O(s)expected to be spontaneous?

(Short Answer)

4.7/5

(71)

Question 35

For the reaction H₂O₂(g) $\rarr$ H₂O(g)+ ¹/₂O₂(g), $\Delta$ H° = -106 kJ/mol and $\Delta$ S° = 58 J/K·mol at 25°C.Calculate $\Delta$ G° for this reaction at this temperature.

(Short Answer)

4.9/5

(80)

Question 36

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

(Multiple Choice)

4.9/5

(84)

Question 37

Under what conditions (always, never, high temperature only, low temperature only)is the reaction O₂(g) $\rarr$ 2O(g)expected to be spontaneous?

(Short Answer)

4.7/5

(72)

Question 38

For the reaction 2NO(g)+ O₂(g) $\rarr$ 2NO₂(g)if initially P(NO)= 1.5 atm, P(O₂)= 1.4 atm, and P(NO₂)= 2.0 atm, calculate $\Delta$ G for this reaction at 25°C.The following data is valid at 25°C: $For the reaction 2NO(g)+ O2(g) \rarr 2NO2(g)if initially P(NO)= 1.5 atm, P(O2)= 1.4 atm, and P(NO2)= 2.0 atm, calculate \Delta G for this reaction at 25°C.The following data is valid at 25°C:$

(Multiple Choice)

4.8/5

(83)

Question 39

At 1500°C the equilibrium constant for the reaction CO(g)+ 2H₂(g) $At 1500°C the equilibrium constant for the reaction CO(g)+ 2H2(g) CH3OH(g)has the value Kp = 1.4 × 10-7.Calculate \Delta G° for this reaction at 1500°C.$ CH₃OH(g)has the value K_p = 1.4 × 10^-7.Calculate $\Delta$ G° for this reaction at 1500°C.

(Multiple Choice)

4.9/5

(67)

Question 40

Showing 21 - 40 of 128

Predict the signs (-, +, or 0)of $\Delta$ H and $\Delta$ S, in that order, for the expansion of an ideal gas into a vacuum.

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

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.

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

Melting an ionic solid always results in an increase in entropy.

Without reference to a table, arrange these reactions according to increasing $\Delta$ S. 1)CH₄(g)+ H₂O(g) $\rarr$ CO(g)+ 3H₂(g) 2)C(s)+ O₂(g) $\rarr$ CO₂(g) 3)H₂O₂(l) $\rarr$ H₂O(l)+ ¹/₂O₂(g)

Under what conditions (always, never, high temperature only, low temperature only)is the process: H₂O(l) $\rarr$ H₂O(s)expected to be spontaneous?

For the reaction H₂O₂(g) $\rarr$ H₂O(g)+ ¹/₂O₂(g), $\Delta$ H° = -106 kJ/mol and $\Delta$ S° = 58 J/K·mol at 25°C.Calculate $\Delta$ G° for this reaction at this temperature.

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

Under what conditions (always, never, high temperature only, low temperature only)is the reaction O₂(g) $\rarr$ 2O(g)expected to be spontaneous?

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 Orbitals

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 Metal Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

Exam 17: Entropy Free Energy and Equilibrium

The solubility product constant at 25°C for AgI(s)in water has the value 8.3 × 10-17.Calculate Δ\DeltaΔ Grxn at 25°C for the process AgI(s) Ag+(aq)+ I- (aq)where [Ag+] = 9.1 × 10-9 and [I-] = 9.1 × 10-9.

Predict the signs (-, +, or 0)of Δ\DeltaΔ H and Δ\DeltaΔ S, in that order, for the expansion of an ideal gas into a vacuum.

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

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.

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

Given the following data, estimate the boiling point of carbon disulfide, CS2, assuming that Δ\DeltaΔ S° and Δ\DeltaΔ H° are temperature-independent.

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.

Melting an ionic solid always results in an increase in entropy.

Without reference to a table, arrange these reactions according to increasing Δ\DeltaΔ S. 1)CH4(g)+ H2O(g) →\rarr→ CO(g)+ 3H2(g) 2)C(s)+ O2(g) →\rarr→ CO2(g) 3)H2O2(l) →\rarr→ H2O(l)+ 1/2O2(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 Calculate the value of the equilibrium constant (Kp)at 800 K and 1 atm pressure.

The equilibrium constant for the reaction AgBr(s) Ag+(aq)+ Br- (aq)is the solubility product constant, Ksp = 7.7 × 10-13 at 25°C.Calculate Δ\DeltaΔ G for the reaction when [Ag+] = 1.0 × 10-2 M and [Br-] = 1.0 × 10-3 M.Is the reaction spontaneous or nonspontaneous at these concentrations?

Sulfur can be separated from lead in the mineral galena, PbS(s), by "roasting" the ore in the presence of oxygen as shown in the following reaction: 2PbS(s)+ 3O2(g) →\rarr→ 2PbO(s)+ 2SO2(g) Calculate Δ\DeltaΔ S° for this reaction using the thermodynamic data provided below.

Under what conditions (always, never, high temperature only, low temperature only)is the process: H2O(l) →\rarr→ H2O(s)expected to be spontaneous?

For the reaction H2O2(g) →\rarr→ H2O(g)+ 1/2O2(g), Δ\DeltaΔ H° = -106 kJ/mol and Δ\DeltaΔ S° = 58 J/K·mol at 25°C.Calculate Δ\DeltaΔ G° for this reaction at this temperature.

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

Under what conditions (always, never, high temperature only, low temperature only)is the reaction O2(g) →\rarr→ 2O(g)expected to be spontaneous?

For the reaction 2NO(g)+ O2(g) →\rarr→ 2NO2(g)if initially P(NO)= 1.5 atm, P(O2)= 1.4 atm, and P(NO2)= 2.0 atm, calculate Δ\DeltaΔ G for this reaction at 25°C.The following data is valid at 25°C:

At 1500°C the equilibrium constant for the reaction CO(g)+ 2H2(g) CH3OH(g)has the value Kp = 1.4 × 10-7.Calculate Δ\DeltaΔ G° for this reaction at 1500°C.

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 Orbitals

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 Metal Chemistry and Coordination Compounds

Organic Chemistry

Synthetic and Natural Organic Polymers

Filters

Predict the signs (-, +, or 0)of $\Delta$ H and $\Delta$ S, in that order, for the expansion of an ideal gas into a vacuum.

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.

Without reference to a table, arrange these reactions according to increasing $\Delta$ S. 1)CH₄(g)+ H₂O(g) $\rarr$ CO(g)+ 3H₂(g) 2)C(s)+ O₂(g) $\rarr$ CO₂(g) 3)H₂O₂(l) $\rarr$ H₂O(l)+ ¹/₂O₂(g)

Under what conditions (always, never, high temperature only, low temperature only)is the process: H₂O(l) $\rarr$ H₂O(s)expected to be spontaneous?

For the reaction H₂O₂(g) $\rarr$ H₂O(g)+ ¹/₂O₂(g), $\Delta$ H° = -106 kJ/mol and $\Delta$ S° = 58 J/K·mol at 25°C.Calculate $\Delta$ G° for this reaction at this temperature.

Under what conditions (always, never, high temperature only, low temperature only)is the reaction O₂(g) $\rarr$ 2O(g)expected to be spontaneous?