Consider the reversible reaction: 2NO2(g) N2O4(g) If the concentrations of both NO2 and N2O4 are each 0.016 M,what is the value of Qc?

A) 0.016 B) 0.50 C) 1.0 D) 2.0 E) 63 A) 0.016 B) 0.50 C) 1.0 D) 2.0 E) 63

Hydrogen sulfide can be formed in the following reaction: H2(g)+ S2(g) H2S(g); ΔH°rxn = -92 kJ/mol The equilibrium constant,KP,is 106 at 1023 K.Estimate the value of KP at 1218 K.(R = 8.314 J/K • mol)

A) 5.05 B) 18.8 C) 34.7 D) 88.9 E) 598 A) 5.05 B) 18.8 C) 34.7 D) 88.9 E) 598

The equilibrium constant KP at 427°C for the reaction N2(g)+ 3H2(g) 2NH3(g)is 9.4 ×10-5.What is ΔG° for the reaction under these conditions? (R = 8.314 J/K • mol)

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

Suppose 75.0 g of PCl5(g)is introduced into an evacuated 3.00-L vessel and allowed to reach equilibrium at 250ºC. PCl5(g) PCl3(g)+ Cl2(g) If KP = 1.80 for this reaction,what is the total pressure inside the vessel at equilibrium? (R =0.0821 atm • L/mol • K)

A) 2.88 atm B) 2.28 atm C) 4.54 atm D) 7.43 atm E) 9.69 atm A) 2.88 atm B) 2.28 atm C) 4.54 atm D) 7.43 atm E) 9.69 atm

Exam 15: Chemical Equilibrium

For the endothermic reaction A2(g) 2A(g),a snapshot of an equilibrium mixture of A(g)and A2(g)at low temperature may look as follows.(Each circle represents 1.0 mol of A atoms,and the volume of the box is 1.0 L.) If the system pressure is lowered,what might the new equilibrium system look like?

(Multiple Choice)

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Question 81

Consider the reversible reaction: 2NO₂(g) N₂O₄(g) If the concentrations of both NO₂ and N₂O₄ are each 0.016 M,what is the value of Q_c?

(Multiple Choice)

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Question 82

A container was charged with hydrogen,nitrogen,and ammonia gases at 120°C and the system was allowed to reach equilibrium.What will happen if the volume of the container is increased at constant temperature? 3H₂(g)+ N₂(g) 2NH₃(g)

(Multiple Choice)

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Question 83

Which substances are included in the equilibrium constant expression,K_c?

(Multiple Choice)

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Question 84

When the concentrations of both the reactants and products remain constant because the forward and reverse reactions are occurring at the same rate then the system is ________________.

(Short Answer)

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Question 85

A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium.The equilibrium concentration of COBr₂ was 0.233 M.What is K_c for this reaction? CO(g)+ Br₂(g) COBr₂(g)

(Multiple Choice)

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Question 86

Hydrogen sulfide can be formed in the following reaction: H₂(g)+ S₂(g) H₂S(g); ΔH°_rxn = -92 kJ/mol The equilibrium constant,K_P,is 106 at 1023 K.Estimate the value of K_P at 1218 K.(R = 8.314 J/K • mol)

(Multiple Choice)

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Question 87

Which is the correct equilibrium constant expression for the following reaction? 2BrCl₃(g) Br₂(g)+ 3Cl₂(g)

(Multiple Choice)

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Question 88

At 250ºC,the equilibrium constant,K_P,for the reaction PCl⁵(g) PCl₃(g)+ Cl₂(g)is 1.80. Sufficient PCl₅ is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC.What is the partial pressure of PCl₅ after the system has reached equilibrium.

(Multiple Choice)

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Question 89

If the system 3H₂(g)+ N₂(g) 2NH₃(g)is at equilibrium and more N₂ is added,a net reaction that consumes some of the added N₂ will occur until a new equilibrium is reached.

(True/False)

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Question 90

Which statement is correct?

(Multiple Choice)

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Question 91

The equilibrium constant K_P at 427°C for the reaction N₂(g)+ 3H₂(g) 2NH₃(g)is 9.4 ×10^-5.What is ΔG° for the reaction under these conditions? (R = 8.314 J/K • mol)

(Multiple Choice)

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Question 92

Nitric oxide and bromine were allowed to react in a sealed container.When equilibrium was reached,the following partial pressures of three gases were measured: NO: 0.526 atm; Br₂ :1.59 atm; NOBr: 7.68 atm.Calculate K_P for the reaction. 2NO(g)+ Br₂(g) 2NOBr(g)

(Multiple Choice)

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Question 93

Consider the equilibrium reaction: N₂O₄(g) 2NO₂(g) Which of the following correctly describes the relationship between K_c and K_P for the reaction?

