A sample of solid NH4NO3 was placed in an evacuated container and then heated so that it decomposed explosively according to the following equation: NH4NO3(s) N2O(g)+ 2H2O(g) At equilibrium the total pressure in the container was found to be 2.72 atm at a temperature of 500.°C.Calculate Kp.

A) 1.64 B) 0.822 C) 2.98 D) 80.5 E) 0.745 A) 1.64 B) 0.822 C) 2.98 D) 80.5 E) 0.745

For the equilibrium N2O4(g) 2NO2(g),at 298 K,Kp = 0.15.For this reaction system,it is found that the partial pressure of N2O4 is 3.7 × 10-2 atm at equilibrium.What is the partial pressure of NO2 at equilibrium?

A) 4.9 atm B) 24 atm C) 0.0016 atm D) 0.0055 atm E) 0.074 atm A) 4.9 atm B) 24 atm C) 0.0016 atm D) 0.0055 atm E) 0.074 atm

Consider the following equilibrium: CO2(g)+ H2(g) CO(g)+ H2O(g); Kc = 1.6 at 1260 K Suppose 0.019 mol CO2 and 0.030 mol H2 are placed in a 3.00-L vessel at 1260 K.What is the equilibrium partial pressure of CO(g)? (R = 0.0821 L · atm/K·mol)

A) 4 atm B) 0.35 atm C) 1.6 atm D) 0.66 atm E) 1 atm A) 4 atm B) 0.35 atm C) 1.6 atm D) 0.66 atm E) 1 atm

The following reaction occurred when a 1.0-liter reaction vessel was initially charged with 2.0 moles of N2(g)and 4.0 moles of H2(g): 3H2(g)+ N2(g) 2NH3(g) Once equilibrium was established,the concentration of NH3(g)was determined to be 0.57 M at 700.°C.The value for Kc at 700.°C for the formation of ammonia is:

A) 3.2 × 10-1 B) 6.1 × 10-3 C) 1.1 × 10-1 D) 6.0 × 10-2 E) none of these A) 3.2 × 10-1 B) 6.1 × 10-3 C) 1.1 × 10-1 D) 6.0 × 10-2 E) none of these

Consider the formation of ozone by the following reaction. 3 O2(g) 2 O3(g) Calculate the value of Kp,given that Kc = 2.5 × 10-29 at 298 K.(R = 0.08206 L⋅atm/mol ⋅ K)

A) 1.0 × 10-30 B) 2.1 × 10-30 C) 2.5 × 10-29 D) 3.3 × 10-28 E) 6.1 ×10-28 A) 1.0 × 10-30 B) 2.1 × 10-30 C) 2.5 × 10-29 D) 3.3 × 10-28 E) 6.1 ×10-28

Consider the reaction below. 2 HF(g) H2(g)+ F2(g)(Kc = 1.00 × 10-2) Given that 1.00 mol of HF(g),0.241 mol of H2(g),and 0.750 mol of F2(g)are mixed in a 5.00 L flask,determine the reaction quotient,Q.

A) Q = 0.0452 B) Q = 0.181 C) Q = 0.0362 D) Q = 1.99 E) None of these A) Q = 0.0452 B) Q = 0.181 C) Q = 0.0362 D) Q = 1.99 E) None of these

When gaseous carbon monoxide and hydrogen are combined in a sealed vessel and heated they will eventually form an equilibrium mixture of reactants and products according to the balanced chemical equilibrium below. CO(g)+ 3H2(g) CH4(g)+ H2O(g) In one such reaction 3 moles of one reactant were combined with 1 mole of the other reactant in a fixed volume vessel and heated to 1200 K.Analysis of the reaction mixture at various times gave the results below.Which component of the reaction mixture is represented by curve B?

A) hydrogen B) carbon monoxide C) either methane or water D) either hydrogen or carbon monoxide E) not enough information to decide A) hydrogen B) carbon monoxide C) either methane or water D) either hydrogen or carbon monoxide E) not enough information to decide

For the reaction 2NO(g)+ O2(g) 2NO2(g)at 750°C,what is the relationship between Kc and Kp?

