Question 1

Given: 4NH3(g)+ 5O2(g) → 4NO(g)+ 6H2O(g)
K
Calculate the equilibrium constant for the following reaction.
2NO(g)+ 3H2O(g) →2NH3(g)+   O2(g)

Accepted Answer

A) -0.5K 
B) -2K 
C) K-1/2  
D) -K 
E) K-1  
A) -0.5K 
B) -2K 
C) K-1/2  
D) -K 
E) K-1

Question 2

Consider the reaction below:
F2(g) → 2F(g)
(a)Compressing the reaction mixture results in a change in Q.True or false?
(b)Heating the reaction mixture causes the reaction to shift to the left.True or false?
(c)At 1000 K,the equilibrium constant for the reaction is about 10-4.If the reaction is perturbed such that Q = 1,the reaction must shift to the left.

Accepted Answer

(a)True
(b

Question 3

At 600S1U1P1$\circ$S1S1P0C,Kc = 2.8 for the reaction 2HgO(s) → 2Hg(l)+ O2(g)
Calculate K at 600S1U1P1$\circ$S1S1P0C for this reaction.

Accepted Answer

A) 6800 
B) 200 
C) 1.4 * 104  
D) 2.8 
E) 138 
A) 6800 
B) 200 
C) 1.4 * 104  
D) 2.8 
E) 138

Question 4

At 600S1U1P1$\circ$S1S1P0C,the equilibrium constant for the reaction 2HgO(s) → 2Hg(l)+ O2(g)
Is 2.8.Calculate the equilibrium constant for the reaction   1/2O2(g)+ Hg(l) → HgO(s)

Accepted Answer

A) -1.7 
B) 1.1 
C) 0.60 
D) 0.36 
E) 1.7 
A) -1.7 
B) 1.1 
C) 0.60 
D) 0.36 
E) 1.7

Question 5

At 25S1U1P1$\circ$S1S1P0C,K  = 6.9 * 105 for the reaction N2(g)+ 3H2(g) →2NH3(g)
Calculate Kc at 25S1U1P1$\circ$S1S1P0C for this reaction.

Accepted Answer

A) 2.8 * 104  
B) 6.8 * 105  
C) 1.1 * 103  
D) 1.7 * 107  
E) 4.1 * 108  
A) 2.8 * 104  
B) 6.8 * 105  
C) 1.1 * 103  
D) 1.7 * 107  
E) 4.1 * 108

Question 6

Given: 2P(g)+ 3Cl2(g) →2PCl3(g)K = 15.0 PCl3(g)+ Cl2(g) →PCl5(g)K = 4.0
What is the value of the equilibrium constant for the reaction below?
2P(g)+ 5Cl2(g) →2PCl5(g)

Accepted Answer

A) 60 
B) 240 
C) 1.1 
D) 3600 
E) 23 
A) 60 
B) 240 
C) 1.1 
D) 3600 
E) 23

Question 7

An endothermic reaction is most likely to have a small equilibrium constant if $\Delta$Sro is small.

Accepted Answer

A) True 
 B)False

Question 8

At 700 K,K = 54 for the reaction H2(g)+ I2(g) →2HI(g)
Calculate Kc at 700 K for this reaction.

Accepted Answer

A) 3.2 * 10-4  
B) 0.94 
C) 7.7 * 10-4  
D) 0.45 
E) 54 
A) 3.2 * 10-4  
B) 0.94 
C) 7.7 * 10-4  
D) 0.45 
E) 54

Question 9

Consider the reaction 4NH3(g)+ 3O2(g) →2N2(g)+ 6H2O(g),K = 1080 at a certain temperature.
Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of oxygen is

Accepted Answer

A) 6 M. 
B) 0 M. 
C) 3 M. 
D) 12 M. 
E) 18 M. 
A) 6 M. 
B) 0 M. 
C) 3 M. 
D) 12 M. 
E) 18 M.

Question 10

The vapor pressure of acetic acid at 25S1U1P1$\circ$S1S1P0C is 16 Torr.$\Delta$Gr for the reaction CH3COOH(l) →CH3COOH(g)
At 25S1U1P1$\circ$S1S1P0C is

Accepted Answer

A) 0 
B) +9.57 kJ·mol-1 
C) -9.57 kJ·mol-1 
D) +1.85 kJ·mol-1 
A) 0 
B) +9.57 kJ·mol-1 
C) -9.57 kJ·mol-1 
D) +1.85 kJ·mol-1

Question 11

For the reaction 2CaSO4(s) → 2CaO(s)+ 2SO2(g)+ O2(g)
K = 0.032 at 700 K.What is the total pressure starting from pure CaSO4(s)?