(Multiple Choice)

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Question 94

If,in a particular process,reactants are able to form products,and products are also able to form reactants,then this process may be described as

(Multiple Choice)

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Question 95

Suppose 75.0 g of PCl₅(g)is introduced into an evacuated 3.00-L vessel and allowed to reach equilibrium at 250ºC. PCl₅(g) PCl₃(g)+ Cl₂(g) If K_P = 1.80 for this reaction,what is the total pressure inside the vessel at equilibrium? (R =0.0821 atm • L/mol • K)

(Multiple Choice)

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Question 96

A quantity of liquid methanol,CH₃OH,is introduced into a rigid 3.00-L vessel,the vessel is sealed,and the temperature is raised to 500 K.At this temperature,the methanol vaporizes and decomposes according to the reaction CH₃OH(g) CO(g)+ 2H₂(g),K_c = 6.90 ×10^-2 If the concentration of H₂ in the equilibrium mixture is 0.426 M,what mass of methanol was initially introduced into the vessel?

(Multiple Choice)

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Question 97

The equilibrium constant,K_P,has a value of 6.5 × 10^-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g)+ Cl₂(g) 2NOCl(g) What is the value of K_c? (R = 0.08206 L • atm/K • mol)

(Multiple Choice)

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Question 98

In the gas phase,formic acid forms a dimer,2HCOOH(g) (HCOOH)₂(g).For this reaction,ΔH° = -60.1 kJ/mol and ΔG° = -13.9 kJ/mol at 25°C.Find the equilibrium constant (K_P)for this reaction at 75 °C.

(Multiple Choice)

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Question 99

Suppose 50.0 g of N₂O₄ is introduced into an evacuated 2.00-L vessel and allowed to come to equilibrium with its decomposition product,N₂O₄(g) 2NO₂(g).For this reaction K_c = 0.133.Once the system has reached equilibrium,5.00 g of NO2 is injected into the vessel,and the system is allowed to equilibrate once again.What is the mass of NO₂ in the final equilibrium mixture?

(Multiple Choice)

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Question 100

Showing 81 - 100 of 135

Exam 15: Chemical Equilibrium

For the endothermic reaction A2(g) 2A(g),a snapshot of an equilibrium mixture of A(g)and A2(g)at low temperature may look as follows.(Each circle represents 1.0 mol of A atoms,and the volume of the box is 1.0 L.) If the system pressure is lowered,what might the new equilibrium system look like?

Consider the reversible reaction: 2NO2(g) N2O4(g) If the concentrations of both NO2 and N2O4 are each 0.016 M,what is the value of Qc?

A container was charged with hydrogen,nitrogen,and ammonia gases at 120°C and the system was allowed to reach equilibrium.What will happen if the volume of the container is increased at constant temperature? 3H2(g)+ N2(g) 2NH3(g)

Which substances are included in the equilibrium constant expression,Kc?

When the concentrations of both the reactants and products remain constant because the forward and reverse reactions are occurring at the same rate then the system is ________________.

A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium.The equilibrium concentration of COBr2 was 0.233 M.What is Kc for this reaction? CO(g)+ Br2(g) COBr2(g)

Hydrogen sulfide can be formed in the following reaction: H2(g)+ S2(g) H2S(g); ΔH°rxn = -92 kJ/mol The equilibrium constant,KP,is 106 at 1023 K.Estimate the value of KP at 1218 K.(R = 8.314 J/K • mol)

Which is the correct equilibrium constant expression for the following reaction? 2BrCl3(g) Br2(g)+ 3Cl2(g)

At 250ºC,the equilibrium constant,KP,for the reaction PCl5(g) PCl3(g)+ Cl2(g)is 1.80. Sufficient PCl5 is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC.What is the partial pressure of PCl5 after the system has reached equilibrium.

If the system 3H2(g)+ N2(g) 2NH3(g)is at equilibrium and more N2 is added,a net reaction that consumes some of the added N2 will occur until a new equilibrium is reached.

Which statement is correct?

The equilibrium constant KP at 427°C for the reaction N2(g)+ 3H2(g) 2NH3(g)is 9.4 ×10-5.What is ΔG° for the reaction under these conditions? (R = 8.314 J/K • mol)

Nitric oxide and bromine were allowed to react in a sealed container.When equilibrium was reached,the following partial pressures of three gases were measured: NO: 0.526 atm; Br2 :1.59 atm; NOBr: 7.68 atm.Calculate KP for the reaction. 2NO(g)+ Br2(g) 2NOBr(g)

Consider the equilibrium reaction: N2O4(g) 2NO2(g) Which of the following correctly describes the relationship between Kc and KP for the reaction?

