Ozone is formed from oxygen.3 O2(g) 2 O3(g) Calculate the value of Kp,given that Kc = 2.5 $\times$10-29 at 298 K.(R = 0.08206 L.atm/mol.K)

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

Given the following chemical equilibrium, COCl2(g) CO(g)+ Cl2(g) Calculate the value of Kc,given that Kp = 6.5 $\times$ 1011 at 298 K.(R = 0.08206 L.atm/mol.K)

A) 1.5 $\times$ 10-12 B) 3.8 $\times$ 10-11 C) 1.1 $\times$ 109 D) 2.7 $\times$ 1010 E) 1.6 $\times$ 1013 A) 1.5 $\times$ 10-12 B) 3.8 $\times$ 10-11 C) 1.1 $\times$ 109 D) 2.7 $\times$ 1010 E) 1.6 $\times$ 1013

Consider the following reaction: Given that 1.00 mol of HF(g),0.389 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 = 0.0729 B) Q = 0.292 C) Q = 0.0584 D) Q = 2.14 E) none of these A) Q = 0.0729 B) Q = 0.292 C) Q = 0.0584 D) Q = 2.14 E) none of these

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 0.191 mol H2 and 0.191 mol I2 at equilibrium.What is the equilibrium constant Kc for the following reaction at 460°C? ½ H2(g)+ ½ I2(g) HI(g)

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

Consider the following equilibrium: Suppose 15.6 g each of CH4,C2H6,C5H12,and C6H14 are placed in a 45.0-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.

Given the equilibrium constants for the equilibria, 2NH4+(aq)+ 2H2O(l) 2NH3(aq)+ 2H3O+(aq); Kc = CH3COOH(aq)+ H2O(l) CH3COO-(aq)+ H3O+(aq); Kc = Determine Kc for the following equilibrium. CH3COOH(aq)+ NH3(aq) CH3COO-(aq)+ NH4+(aq)

A) 3.08 $\times$ 104 B) 3.25 $\times$ 10-5 C) 9.96 $\times$ 10-15 D) 1.00 $\times$ 1014 E) 1.75 $\times$ 10-5 A) 3.08 $\times$ 104 B) 3.25 $\times$ 10-5 C) 9.96 $\times$ 10-15 D) 1.00 $\times$ 1014 E) 1.75 $\times$ 10-5

If Kc = 0.152 for A2 + 2B 2AB,what is the value of Kc for the reaction 4AB 2A2 + 4B?

A) 0.152 B) 0.304 C) 43.3 D) -0.152 E) 3.29 A) 0.152 B) 0.304 C) 43.3 D) -0.152 E) 3.29

Exam 16: Principles of Reactivity: Chemical Equilibria

Ozone is formed from oxygen.3 O₂(g) $Ozone is formed from oxygen.3 O2(g) 2 O3(g) Calculate the value of Kp,given that Kc = 2.5 \times 10-29 at 298 K.(R = 0.08206 L.atm/mol.K)$ 2 O₃(g) Calculate the value of K_p,given that K_c = 2.5 $\times$ 10^-29 at 298 K.(R = 0.08206 L.atm/mol.K)

(Multiple Choice)

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Question 61

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 62

If a stress is applied to an equilibrium system,the system will respond in such a way as to relieve that stress.This is a statement of ________ principle.

(Short Answer)

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Question 63

At 25 ^$\circ$C,the decomposition of dinitrogen tetraoxide N₂O₄(g) $At 25 \circ C,the decomposition of dinitrogen tetraoxide N2O4(g) 2 NO2(g) Has an equilibrium constant (Kp)of 0.144.At equilibrium,the total pressure of the system is 0.0758 atm.What is the partial pressure of each gas?$ 2 NO₂(g) Has an equilibrium constant (K_p)of 0.144.At equilibrium,the total pressure of the system is 0.0758 atm.What is the partial pressure of each gas?

(Multiple Choice)

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Question 64

For which one of the following reactions does K_p equal K_c?

(Multiple Choice)

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Question 65

What is the balanced equation for the following equilibrium expression?

(Multiple Choice)

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Question 66

Given the following chemical equilibrium, COCl₂(g) $Given the following chemical equilibrium, COCl2(g) CO(g)+ Cl2(g) Calculate the value of Kc,given that Kp = 6.5 \times 1011 at 298 K.(R = 0.08206 L.atm/mol.K)$ CO(g)+ Cl₂(g) Calculate the value of K_c,given that K_p = 6.5 $\times$ 10¹¹ at 298 K.(R = 0.08206 L.atm/mol.K)

(Multiple Choice)

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Question 67

Consider the following reaction: Given that 1.00 mol of HF(g),0.389 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 68

Write the expression for K_p for the reaction below.

(Multiple Choice)

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Question 69

A 3.00-liter flask initially contains 3.00 mol of gas A and 1.50 mol of gas B.Gas A decomposes according to the following reaction: The equilibrium concentration of gas C is 0.146 mol/L.Determine the value of the equilibrium constant,K_c.