Accepted Answer

A) 0.22 bar 
B) 0.011 bar 
C) 0.60 bar 
D) 0.20 bar 
E) 0.40 bar 
A) 0.22 bar 
B) 0.011 bar 
C) 0.60 bar 
D) 0.20 bar 
E) 0.40 bar

Question 12

For a pure solid or liquid,the molar free energy always has its standard value.

Accepted Answer

A) True 
 B)False

Question 13

The van't Hoff equation can be used to obtain the standard reaction enthalpy for a reaction if the equilibrium constant for the reaction is known at two different temperatures.

Accepted Answer

A) True 
 B)False

Question 14

For the equilibrium CaCO3(s) → CaO(s)+ CO2(g),(a)represents the composition at equilibrium at a certain temperature.In (b),a small amount of Ca*CO3(s)has been added (Ca*CO3(s)represents Ca14CO3(s)or labeled calcium carbonate).Draw the composition in (c)at equilibrium and explain your drawing.

Accepted Answer

CaCO₃,Ca^*CO₃,CaO,and a

Question 15

The equilibrium constant,Kc,for the reaction 2NOCl(g) →2NO(g)+ Cl2(g)
Is 0.51 at a certain temperature.A mixture of NOCl,NO,and Cl2 with concentrations 1.3,1.2,and 0.60 M,respectively,was introduced into a container at this temperature.Which of the following is true?

Accepted Answer

A) Cl2(g)is produced until equilibrium is reached. 
B) [NOCl] = [NO] = [Cl2] at equilibrium. 
C) NOCl(g)is produced until equilibrium is reached. 
D) [Cl2] = 0.30 M at equilibrium. 
E) No apparent reaction takes place. 
A) Cl2(g)is produced until equilibrium is reached. 
B) [NOCl] = [NO] = [Cl2] at equilibrium. 
C) NOCl(g)is produced until equilibrium is reached. 
D) [Cl2] = 0.30 M at equilibrium. 
E) No apparent reaction takes place.

Question 16

The effect of a volume decrease on the reaction C(s)+ H2O(g) → CO(g)+ H2(g)
Is

Accepted Answer

A) that K decreases. 
B) more CO(g)and H2(g)are produced. 
C) no change. 
D) more H2O(g)is produced. 
E) that K increases. 
A) that K decreases. 
B) more CO(g)and H2(g)are produced. 
C) no change. 
D) more H2O(g)is produced. 
E) that K increases.

Question 17

Write the equilibrium constant for 2NaBr(aq)+ Pb(ClO4)2(aq) →PbBr2(s)+ 2NaClO4(aq).

Accepted Answer

A) K = [Pb2+][Br-2  
B) K = 1/([Pb2+][Br-2) 
C) K = [NaClO4]2/([NaBr]2[Pb(ClO4)2] 
D) K = [PbBr2]/([Pb2+][Br-]2) 
E) K = 1/([Pb(ClO4)2][NaBr]2) 
A) K = [Pb2+][Br-2  
B) K = 1/([Pb2+][Br-2) 
C) K = [NaClO4]2/([NaBr]2[Pb(ClO4)2] 
D) K = [PbBr2]/([Pb2+][Br-]2) 
E) K = 1/([Pb(ClO4)2][NaBr]2)

Question 18

Consider the reaction 
2CuBr2(s)$\rightarrow$2CuBr(s)+ Br2(g)
If the equilibrium vapor pressure of Br2(g)is 1.43 * 10-5 Torr at 298 K,what is $\Delta$G at this temperature when Br2(g)is produced at a pressure of 7.50 * 10-8 Torr.

Accepted Answer

A) -5.65 kJ 
B) 13.0 kJ 
C) 5.65 kJ 
D) -3.42 kJ 
E) -13.0 kJ 
A) -5.65 kJ 
B) 13.0 kJ 
C) 5.65 kJ 
D) -3.42 kJ 
E) -13.0 kJ

Question 19

Consider the following reaction at a certain temperature: 
PCl5(g) →PCl3(g)+ Cl2(g)
Kc = 0.100
At equilibrium,[PCl5] = 2.00 M and [PCl3] = [Cl2] = 1.00 M.If suddenly 1.00 M PCl3(g)and Cl2(g)is added,what is the equilibrium concentration of PCl5(g)?