A) Kc = Kp B) Kc = Kp × (RT)-1 C) Kc = Kp = 1.0 D) Kc = Kp × (RT)¾ E) Kc = Kp × (RT)1 A) Kc = Kp B) Kc = Kp × (RT)-1 C) Kc = Kp = 1.0 D) Kc = Kp × (RT)¾ E) Kc = Kp × (RT)1

Consider the following equilibrium. PCl3(g)+ Cl2(g) PCl5(g) ΔH = -92 kJ The concentration of PCl3 at equilibrium can be increased by:

A) decreasing the temperature. B) adding Cl2 to the system. C) adding PCl5 to the system. D) increasing the pressure. E) adding a catalyst. A) decreasing the temperature. B) adding Cl2 to the system. C) adding PCl5 to the system. D) increasing the pressure. E) adding a catalyst.

Assume that the following chemical reaction is at equilibrium. 2 ICl(g) I2(g)+ Cl2(g) ΔH° = +26.9 kJ At 25 °C,Kp = 2.0 × 105.If the temperature is increase to 45 °C,which statement applies?

A) Kp will decrease and the reaction will proceed in the backward direction. B) Kp will decrease and the reaction will proceed in the forward direction. C) Kp will remain unchanged and the reaction will proceed in the forward direction. D) Kp will increase and the reaction will proceed in the backward direction. E) Kp will increase and the reaction will proceed in the forward direction. A) Kp will decrease and the reaction will proceed in the backward direction. B) Kp will decrease and the reaction will proceed in the forward direction. C) Kp will remain unchanged and the reaction will proceed in the forward direction. D) Kp will increase and the reaction will proceed in the backward direction. E) Kp will increase and the reaction will proceed in the forward direction.

Exam 16: Principles of Chemical Reactivity: Equilibria

A sample of solid NH₄NO₃ was placed in an evacuated container and then heated so that it decomposed explosively according to the following equation: NH₄NO₃(s) N₂O(g)+ 2H₂O(g) At equilibrium the total pressure in the container was found to be 2.72 atm at a temperature of 500.°C.Calculate K_p.

(Multiple Choice)

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Question 61

For the equilibrium N₂O₄(g) 2NO₂(g),at 298 K,K_p = 0.15.For this reaction system,it is found that the partial pressure of N₂O₄ is 3.7 × 10^-2 atm at equilibrium.What is the partial pressure of NO₂ at equilibrium?

(Multiple Choice)

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Question 62

Which of the following is the correct balanced equation for the equilibrium constant expression given below?

(Multiple Choice)

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Question 63

At 25 °C,0.138 mg AgBr dissolves in 10.0 L of water.What is the equilibrium constant for the reaction below? AgBr(s) Ag⁺(aq)+ Br^-(aq)

(Multiple Choice)

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Question 64

Consider the following equilibrium: CO₂(g)+ H₂(g) CO(g)+ H₂O(g); K_c = 1.6 at 1260 K Suppose 0.019 mol CO₂ and 0.030 mol H₂ are placed in a 3.00-L vessel at 1260 K.What is the equilibrium partial pressure of CO(g)? (R = 0.0821 L · atm/K·mol)

(Multiple Choice)

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Question 65

The following reaction occurred when a 1.0-liter reaction vessel was initially charged with 2.0 moles of N₂(g)and 4.0 moles of H₂(g): 3H₂(g)+ N₂(g) 2NH₃(g) Once equilibrium was established,the concentration of NH₃(g)was determined to be 0.57 M at 700.°C.The value for K_c at 700.°C for the formation of ammonia is:

(Multiple Choice)

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Question 66

Consider the formation of ozone by the following reaction. 3 O₂(g) 2 O₃(g) Calculate the value of K_p,given that K_c = 2.5 × 10^-29 at 298 K.(R = 0.08206 L⋅atm/mol ⋅ K)

(Multiple Choice)

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Question 67

The standard enthalpy of formation of ammonia is -46.1 kJ/mol. 1/2 N₂(g)+ 3/2 H₂(g) NH₃(g) Commercially,the reaction is carried out at high temperatures.Using your knowledge of kinetics and equilibrium,explain an advantage and a disadvantage of synthesizing ammonia at high temperatures.

