The Ostwald process converts ammonia (NH3)to nitric oxide (NO)by reaction with oxygen in the presence of a catalyst at high temperatures.In a test of the process a reaction vessel is initially charged with 4.80 mol NH3(g)and 5.80 mol O2(g),sealed,and heated at a fixed high temperature.When equilibrium is established the reaction mixture is analyzed and found to contain 3.80 mol NO(g).What is the quantity of NH3(g)in the equilibrium reaction mixture? 4NH3(g)+ 5O2(g) 4NO(g)+ 6H2O(g)

A) 1 mol NH3(g) B) 8.6 mol NH3(g) C) 4.8 mol NH3(g) D) 1.05 mol NH3(g) E) 2 mol NH3(g) A) 1 mol NH3(g) B) 8.6 mol NH3(g) C) 4.8 mol NH3(g) D) 1.05 mol NH3(g) E) 2 mol NH3(g)

Nitrogen trifluoride decomposes to form nitrogen and fluorine gases according to the following equation: 2NF3(g) N2(g)+ 3F2(g) When 2.54 mol of NF3 is placed in a 6.00-L container and allowed to come to equilibrium at 800 K,the mixture is found to contain 0.0434 mol of N2.What is the value of Kp at this temperature? (R = 0.0821 L · atm · mol-1 · K-1)

A) 1.54 × 10-5 B) 1.91 × 10-3 C) 1.78 × 10-3 D) 1.59 × 10-5 E) 4.43 × 10-7 A) 1.54 × 10-5 B) 1.91 × 10-3 C) 1.78 × 10-3 D) 1.59 × 10-5 E) 4.43 × 10-7

Consider the following equilibrium: C2H6(g)+ C5H12(g) CH4(g)+ C6H14(g); Kp = 9.57 at 500 K Suppose 11.6 g each of CH4,C2H6,C5H12,and C6H14 are placed in a 30.0-L reaction vessel at 500 K.Which of the following statements is correct?

A) Because Qc c,more products will be formed. B) Because Qc = 1,the system is at equilibrium. C) Because Qc = 1,more products will be formed. D) Because Qc = 1,more reactants will be formed. E) Because Qc > Kc,more reactants will be formed. A) Because Qc c,more products will be formed. B) Because Qc = 1,the system is at equilibrium. C) Because Qc = 1,more products will be formed. D) Because Qc = 1,more reactants will be formed. E) Because Qc > Kc,more reactants will be formed.

What effect will spraying liquid water into the equilibrium given below have if NH3 is far more soluble in water than is N2 or H2? N2(g)+ 3H2(g) 2NH3(g)

A) More NH3(g)will form. B) More H2(g)will form. C) Less NH3(g)will form. D) This will not affect the system. E) More N2(g)will form. A) More NH3(g)will form. B) More H2(g)will form. C) Less NH3(g)will form. D) This will not affect the system. E) More N2(g)will form.

When the pressure of an equilibrium mixture of SO2,O2,and SO3 is halved at constant temperature,what is the effect on Kp? 2SO2(g)+ O2(g) 2SO3(g)

A) Kp is doubled. B) Kp is halved. C) Kp is unchanged. D) Kp is tripled. E) Kp is decreased by a third. A) Kp is doubled. B) Kp is halved. C) Kp is unchanged. D) Kp is tripled. E) Kp is decreased by a third.

Consider the following equilibrium: O2(g)+ 2F2(g) 2OF2(g); Kp = 2.3 × 10-15 Which of the following statements is true?

A) If the reaction mixture initially contains only OF2(g),then at equilibrium,the reaction mixture will consist of essentially only O2(g)and F2(g). B) For this equilibrium,Kc = Kp. C) If the reaction mixture initially contains only OF2(g),then the total pressure at equilibrium will be less than the total initial pressure. D) If the reaction mixture initially contains only O2(g)and F2(g),then at equilibrium,the reaction mixture will consist of essentially only OF2(g). E) If the reaction mixture initially contains only O2(g)and F2(g),then the total pressure at equilibrium will be greater than the total initial pressure. A) If the reaction mixture initially contains only OF2(g),then at equilibrium,the reaction mixture will consist of essentially only O2(g)and F2(g). B) For this equilibrium,Kc = Kp. C) If the reaction mixture initially contains only OF2(g),then the total pressure at equilibrium will be less than the total initial pressure. D) If the reaction mixture initially contains only O2(g)and F2(g),then at equilibrium,the reaction mixture will consist of essentially only OF2(g). E) If the reaction mixture initially contains only O2(g)and F2(g),then the total pressure at equilibrium will be greater than the total initial pressure.