Accepted Answer

A) essentially 4.00 M 
B) 0.58 M 
C) 2.58 M 
D) 3.42 M 
E) 1.42 M 
A) essentially 4.00 M 
B) 0.58 M 
C) 2.58 M 
D) 3.42 M 
E) 1.42 M

Question 20

Which of the following statements is true?

Accepted Answer

A) When the value of Q is large,the equilibrium lies on the product side of the equilibrium reaction. 
B) When the value of K is large,the equilibrium lies on the reactant side of the equilibrium reaction. 
C) A small value of K means that the equilibrium concentrations of the reactants are small compared to the equilibrium concentrations of the products. 
D) A large value of K means that the equilibrium concentrations of products are large compared to the equilibrium concentrations of the reactants. 
E) When the value of K is small,the equilibrium lies on the product side of the equilibrium reaction. 
A) When the value of Q is large,the equilibrium lies on the product side of the equilibrium reaction. 
B) When the value of K is large,the equilibrium lies on the reactant side of the equilibrium reaction. 
C) A small value of K means that the equilibrium concentrations of the reactants are small compared to the equilibrium concentrations of the products. 
D) A large value of K means that the equilibrium concentrations of products are large compared to the equilibrium concentrations of the reactants. 
E) When the value of K is small,the equilibrium lies on the product side of the equilibrium reaction.

Given: 4NH₃(g)+ 5O₂(g) → 4NO(g)+ 6H₂O(g) K Calculate the equilibrium constant for the following reaction. 2NO(g)+ 3H₂O(g) →2NH₃(g)+ O₂(g)

At 600^$\circ$C,K_c = 2.8 for the reaction 2HgO(s) → 2Hg(l)+ O₂(g) Calculate K at 600^$\circ$C for this reaction.

At 25^$\circ$C,K = 6.9 * 10⁵ for the reaction N₂(g)+ 3H₂(g) →2NH₃(g) Calculate K_c at 25^$\circ$C for this reaction.

Given: 2P(g)+ 3Cl₂(g) →2PCl₃(g)K = 15.0 PCl₃(g)+ Cl₂(g) →PCl₅(g)K = 4.0 What is the value of the equilibrium constant for the reaction below? 2P(g)+ 5Cl₂(g) →2PCl₅(g)

An endothermic reaction is most likely to have a small equilibrium constant if $\Delta$ S_r^o is small.

At 700 K,K = 54 for the reaction H₂(g)+ I₂(g) →2HI(g) Calculate K_c at 700 K for this reaction.

Consider the reaction 4NH₃(g)+ 3O₂(g) →2N₂(g)+ 6H₂O(g),K = 10⁸⁰ at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of oxygen is

The vapor pressure of acetic acid at 25^$\circ$C is 16 Torr. $\Delta$ G_r for the reaction CH₃COOH(l) →CH₃COOH(g) At 25^$\circ$C is

For the reaction 2CaSO₄(s) → 2CaO(s)+ 2SO₂(g)+ O₂(g) K = 0.032 at 700 K.What is the total pressure starting from pure CaSO₄(s)?

For a pure solid or liquid,the molar free energy always has its standard value.

The van't Hoff equation can be used to obtain the standard reaction enthalpy for a reaction if the equilibrium constant for the reaction is known at two different temperatures.

The equilibrium constant,K_c,for the reaction 2NOCl(g) →2NO(g)+ Cl₂(g) Is 0.51 at a certain temperature.A mixture of NOCl,NO,and Cl₂ with concentrations 1.3,1.2,and 0.60 M,respectively,was introduced into a container at this temperature.Which of the following is true?

The effect of a volume decrease on the reaction C(s)+ H₂O(g) → CO(g)+ H₂(g) Is

Write the equilibrium constant for 2NaBr(aq)+ Pb(ClO₄)₂(aq) →PbBr₂(s)+ 2NaClO₄(aq).