(Essay)

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Question 68

Consider the reaction below. 2 HF(g) H₂(g)+ F₂(g)(K_c = 1.00 × 10^-2) Given that 1.00 mol of HF(g),0.241 mol of H₂(g),and 0.750 mol of F₂(g)are mixed in a 5.00 L flask,determine the reaction quotient,Q.

(Multiple Choice)

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Question 69

Write the expression for K_p for the reaction below. 2 NOBr(g) 2 NO(g)+ Br₂( )

(Multiple Choice)

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Question 70

When gaseous carbon monoxide and hydrogen are combined in a sealed vessel and heated they will eventually form an equilibrium mixture of reactants and products according to the balanced chemical equilibrium below. CO(g)+ 3H₂(g) CH₄(g)+ H₂O(g) In one such reaction 3 moles of one reactant were combined with 1 mole of the other reactant in a fixed volume vessel and heated to 1200 K.Analysis of the reaction mixture at various times gave the results below.Which component of the reaction mixture is represented by curve B?

(Multiple Choice)

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Question 71

Which of the following statements is true if reaction quotient (Q)is greater than equilibrium constant (K)?

(Multiple Choice)

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Question 72

For the reaction 2NO(g)+ O₂(g) 2NO₂(g)at 750°C,what is the relationship between K_c and K_p?

(Multiple Choice)

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Question 73

Consider the following equilibrium. PCl₃(g)+ Cl₂(g) PCl₅(g) ΔH = -92 kJ The concentration of PCl₃ at equilibrium can be increased by:

(Multiple Choice)

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Question 74

Assume that the following chemical reaction is at equilibrium. 2 ICl(g) I₂(g)+ Cl₂(g) ΔH° = +26.9 kJ At 25 °C,K_p = 2.0 × 10⁵.If the temperature is increase to 45 °C,which statement applies?

(Multiple Choice)

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Question 75

What is the K_c expression for the equilibrium given below? CuI(s) Cu⁺(aq)+ I−(aq)

(Multiple Choice)

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Question 76

Excess Ag₂SO₄(s)is placed in water at 25 °C.At equilibrium,the solution contains 0.029 M Ag⁺(aq).What is the equilibrium constant for the reaction below? Ag₂SO₄(s) 2 Ag⁺(aq)+ SO₄^2-(aq)

(Multiple Choice)

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Question 77

Showing 61 - 77 of 77

For the equilibrium N₂O₄(g) 2NO₂(g),at 298 K,K_p = 0.15.For this reaction system,it is found that the partial pressure of N₂O₄ is 3.7 × 10^-2 atm at equilibrium.What is the partial pressure of NO₂ at equilibrium?

Which of the following is the correct balanced equation for the equilibrium constant expression given below?

At 25 °C,0.138 mg AgBr dissolves in 10.0 L of water.What is the equilibrium constant for the reaction below? AgBr(s) Ag⁺(aq)+ Br^-(aq)

Consider the following equilibrium: CO₂(g)+ H₂(g) CO(g)+ H₂O(g); K_c = 1.6 at 1260 K Suppose 0.019 mol CO₂ and 0.030 mol H₂ are placed in a 3.00-L vessel at 1260 K.What is the equilibrium partial pressure of CO(g)? (R = 0.0821 L · atm/K·mol)

Consider the formation of ozone by the following reaction. 3 O₂(g) 2 O₃(g) Calculate the value of K_p,given that K_c = 2.5 × 10^-29 at 298 K.(R = 0.08206 L⋅atm/mol ⋅ K)

The standard enthalpy of formation of ammonia is -46.1 kJ/mol. 1/2 N₂(g)+ 3/2 H₂(g) NH₃(g) Commercially,the reaction is carried out at high temperatures.Using your knowledge of kinetics and equilibrium,explain an advantage and a disadvantage of synthesizing ammonia at high temperatures.

