Question 1

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

Accepted Answer

The answer of $\Delta$Hvap for ethanol is 38.7 kJ/mol at...

Question 2

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.

Accepted Answer

The answer of For the reaction H2O2(g) $\rarr$ H2O(g)+ 1/2O2(g),...

Question 3

Hydrogen peroxide (H2O2)decomposes according to the equation H2O2(l)$\rarr$ H2O(l)+ 1/2O2(g).
Calculate Kp for this reaction at 25°C. ($\Delta$H° = -98.2 kJ/mol, $\Delta$S° = 70.1 J/K·mol)

Accepted Answer

A) 1.3 * 10-21 
B) 20.9 
C) 3.46 * 1017 
D) 7.5 * 1020 
E) 8.6 * 104 
A) 1.3 * 10-21 
B) 20.9 
C) 3.46 * 1017 
D) 7.5 * 1020 
E) 8.6 * 104

Question 4

For the reaction 2C(graphite)+ H2(g) $\rarr$C2H2(g), $\Delta$G°= +209.2 kJ/mol at 25°C. If P(H2)= 100. atm, and P(C2H2)= 0.10 atm, calculate $\Delta$G for this reaction.

Accepted Answer

A) +207.8 kJ/mol 
B) +226.3 kJ/mol 
C) +192.1 kJ/mol 
D) +17.3 kJ/mol 
E) -16.9 kJ/mol 
A) +207.8 kJ/mol 
B) +226.3 kJ/mol 
C) +192.1 kJ/mol 
D) +17.3 kJ/mol 
E) -16.9 kJ/mol

Question 5

For the reaction CuS(s)+ H2(g) $\rarr$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).

Accepted Answer

The answer of For the reaction CuS(s)+ H2(g) $\rarr$H2S(g)+ Cu(s),
$\Delta$G°f...

Question 6

Mg2+(aq)+ 2OH-(aq) $\rarr$ Mg(OH)2(s)

Accepted Answer

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

Question 7

Predict the sign of $\Delta$S for the reaction O2(g) $\rarr$ 2O(g).

Accepted Answer

The answer of Predict the sign of $\Delta$S for the...

Question 8

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

Accepted Answer

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

Question 9

Calculate $\Delta$S° at 25°C for the reduction of PbO(s), 2PbO(s)+ C(s) $\rarr$ 2Pb(s)+ CO2(g)given these absolute entropies:

Accepted Answer

A) +198.8 J/K·mol 
B) +488.0 J/K·mol 
C) +353.6 J/K·mol 
D) -203.3 J/K·mol 
E) +203.3 J/K·mol 
A) +198.8 J/K·mol 
B) +488.0 J/K·mol 
C) +353.6 J/K·mol 
D) -203.3 J/K·mol 
E) +203.3 J/K·mol

Question 10

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

Accepted Answer

A) CH4(g)+ 2O2(g) $\rarr$ CO2(g)+ 2H2O(g) 
B) C2H2(g)+ 5/2O2(g) $\rarr$2CO2(g)+ H2O(g) 
C) C2H4(g)+ 3O2(g) $\rarr$2CO2(g)+ 2H2O(g) 
D) C2H6(g)+ 7/2O2(g) $\rarr$ 2CO2(g)+ 3H2O(g) 
A) CH4(g)+ 2O2(g) $\rarr$ CO2(g)+ 2H2O(g) 
B) C2H2(g)+ 5/2O2(g) $\rarr$2CO2(g)+ H2O(g) 
C) C2H4(g)+ 3O2(g) $\rarr$2CO2(g)+ 2H2O(g) 
D) C2H6(g)+ 7/2O2(g) $\rarr$ 2CO2(g)+ 3H2O(g)

Question 11

For the reaction 3H2(g)+ N2(g) $\rarr$2NH3(g), Kc = 9.0 at 350°C. Calculate $\Delta$G° at 350°C.

Accepted Answer

The answer of For the reaction 3H2(g)+ N2(g) $\rarr$2NH3(g), Kc...

Question 12

Determine the equilibrium constant (Kp)at 25°C for the reaction CO(g)+ H2O(g) $\rarr$ CO2(g)+ H2(g) $\Delta$G° = -28.5 kJ/mol.

Accepted Answer

A) 2.9 * 10-60 
B) 1.0 * 10-4 
C) 1.2 
D) 1.0 * 105 
E) 3.4 * 1059 
A) 2.9 * 10-60 
B) 1.0 * 10-4 
C) 1.2 
D) 1.0 * 105 
E) 3.4 * 1059

Question 13

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

Accepted Answer

2.8 * 10^-9

Question 14

Given the following data, calculate the boiling point of HCOOH (formic acid).