Consider the reaction 2CuBr₂(s) $\rightarrow$ 2CuBr(s)+ Br₂(g) If the equilibrium vapor pressure of Br₂(g)is 1.43 * 10^-5 Torr at 298 K,what is $\Delta$ G at this temperature when Br₂(g)is produced at a pressure of 7.50 * 10^-8 Torr.

Consider the following reaction at a certain temperature: PCl₅(g) →PCl₃(g)+ Cl₂(g) K_c = 0.100 At equilibrium,[PCl₅] = 2.00 M and [PCl₃] = [Cl₂] = 1.00 M.If suddenly 1.00 M PCl₃(g)and Cl₂(g)is added,what is the equilibrium concentration of PCl₅(g)?

Which of the following statements is true?

The Quantum World

Quantum Mechanics in Action: Atoms

Chemical Bonds

Molecular Shape and Structure

The Properties of Gases

Liquids and Solids

Inorganic Materials

Thermodynamics: The First Law

Thermodynamics: The Second and Third Laws

Physical Equilibria

Acids and Bases

Aqueous Equilibria

Electrochemistry

Chemical Kinetics

The Elements: the Main Group Elements

The Elements: The D Block

Nuclear Chemistry

Organic Chemistry I

Organic Chemistry II

Filters

Exam 11: Chemical Equilibria

Given: 4NH3(g)+ 5O2(g) → 4NO(g)+ 6H2O(g) K Calculate the equilibrium constant for the following reaction. 2NO(g)+ 3H2O(g) →2NH3(g)+ O2(g)

At 600 ∘\circ∘ C,Kc = 2.8 for the reaction 2HgO(s) → 2Hg(l)+ O2(g) Calculate K at 600 ∘\circ∘ C for this reaction.

At 600 ∘\circ∘ C,the equilibrium constant for the reaction 2HgO(s) → 2Hg(l)+ O2(g) Is 2.8.Calculate the equilibrium constant for the reaction 1/2O2(g)+ Hg(l) → HgO(s)

At 25 ∘\circ∘ C,K = 6.9 * 105 for the reaction N2(g)+ 3H2(g) →2NH3(g) Calculate Kc at 25 ∘\circ∘ C for this reaction.

Given: 2P(g)+ 3Cl2(g) →2PCl3(g)K = 15.0 PCl3(g)+ Cl2(g) →PCl5(g)K = 4.0 What is the value of the equilibrium constant for the reaction below? 2P(g)+ 5Cl2(g) →2PCl5(g)

An endothermic reaction is most likely to have a small equilibrium constant if Δ\DeltaΔ Sro is small.

At 700 K,K = 54 for the reaction H2(g)+ I2(g) →2HI(g) Calculate Kc at 700 K for this reaction.

Consider the reaction 4NH3(g)+ 3O2(g) →2N2(g)+ 6H2O(g),K = 1080 at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of oxygen is

The vapor pressure of acetic acid at 25 ∘\circ∘ C is 16 Torr. Δ\DeltaΔ Gr for the reaction CH3COOH(l) →CH3COOH(g) At 25 ∘\circ∘ C is

For the reaction 2CaSO4(s) → 2CaO(s)+ 2SO2(g)+ O2(g) K = 0.032 at 700 K.What is the total pressure starting from pure CaSO4(s)?

For a pure solid or liquid,the molar free energy always has its standard value.

The van't Hoff equation can be used to obtain the standard reaction enthalpy for a reaction if the equilibrium constant for the reaction is known at two different temperatures.

For the equilibrium CaCO3(s) → CaO(s)+ CO2(g),(a)represents the composition at equilibrium at a certain temperature.In (b),a small amount of Ca*CO3(s)has been added (Ca*CO3(s)represents Ca14CO3(s)or labeled calcium carbonate).Draw the composition in (c)at equilibrium and explain your drawing.

The equilibrium constant,Kc,for the reaction 2NOCl(g) →2NO(g)+ Cl2(g) Is 0.51 at a certain temperature.A mixture of NOCl,NO,and Cl2 with concentrations 1.3,1.2,and 0.60 M,respectively,was introduced into a container at this temperature.Which of the following is true?

The effect of a volume decrease on the reaction C(s)+ H2O(g) → CO(g)+ H2(g) Is

Write the equilibrium constant for 2NaBr(aq)+ Pb(ClO4)2(aq) →PbBr2(s)+ 2NaClO4(aq).