A 2.50-mol sample of HI is placed in a 1.00-L vessel at 460°C,and the reaction system is allowed to come to equilibrium.The HI partially decomposes,forming 0.190 mol H2 and 0.190 mol I2 at equilibrium.What is the equilibrium constant Kc for the following reaction at 460°C? 1/2 H2(g)+ 1/2 I2(g) HI(g)

A) 1.23 × 102 B) 8.10 × 10-3 C) 1.72 × 10-2 D) 11.1 E) 7.63 A) 1.23 × 102 B) 8.10 × 10-3 C) 1.72 × 10-2 D) 11.1 E) 7.63

At 550 K,Kp = 7.7 × 102 for the following equilibrium. SO2(g)+ NO2(g) SO3(g)+ NO(g) If 0.279 mol each of SO3 and NO are placed in a 4.00-L container at 550 K,what is the concentration of SO3 at equilibrium? (R = 0.0821 L · atm/(K · mol))

A) 3 M B) 0.067 M C) 0.069 M D) 17 M E) 0.017 M A) 3 M B) 0.067 M C) 0.069 M D) 17 M E) 0.017 M

If Kc = 0.133 for A2 + 2B 2AB,what is the value of Kc for the reaction 4AB 2A2 + 4B?

A) 0.133 B) 0.266 C) 56.5 D) -0.133 E) 3.76 A) 0.133 B) 0.266 C) 56.5 D) -0.133 E) 3.76

Exam 14: Chemical Equilibrium

The Ostwald process converts ammonia (NH₃)to nitric oxide (NO)by reaction with oxygen in the presence of a catalyst at high temperatures.In a test of the process a reaction vessel is initially charged with 4.80 mol NH₃(g)and 5.80 mol O₂(g),sealed,and heated at a fixed high temperature.When equilibrium is established the reaction mixture is analyzed and found to contain 3.80 mol NO(g).What is the quantity of NH₃(g)in the equilibrium reaction mixture? 4NH₃(g)+ 5O₂(g) 4NO(g)+ 6H₂O(g)

(Multiple Choice)

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Question 81

Nitrogen trifluoride decomposes to form nitrogen and fluorine gases according to the following equation: 2NF₃(g) N₂(g)+ 3F₂(g) When 2.54 mol of NF₃ is placed in a 6.00-L container and allowed to come to equilibrium at 800 K,the mixture is found to contain 0.0434 mol of N₂.What is the value of K_p at this temperature? (R = 0.0821 L · atm · mol^-1 · K^-1)

(Multiple Choice)

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Question 82

Consider the following equilibrium: C₂H₆(g)+ C₅H₁₂(g) CH₄(g)+ C₆H₁₄(g); K_p = 9.57 at 500 K Suppose 11.6 g each of CH₄,C₂H₆,C₅H₁₂,and C₆H₁₄ are placed in a 30.0-L reaction vessel at 500 K.Which of the following statements is correct?

(Multiple Choice)

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Question 83

Hydrogen iodide undergoes decomposition according to the equation 2HI(g) H₂(g)+ I₂(g) The equilibrium constant K_c at 425°C for this system is 0.018.If 1.0 mol each of H₂,I₂,and HI were placed together in a 1-L container at 425°C,then

(Multiple Choice)

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Question 84

What effect will spraying liquid water into the equilibrium given below have if NH₃ is far more soluble in water than is N₂ or H₂? N₂(g)+ 3H₂(g) 2NH₃(g)

(Multiple Choice)

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Question 85

In an experiment,0.30 mol H₂ and 0.30 mol I₂ are mixed in a 1.00-L container,and the reaction forms HI.If K_c = 49.for this reaction,what is the equilibrium concentration of HI? I₂(g)+ H₂(g) 2HI(g)

(Multiple Choice)

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Question 86

When the pressure of an equilibrium mixture of SO₂,O₂,and SO₃ is halved at constant temperature,what is the effect on K_p? 2SO₂(g)+ O₂(g) 2SO₃(g)

(Multiple Choice)

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Question 87

Consider the following equilibrium: NH₄Cl(s) NH₃(g)+ HCl(g) Suppose a vessel containing NH₄Cl(s),NH₃(g)and HCl(g)is at equilibrium.If the volume of the vessel is instantaneously doubled while keeping the temperature constant,when a new equilibrium is reached,which of the following statements is incorrect?

(Multiple Choice)

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Question 88

What is the K_c expression for the following equilibrium? CuBr(s) Cu⁺(aq)+ Br^-(aq)

(Multiple Choice)

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Question 89

Consider the following equilibrium: O₂(g)+ 2F₂(g) 2OF₂(g); K_p = 2.3 × 10^-15 Which of the following statements is true?