Accepted Answer

The answer of Given the following data, calculate the boiling...

Question 15

Using the thermodynamic data provided below, determine the temperature in °C at which the decomposition of solid calcium carbonate to form solid calcium oxide and oxygen becomes spontaneous.

Accepted Answer

The answer of Using the thermodynamic data provided below, determine...

Question 16

H2O2(l) $\rarr$ H2O(l)+ 1/2O2(g)

Accepted Answer

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

Question 17

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

Accepted Answer

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

Question 18

The equilibrium constant at 427°C for the reaction N2(g)+ 3H2(g) $\rarr$ 2NH3(g)is Kp = 9.4 * 10-5. Calculate the value of $\Delta$G° for the reaction under these conditions.

Accepted Answer

A) -33 kJ/mol 
B) -54 kJ/mol 
C) 54 kJ/mol 
D) 33 kJ/mol 
E) 1.3 J/mol 
A) -33 kJ/mol 
B) -54 kJ/mol 
C) 54 kJ/mol 
D) 33 kJ/mol 
E) 1.3 J/mol

Question 19

Find the temperature at which Kp = 42.0 for the reaction H2(g)+ I2(g) $\rarr$ 2HI(g). [Given: at 25°C, for H2(g), $\Delta$H°f = 0, S° = 131.0 J/mol·K; for I2(g), $\Delta$H°f = 62.26 kJ/mol, S° = 260.6 J/mol·K; for HI(g), $\Delta$H°f = 25.9 kJ/mol, S° = 206.3 J/mol·K; assume that $\Delta$H° and $\Delta$S° are independent of temperature.]

Accepted Answer

A) 1040 K 
B) 168 K 
C) 539 K 
D) 1400 K 
E) 34,200 K 
A) 1040 K 
B) 168 K 
C) 539 K 
D) 1400 K 
E) 34,200 K

Question 20

Given the following data, estimate the boiling point of bromine, Br2, assuming that $\Delta$S° and $\Delta$H° are temperature-independent.

Accepted Answer

The answer of Given the following data, estimate the boiling...

$\Delta$ 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?

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.

Hydrogen peroxide (H₂O₂)decomposes according to the equation H₂O₂(l) $\rarr$ H₂O(l)+ ¹/₂O₂(g). Calculate K_p for this reaction at 25°C. ( $\Delta$ H° = -98.2 kJ/mol, $\Delta$ S° = 70.1 J/K·mol)

For the reaction 2C(graphite)+ H₂(g) $\rarr$ C₂H₂(g), $\Delta$ G°= +209.2 kJ/mol at 25°C. If P(H₂)= 100. atm, and P(C₂H₂)= 0.10 atm, calculate $\Delta$ G for this reaction.

Mg²⁺(aq)+ 2OH^-(aq) $\rarr$ Mg(OH)₂(s)

Predict the sign of $\Delta$ S for the reaction O₂(g) $\rarr$ 2O(g).

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

Calculate $\Delta$ S° at 25°C for the reduction of PbO(s), 2PbO(s)+ C(s) $\rarr$ 2Pb(s)+ CO₂(g)given these absolute entropies: $Calculate \Delta S° at 25°C for the reduction of PbO(s), 2PbO(s)+ C(s) \rarr 2Pb(s)+ CO<sub>2</sub>(g)given these absolute entropies:$

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

For the reaction 3H₂(g)+ N₂(g) $\rarr$ 2NH₃(g), K_c = 9.0 at 350°C. Calculate $\Delta$ G° at 350°C.

Determine the equilibrium constant (K_p)at 25°C for the reaction CO(g)+ H₂O(g) $\rarr$ CO₂(g)+ H₂(g) $\Delta$ G° = -28.5 kJ/mol.

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

Given the following data, calculate the boiling point of HCOOH (formic acid).

Using the thermodynamic data provided below, determine the temperature in °C at which the decomposition of solid calcium carbonate to form solid calcium oxide and oxygen becomes spontaneous.

H₂O₂(l) $\rarr$ H₂O(l)+ ¹/₂O₂(g)

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

The equilibrium constant at 427°C for the reaction N₂(g)+ 3H₂(g) $\rarr$ 2NH₃(g)is K_p = 9.4 * 10^-5. Calculate the value of $\Delta$ G° for the reaction under these conditions.

Given the following data, estimate the boiling point of bromine, Br₂, assuming that $\Delta$ S° and $\Delta$ H° are temperature-independent. $Given the following data, estimate the boiling point of bromine, Br<sub>2</sub>, assuming that \Delta S° and \Delta H° are temperature-independent.$

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

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Exam 18: Thermodynamics

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?