Consider the reaction below. 2 HF(g) H₂(g)+ F₂(g)(K_c = 1.00 × 10^-2) Given that 1.00 mol of HF(g),0.241 mol of H₂(g),and 0.750 mol of F₂(g)are mixed in a 5.00 L flask,determine the reaction quotient,Q.

Write the expression for K_p for the reaction below. 2 NOBr(g) 2 NO(g)+ Br₂( )

Which of the following statements is true if reaction quotient (Q)is greater than equilibrium constant (K)?

For the reaction 2NO(g)+ O₂(g) 2NO₂(g)at 750°C,what is the relationship between K_c and K_p?

Consider the following equilibrium. PCl₃(g)+ Cl₂(g) PCl₅(g) ΔH = -92 kJ The concentration of PCl₃ at equilibrium can be increased by:

Assume that the following chemical reaction is at equilibrium. 2 ICl(g) I₂(g)+ Cl₂(g) ΔH° = +26.9 kJ At 25 °C,K_p = 2.0 × 10⁵.If the temperature is increase to 45 °C,which statement applies?

What is the K_c expression for the equilibrium given below? CuI(s) Cu⁺(aq)+ I−(aq)

Excess Ag₂SO₄(s)is placed in water at 25 °C.At equilibrium,the solution contains 0.029 M Ag⁺(aq).What is the equilibrium constant for the reaction below? Ag₂SO₄(s) 2 Ag⁺(aq)+ SO₄^2-(aq)

Basic Concepts of Chemistry

Lets Review: The Tools of Quantitative Chemistry

Atoms, molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

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The Chemistry of the Main Group Elements

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Carbon: Not Just Another Element

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Exam 16: Principles of Chemical Reactivity: Equilibria

A sample of solid NH4NO3 was placed in an evacuated container and then heated so that it decomposed explosively according to the following equation: NH4NO3(s) N2O(g)+ 2H2O(g) At equilibrium the total pressure in the container was found to be 2.72 atm at a temperature of 500.°C.Calculate Kp.

For the equilibrium N2O4(g) 2NO2(g),at 298 K,Kp = 0.15.For this reaction system,it is found that the partial pressure of N2O4 is 3.7 × 10-2 atm at equilibrium.What is the partial pressure of NO2 at equilibrium?

Which of the following is the correct balanced equation for the equilibrium constant expression given below?

At 25 °C,0.138 mg AgBr dissolves in 10.0 L of water.What is the equilibrium constant for the reaction below? AgBr(s) Ag+(aq)+ Br-(aq)

Consider the following equilibrium: CO2(g)+ H2(g) CO(g)+ H2O(g); Kc = 1.6 at 1260 K Suppose 0.019 mol CO2 and 0.030 mol H2 are placed in a 3.00-L vessel at 1260 K.What is the equilibrium partial pressure of CO(g)? (R = 0.0821 L · atm/K·mol)

Consider the formation of ozone by the following reaction. 3 O2(g) 2 O3(g) Calculate the value of Kp,given that Kc = 2.5 × 10-29 at 298 K.(R = 0.08206 L⋅atm/mol ⋅ K)

The standard enthalpy of formation of ammonia is -46.1 kJ/mol. 1/2 N2(g)+ 3/2 H2(g) NH3(g) Commercially,the reaction is carried out at high temperatures.Using your knowledge of kinetics and equilibrium,explain an advantage and a disadvantage of synthesizing ammonia at high temperatures.

Consider the reaction below. 2 HF(g) H2(g)+ F2(g)(Kc = 1.00 × 10-2) Given that 1.00 mol of HF(g),0.241 mol of H2(g),and 0.750 mol of F2(g)are mixed in a 5.00 L flask,determine the reaction quotient,Q.