(Multiple Choice)

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Question 90

A 2.50-mol sample of HI is placed in a 1.00-L vessel at 460°C,and the reaction system is allowed to come to equilibrium.The HI partially decomposes,forming 0.190 mol H₂ and 0.190 mol I₂ at equilibrium.What is the equilibrium constant K_c for the following reaction at 460°C? 1/2 H₂(g)+ 1/2 I₂(g) HI(g)

(Multiple Choice)

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Question 91

For which of the following systems at equilibrium and at constant temperature will increasing the volume have no effect on the equilibrium?

(Multiple Choice)

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Question 92

The following equilibrium is exothermic.How could the yield of diiodine pentoxide be increased? I₂(g)+ 5CO₂(g) 5CO(g)+ I₂O₅(g)

(Multiple Choice)

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Question 93

At 550 K,K_p = 7.7 × 10² for the following equilibrium. SO₂(g)+ NO₂(g) SO₃(g)+ NO(g) If 0.279 mol each of SO₃ and NO are placed in a 4.00-L container at 550 K,what is the concentration of SO₃ at equilibrium? (R = 0.0821 L · atm/(K · mol))

(Multiple Choice)

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Question 94

For which of the following reactions will the reactant experience the largest degree of decomposition upon reaching equilibrium at 500 K?

(Multiple Choice)

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Question 95

If K_c = 0.133 for A₂ + 2B 2AB,what is the value of K_c for the reaction 4AB 2A₂ + 4B?

(Multiple Choice)

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Question 96

The _____ is a relation that states that the values of the equilibrium-constant expression K_c are constant for a particular reaction at a given temperature,whatever equilibrium concentrations are substituted.

(Multiple Choice)

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Question 97

Showing 81 - 97 of 97

Consider the following equilibrium: C₂H₆(g)+ C₅H₁₂(g) CH₄(g)+ C₆H₁₄(g); K_p = 9.57 at 500 K Suppose 11.6 g each of CH₄,C₂H₆,C₅H₁₂,and C₆H₁₄ are placed in a 30.0-L reaction vessel at 500 K.Which of the following statements is correct?

Hydrogen iodide undergoes decomposition according to the equation 2HI(g) H₂(g)+ I₂(g) The equilibrium constant K_c at 425°C for this system is 0.018.If 1.0 mol each of H₂,I₂,and HI were placed together in a 1-L container at 425°C,then

What effect will spraying liquid water into the equilibrium given below have if NH₃ is far more soluble in water than is N₂ or H₂? N₂(g)+ 3H₂(g) 2NH₃(g)

In an experiment,0.30 mol H₂ and 0.30 mol I₂ are mixed in a 1.00-L container,and the reaction forms HI.If K_c = 49.for this reaction,what is the equilibrium concentration of HI? I₂(g)+ H₂(g) 2HI(g)

When the pressure of an equilibrium mixture of SO₂,O₂,and SO₃ is halved at constant temperature,what is the effect on K_p? 2SO₂(g)+ O₂(g) 2SO₃(g)

What is the K_c expression for the following equilibrium? CuBr(s) Cu⁺(aq)+ Br^-(aq)

Consider the following equilibrium: O₂(g)+ 2F₂(g) 2OF₂(g); K_p = 2.3 × 10^-15 Which of the following statements is true?

For which of the following systems at equilibrium and at constant temperature will increasing the volume have no effect on the equilibrium?

The following equilibrium is exothermic.How could the yield of diiodine pentoxide be increased? I₂(g)+ 5CO₂(g) 5CO(g)+ I₂O₅(g)

At 550 K,K_p = 7.7 × 10² for the following equilibrium. SO₂(g)+ NO₂(g) SO₃(g)+ NO(g) If 0.279 mol each of SO₃ and NO are placed in a 4.00-L container at 550 K,what is the concentration of SO₃ at equilibrium? (R = 0.0821 L · atm/(K · mol))

For which of the following reactions will the reactant experience the largest degree of decomposition upon reaching equilibrium at 500 K?

If K_c = 0.133 for A₂ + 2B 2AB,what is the value of K_c for the reaction 4AB 2A₂ + 4B?

The _____ is a relation that states that the values of the equilibrium-constant expression K_c are constant for a particular reaction at a given temperature,whatever equilibrium concentrations are substituted.

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Exam 14: Chemical Equilibrium

Consider the following equilibrium: C2H6(g)+ C5H12(g) CH4(g)+ C6H14(g); Kp = 9.57 at 500 K Suppose 11.6 g each of CH4,C2H6,C5H12,and C6H14 are placed in a 30.0-L reaction vessel at 500 K.Which of the following statements is correct?