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.

Hydrogen peroxide (H2O2)decomposes according to the equation H2O2(l) →\rarr→ H2O(l)+ 1/2O2(g). Calculate Kp for this reaction at 25°C. ( Δ\DeltaΔ H° = -98.2 kJ/mol, Δ\DeltaΔ S° = 70.1 J/K·mol)

For the reaction 2C(graphite)+ H2(g) →\rarr→ C2H2(g), Δ\DeltaΔ G°= +209.2 kJ/mol at 25°C. If P(H2)= 100. atm, and P(C2H2)= 0.10 atm, calculate Δ\DeltaΔ G for this reaction.

Mg2+(aq)+ 2OH-(aq) →\rarr→ Mg(OH)2(s)

Predict the sign of Δ\DeltaΔ S for the reaction O2(g) →\rarr→ 2O(g).

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

Calculate Δ\DeltaΔ S° at 25°C for the reduction of PbO(s), 2PbO(s)+ C(s) →\rarr→ 2Pb(s)+ CO2(g)given these absolute entropies:

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

For the reaction 3H2(g)+ N2(g) →\rarr→ 2NH3(g), Kc = 9.0 at 350°C. Calculate Δ\DeltaΔ G° at 350°C.

Determine the equilibrium constant (Kp)at 25°C for the reaction CO(g)+ H2O(g) →\rarr→ CO2(g)+ H2(g) Δ\DeltaΔ G° = -28.5 kJ/mol.

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

Given the following data, calculate the boiling point of HCOOH (formic acid).

Using the thermodynamic data provided below, determine the temperature in °C at which the decomposition of solid calcium carbonate to form solid calcium oxide and oxygen becomes spontaneous.

H2O2(l) →\rarr→ H2O(l)+ 1/2O2(g)

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

The equilibrium constant at 427°C for the reaction N2(g)+ 3H2(g) →\rarr→ 2NH3(g)is Kp = 9.4 * 10-5. Calculate the value of Δ\DeltaΔ G° for the reaction under these conditions.

Given the following data, estimate the boiling point of bromine, Br2, assuming that Δ\DeltaΔ S° and Δ\DeltaΔ H° are temperature-independent.

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

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$\Delta$ 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?

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.

Hydrogen peroxide (H₂O₂)decomposes according to the equation H₂O₂(l) $\rarr$ H₂O(l)+ ¹/₂O₂(g). Calculate K_p for this reaction at 25°C. ( $\Delta$ H° = -98.2 kJ/mol, $\Delta$ S° = 70.1 J/K·mol)

For the reaction 2C(graphite)+ H₂(g) $\rarr$ C₂H₂(g), $\Delta$ G°= +209.2 kJ/mol at 25°C. If P(H₂)= 100. atm, and P(C₂H₂)= 0.10 atm, calculate $\Delta$ G for this reaction.

Mg²⁺(aq)+ 2OH^-(aq) $\rarr$ Mg(OH)₂(s)

Predict the sign of $\Delta$ S for the reaction O₂(g) $\rarr$ 2O(g).

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

Calculate $\Delta$ S° at 25°C for the reduction of PbO(s), 2PbO(s)+ C(s) $\rarr$ 2Pb(s)+ CO₂(g)given these absolute entropies: $Calculate \Delta S° at 25°C for the reduction of PbO(s), 2PbO(s)+ C(s) \rarr 2Pb(s)+ CO<sub>2</sub>(g)given these absolute entropies:$

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

For the reaction 3H₂(g)+ N₂(g) $\rarr$ 2NH₃(g), K_c = 9.0 at 350°C. Calculate $\Delta$ G° at 350°C.

Determine the equilibrium constant (K_p)at 25°C for the reaction CO(g)+ H₂O(g) $\rarr$ CO₂(g)+ H₂(g) $\Delta$ G° = -28.5 kJ/mol.

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

H₂O₂(l) $\rarr$ H₂O(l)+ ¹/₂O₂(g)

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

The equilibrium constant at 427°C for the reaction N₂(g)+ 3H₂(g) $\rarr$ 2NH₃(g)is K_p = 9.4 * 10^-5. Calculate the value of $\Delta$ G° for the reaction under these conditions.

Given the following data, estimate the boiling point of bromine, Br₂, assuming that $\Delta$ S° and $\Delta$ H° are temperature-independent. $Given the following data, estimate the boiling point of bromine, Br<sub>2</sub>, assuming that \Delta S° and \Delta H° are temperature-independent.$