Consider the reaction 2CuBr2(s) →\rightarrow→ 2CuBr(s)+ Br2(g) If the equilibrium vapor pressure of Br2(g)is 1.43 * 10-5 Torr at 298 K,what is Δ\DeltaΔ G at this temperature when Br2(g)is produced at a pressure of 7.50 * 10-8 Torr.

Consider the following reaction at a certain temperature: PCl5(g) →PCl3(g)+ Cl2(g) Kc = 0.100 At equilibrium,[PCl5] = 2.00 M and [PCl3] = [Cl2] = 1.00 M.If suddenly 1.00 M PCl3(g)and Cl2(g)is added,what is the equilibrium concentration of PCl5(g)?

Which of the following statements is true?

The Quantum World

Quantum Mechanics in Action: Atoms

Chemical Bonds

Molecular Shape and Structure

The Properties of Gases

Liquids and Solids

Inorganic Materials

Thermodynamics: The First Law

Thermodynamics: The Second and Third Laws

Physical Equilibria

Acids and Bases

Aqueous Equilibria

Electrochemistry

Chemical Kinetics

The Elements: the Main Group Elements

The Elements: The D Block

Nuclear Chemistry

Organic Chemistry I

Organic Chemistry II

Filters

Given: 4NH₃(g)+ 5O₂(g) → 4NO(g)+ 6H₂O(g) K Calculate the equilibrium constant for the following reaction. 2NO(g)+ 3H₂O(g) →2NH₃(g)+ O₂(g)

At 600^$\circ$C,K_c = 2.8 for the reaction 2HgO(s) → 2Hg(l)+ O₂(g) Calculate K at 600^$\circ$C for this reaction.

At 25^$\circ$C,K = 6.9 * 10⁵ for the reaction N₂(g)+ 3H₂(g) →2NH₃(g) Calculate K_c at 25^$\circ$C for this reaction.

Given: 2P(g)+ 3Cl₂(g) →2PCl₃(g)K = 15.0 PCl₃(g)+ Cl₂(g) →PCl₅(g)K = 4.0 What is the value of the equilibrium constant for the reaction below? 2P(g)+ 5Cl₂(g) →2PCl₅(g)

An endothermic reaction is most likely to have a small equilibrium constant if $\Delta$ S_r^o is small.

At 700 K,K = 54 for the reaction H₂(g)+ I₂(g) →2HI(g) Calculate K_c at 700 K for this reaction.

Consider the reaction 4NH₃(g)+ 3O₂(g) →2N₂(g)+ 6H₂O(g),K = 10⁸⁰ at a certain temperature. Initially,all reactants and products have concentrations equal to 12 M.At equilibrium,the approximate concentration of oxygen is

The vapor pressure of acetic acid at 25^$\circ$C is 16 Torr. $\Delta$ G_r for the reaction CH₃COOH(l) →CH₃COOH(g) At 25^$\circ$C is

For the reaction 2CaSO₄(s) → 2CaO(s)+ 2SO₂(g)+ O₂(g) K = 0.032 at 700 K.What is the total pressure starting from pure CaSO₄(s)?

The equilibrium constant,K_c,for the reaction 2NOCl(g) →2NO(g)+ Cl₂(g) Is 0.51 at a certain temperature.A mixture of NOCl,NO,and Cl₂ with concentrations 1.3,1.2,and 0.60 M,respectively,was introduced into a container at this temperature.Which of the following is true?

The effect of a volume decrease on the reaction C(s)+ H₂O(g) → CO(g)+ H₂(g) Is

Write the equilibrium constant for 2NaBr(aq)+ Pb(ClO₄)₂(aq) →PbBr₂(s)+ 2NaClO₄(aq).

Consider the reaction 2CuBr₂(s) $\rightarrow$ 2CuBr(s)+ Br₂(g) If the equilibrium vapor pressure of Br₂(g)is 1.43 * 10^-5 Torr at 298 K,what is $\Delta$ G at this temperature when Br₂(g)is produced at a pressure of 7.50 * 10^-8 Torr.

Consider the following reaction at a certain temperature: PCl₅(g) →PCl₃(g)+ Cl₂(g) K_c = 0.100 At equilibrium,[PCl₅] = 2.00 M and [PCl₃] = [Cl₂] = 1.00 M.If suddenly 1.00 M PCl₃(g)and Cl₂(g)is added,what is the equilibrium concentration of PCl₅(g)?