Hydrogen iodide undergoes decomposition according to the equation 2HI(g) H2(g)+ I2(g) The equilibrium constant Kc at 425°C for this system is 0.018.If 1.0 mol each of H2,I2,and HI were placed together in a 1-L container at 425°C,then

What effect will spraying liquid water into the equilibrium given below have if NH3 is far more soluble in water than is N2 or H2? N2(g)+ 3H2(g) 2NH3(g)

In an experiment,0.30 mol H2 and 0.30 mol I2 are mixed in a 1.00-L container,and the reaction forms HI.If Kc = 49.for this reaction,what is the equilibrium concentration of HI? I2(g)+ H2(g) 2HI(g)

When the pressure of an equilibrium mixture of SO2,O2,and SO3 is halved at constant temperature,what is the effect on Kp? 2SO2(g)+ O2(g) 2SO3(g)

What is the Kc expression for the following equilibrium? CuBr(s) Cu+(aq)+ Br-(aq)

Consider the following equilibrium: O2(g)+ 2F2(g) 2OF2(g); Kp = 2.3 × 10-15 Which of the following statements is true?

For which of the following systems at equilibrium and at constant temperature will increasing the volume have no effect on the equilibrium?

The following equilibrium is exothermic.How could the yield of diiodine pentoxide be increased? I2(g)+ 5CO2(g) 5CO(g)+ I2O5(g)

At 550 K,Kp = 7.7 × 102 for the following equilibrium. SO2(g)+ NO2(g) SO3(g)+ NO(g) If 0.279 mol each of SO3 and NO are placed in a 4.00-L container at 550 K,what is the concentration of SO3 at equilibrium? (R = 0.0821 L · atm/(K · mol))

For which of the following reactions will the reactant experience the largest degree of decomposition upon reaching equilibrium at 500 K?

If Kc = 0.133 for A2 + 2B 2AB,what is the value of Kc for the reaction 4AB 2A2 + 4B?

The _____ is a relation that states that the values of the equilibrium-constant expression Kc are constant for a particular reaction at a given temperature,whatever equilibrium concentrations are substituted.

Chemistry and Measurement

Atoms, molecules, and Ions

Calculations With Chemical Formulas and Equations

Chemical Reactions

The Gaseous State

Thermochemistry

Quantum Theory of the Atom

Electron Configurations and Periodicity

Ionic and Covalent Bonding

Molecular Geometry and Chemical Bonding Theory

States of Matter; Liquids and Solids

Solutions

Rates of Reaction

Acids and Bases

Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Thermodynamics and Equilibrium

Electrochemistry

Nuclear Chemistry

Chemistry of the Main-Group Metals

The Transition Elements and Coordination Compounds

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Polymer Materials: Synthetic and Biological

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Consider the following equilibrium: C₂H₆(g)+ C₅H₁₂(g) CH₄(g)+ C₆H₁₄(g); K_p = 9.57 at 500 K Suppose 11.6 g each of CH₄,C₂H₆,C₅H₁₂,and C₆H₁₄ are placed in a 30.0-L reaction vessel at 500 K.Which of the following statements is correct?

Hydrogen iodide undergoes decomposition according to the equation 2HI(g) H₂(g)+ I₂(g) The equilibrium constant K_c at 425°C for this system is 0.018.If 1.0 mol each of H₂,I₂,and HI were placed together in a 1-L container at 425°C,then

What effect will spraying liquid water into the equilibrium given below have if NH₃ is far more soluble in water than is N₂ or H₂? N₂(g)+ 3H₂(g) 2NH₃(g)

In an experiment,0.30 mol H₂ and 0.30 mol I₂ are mixed in a 1.00-L container,and the reaction forms HI.If K_c = 49.for this reaction,what is the equilibrium concentration of HI? I₂(g)+ H₂(g) 2HI(g)

When the pressure of an equilibrium mixture of SO₂,O₂,and SO₃ is halved at constant temperature,what is the effect on K_p? 2SO₂(g)+ O₂(g) 2SO₃(g)

What is the K_c expression for the following equilibrium? CuBr(s) Cu⁺(aq)+ Br^-(aq)

Consider the following equilibrium: O₂(g)+ 2F₂(g) 2OF₂(g); K_p = 2.3 × 10^-15 Which of the following statements is true?

The following equilibrium is exothermic.How could the yield of diiodine pentoxide be increased? I₂(g)+ 5CO₂(g) 5CO(g)+ I₂O₅(g)

At 550 K,K_p = 7.7 × 10² for the following equilibrium. SO₂(g)+ NO₂(g) SO₃(g)+ NO(g) If 0.279 mol each of SO₃ and NO are placed in a 4.00-L container at 550 K,what is the concentration of SO₃ at equilibrium? (R = 0.0821 L · atm/(K · mol))

If K_c = 0.133 for A₂ + 2B 2AB,what is the value of K_c for the reaction 4AB 2A₂ + 4B?

The _____ is a relation that states that the values of the equilibrium-constant expression K_c are constant for a particular reaction at a given temperature,whatever equilibrium concentrations are substituted.