If,in a particular process,reactants are able to form products,and products are also able to form reactants,then this process may be described as

Suppose 75.0 g of PCl5(g)is introduced into an evacuated 3.00-L vessel and allowed to reach equilibrium at 250ºC. PCl5(g) PCl3(g)+ Cl2(g) If KP = 1.80 for this reaction,what is the total pressure inside the vessel at equilibrium? (R =0.0821 atm • L/mol • K)

The equilibrium constant,KP,has a value of 6.5 × 10-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g)+ Cl2(g) 2NOCl(g) What is the value of Kc? (R = 0.08206 L • atm/K • mol)

In the gas phase,formic acid forms a dimer,2HCOOH(g) (HCOOH)2(g).For this reaction,ΔH° = -60.1 kJ/mol and ΔG° = -13.9 kJ/mol at 25°C.Find the equilibrium constant (KP)for this reaction at 75 °C.

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Consider the reversible reaction: 2NO₂(g) N₂O₄(g) If the concentrations of both NO₂ and N₂O₄ are each 0.016 M,what is the value of Q_c?

A container was charged with hydrogen,nitrogen,and ammonia gases at 120°C and the system was allowed to reach equilibrium.What will happen if the volume of the container is increased at constant temperature? 3H₂(g)+ N₂(g) 2NH₃(g)

Which substances are included in the equilibrium constant expression,K_c?

A mixture of 0.500 mole of carbon monoxide and 0.400 mole of bromine was placed into a rigid 1.00-L container and the system was allowed to come to equilibrium.The equilibrium concentration of COBr₂ was 0.233 M.What is K_c for this reaction? CO(g)+ Br₂(g) COBr₂(g)

Hydrogen sulfide can be formed in the following reaction: H₂(g)+ S₂(g) H₂S(g); ΔH°_rxn = -92 kJ/mol The equilibrium constant,K_P,is 106 at 1023 K.Estimate the value of K_P at 1218 K.(R = 8.314 J/K • mol)

Which is the correct equilibrium constant expression for the following reaction? 2BrCl₃(g) Br₂(g)+ 3Cl₂(g)

At 250ºC,the equilibrium constant,K_P,for the reaction PCl⁵(g) PCl₃(g)+ Cl₂(g)is 1.80. Sufficient PCl₅ is put into a reaction vessel to give an initial pressure of 2.74 atm at 250ºC.What is the partial pressure of PCl₅ after the system has reached equilibrium.

If the system 3H₂(g)+ N₂(g) 2NH₃(g)is at equilibrium and more N₂ is added,a net reaction that consumes some of the added N₂ will occur until a new equilibrium is reached.

The equilibrium constant K_P at 427°C for the reaction N₂(g)+ 3H₂(g) 2NH₃(g)is 9.4 ×10^-5.What is ΔG° for the reaction under these conditions? (R = 8.314 J/K • mol)

Nitric oxide and bromine were allowed to react in a sealed container.When equilibrium was reached,the following partial pressures of three gases were measured: NO: 0.526 atm; Br₂ :1.59 atm; NOBr: 7.68 atm.Calculate K_P for the reaction. 2NO(g)+ Br₂(g) 2NOBr(g)

Consider the equilibrium reaction: N₂O₄(g) 2NO₂(g) Which of the following correctly describes the relationship between K_c and K_P for the reaction?

Suppose 75.0 g of PCl₅(g)is introduced into an evacuated 3.00-L vessel and allowed to reach equilibrium at 250ºC. PCl₅(g) PCl₃(g)+ Cl₂(g) If K_P = 1.80 for this reaction,what is the total pressure inside the vessel at equilibrium? (R =0.0821 atm • L/mol • K)

The equilibrium constant,K_P,has a value of 6.5 × 10^-4 at 308 K for the reaction of nitrogen monoxide with chlorine. 2NO(g)+ Cl₂(g) 2NOCl(g) What is the value of K_c? (R = 0.08206 L • atm/K • mol)

In the gas phase,formic acid forms a dimer,2HCOOH(g) (HCOOH)₂(g).For this reaction,ΔH° = -60.1 kJ/mol and ΔG° = -13.9 kJ/mol at 25°C.Find the equilibrium constant (K_P)for this reaction at 75 °C.