Write the expression for Kp for the reaction below. 2 NOBr(g) 2 NO(g)+ Br2( )

Which of the following statements is true if reaction quotient (Q)is greater than equilibrium constant (K)?

For the reaction 2NO(g)+ O2(g) 2NO2(g)at 750°C,what is the relationship between Kc and Kp?

Consider the following equilibrium. PCl3(g)+ Cl2(g) PCl5(g) ΔH = -92 kJ The concentration of PCl3 at equilibrium can be increased by:

Assume that the following chemical reaction is at equilibrium. 2 ICl(g) I2(g)+ Cl2(g) ΔH° = +26.9 kJ At 25 °C,Kp = 2.0 × 105.If the temperature is increase to 45 °C,which statement applies?

What is the Kc expression for the equilibrium given below? CuI(s) Cu+(aq)+ I−(aq)

Excess Ag2SO4(s)is placed in water at 25 °C.At equilibrium,the solution contains 0.029 M Ag+(aq).What is the equilibrium constant for the reaction below? Ag2SO4(s) 2 Ag+(aq)+ SO42-(aq)

Basic Concepts of Chemistry

Lets Review: The Tools of Quantitative Chemistry

Atoms, molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

For the equilibrium N₂O₄(g) 2NO₂(g),at 298 K,K_p = 0.15.For this reaction system,it is found that the partial pressure of N₂O₄ is 3.7 × 10^-2 atm at equilibrium.What is the partial pressure of NO₂ at equilibrium?

At 25 °C,0.138 mg AgBr dissolves in 10.0 L of water.What is the equilibrium constant for the reaction below? AgBr(s) Ag⁺(aq)+ Br^-(aq)

Consider the following equilibrium: CO₂(g)+ H₂(g) CO(g)+ H₂O(g); K_c = 1.6 at 1260 K Suppose 0.019 mol CO₂ and 0.030 mol H₂ are placed in a 3.00-L vessel at 1260 K.What is the equilibrium partial pressure of CO(g)? (R = 0.0821 L · atm/K·mol)

Consider the formation of ozone by the following reaction. 3 O₂(g) 2 O₃(g) Calculate the value of K_p,given that K_c = 2.5 × 10^-29 at 298 K.(R = 0.08206 L⋅atm/mol ⋅ K)

The standard enthalpy of formation of ammonia is -46.1 kJ/mol. 1/2 N₂(g)+ 3/2 H₂(g) NH₃(g) Commercially,the reaction is carried out at high temperatures.Using your knowledge of kinetics and equilibrium,explain an advantage and a disadvantage of synthesizing ammonia at high temperatures.

Consider the reaction below. 2 HF(g) H₂(g)+ F₂(g)(K_c = 1.00 × 10^-2) Given that 1.00 mol of HF(g),0.241 mol of H₂(g),and 0.750 mol of F₂(g)are mixed in a 5.00 L flask,determine the reaction quotient,Q.

Write the expression for K_p for the reaction below. 2 NOBr(g) 2 NO(g)+ Br₂( )

For the reaction 2NO(g)+ O₂(g) 2NO₂(g)at 750°C,what is the relationship between K_c and K_p?

Consider the following equilibrium. PCl₃(g)+ Cl₂(g) PCl₅(g) ΔH = -92 kJ The concentration of PCl₃ at equilibrium can be increased by:

Assume that the following chemical reaction is at equilibrium. 2 ICl(g) I₂(g)+ Cl₂(g) ΔH° = +26.9 kJ At 25 °C,K_p = 2.0 × 10⁵.If the temperature is increase to 45 °C,which statement applies?

What is the K_c expression for the equilibrium given below? CuI(s) Cu⁺(aq)+ I−(aq)

Excess Ag₂SO₄(s)is placed in water at 25 °C.At equilibrium,the solution contains 0.029 M Ag⁺(aq).What is the equilibrium constant for the reaction below? Ag₂SO₄(s) 2 Ag⁺(aq)+ SO₄^2-(aq)