(Multiple Choice)

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Question 70

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 0.191 mol H₂ and 0.191 mol I₂ at equilibrium.What is the equilibrium constant K_c for the following reaction at 460°C? ½ H₂(g)+ ½ I₂(g) HI(g)

(Multiple Choice)

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Question 71

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

(Multiple Choice)

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Question 72

Consider the following equilibrium: Suppose 15.6 g each of CH₄,C₂H₆,C₅H₁₂,and C₆H₁₄ are placed in a 45.0-L reaction vessel at 500 K.Which of the following statements is correct?

(Multiple Choice)

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Question 73

At 800 K,the equilibrium constant,K_p,for the following reaction is 3.2 $\times$ 10^-7.2 H₂S(g) $At 800 K,the equilibrium constant,Kp,for the following reaction is 3.2 \times 10-7.2 H2S(g) 2 H2(g)+ S2(g) A reaction vessel at 800 K initially contains 3.00 atm of H2S.If the reaction is allowed to equilibrate,what is the equilibrium pressure of S2?$ 2 H₂(g)+ S₂(g) A reaction vessel at 800 K initially contains 3.00 atm of H₂S.If the reaction is allowed to equilibrate,what is the equilibrium pressure of S₂?

(Multiple Choice)

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Question 74

Given the equilibrium constants for the equilibria, 2NH₄⁺(aq)+ 2H₂O(l) 2NH₃(aq)+ 2H₃O⁺(aq); K_c = CH₃COOH(aq)+ H₂O(l) CH₃COO^-(aq)+ H₃O⁺(aq); K_c = Determine K_c for the following equilibrium. CH₃COOH(aq)+ NH₃(aq) CH₃COO^-(aq)+ NH₄⁺(aq)

(Multiple Choice)

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Question 75

Consider the following equilibrium at 25°C: 2ICl(g) $Consider the following equilibrium at 25°C: 2ICl(g) I2(g)+ Cl2(g); \Delta H = 27 kJ; Kp = 6.2 \times 10-6 Which of the following would be true if the temperature were increased to 100°C? 1)The value of Kp would increase. 2)The concentration of ICl(g)would increase. 3)The partial pressure of I2 would increase.$ I₂(g)+ Cl₂(g); $\Delta$ H = 27 kJ; K_p = 6.2 $\times$ 10^-6 Which of the following would be true if the temperature were increased to 100°C? 1)The value of K_p would increase. 2)The concentration of ICl(g)would increase. 3)The partial pressure of I₂ would increase.

(Multiple Choice)

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Question 76

Write the expression for K for the reaction below.

(Multiple Choice)

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Question 77

If K_c = 0.152 for A₂ + 2B 2AB,what is the value of K_c for the reaction 4AB 2A₂ + 4B?

(Multiple Choice)

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Question 78

What is the expression for K_c for the following equilibrium?

(Multiple Choice)

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Question 79

A sample of solid NH₄NO₃ was placed in an evacuated container and then heated so that it decomposed explosively according to the following equation: At equilibrium the total pressure in the container was found to be 2.81 atm at a temperature of 500.°C.Calculate K_p.

(Multiple Choice)

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Question 80

Showing 61 - 80 of 82

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.

If a stress is applied to an equilibrium system,the system will respond in such a way as to relieve that stress.This is a statement of ________ principle.

For which one of the following reactions does K_p equal K_c?

What is the balanced equation for the following equilibrium expression?

Consider the following reaction: Given that 1.00 mol of HF(g),0.389 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.

A 3.00-liter flask initially contains 3.00 mol of gas A and 1.50 mol of gas B.Gas A decomposes according to the following reaction: The equilibrium concentration of gas C is 0.146 mol/L.Determine the value of the equilibrium constant,K_c.

Consider the following equilibrium: Suppose 15.6 g each of CH₄,C₂H₆,C₅H₁₂,and C₆H₁₄ are placed in a 45.0-L reaction vessel at 500 K.Which of the following statements is correct?

Given the equilibrium constants for the equilibria, 2NH₄⁺(aq)+ 2H₂O(l) 2NH₃(aq)+ 2H₃O⁺(aq); K_c = CH₃COOH(aq)+ H₂O(l) CH₃COO^-(aq)+ H₃O⁺(aq); K_c = Determine K_c for the following equilibrium. CH₃COOH(aq)+ NH₃(aq) CH₃COO^-(aq)+ NH₄⁺(aq)

Write the expression for K for the reaction below.

If K_c = 0.152 for A₂ + 2B 2AB,what is the value of K_c for the reaction 4AB 2A₂ + 4B?

What is the expression for K_c for the following equilibrium?

A sample of solid NH₄NO₃ was placed in an evacuated container and then heated so that it decomposed explosively according to the following equation: At equilibrium the total pressure in the container was found to be 2.81 atm at a temperature of 500.°C.Calculate K_p.

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Exam 16: Principles of Reactivity: Chemical Equilibria

Ozone is formed from oxygen.3 O2(g) 2 O3(g) Calculate the value of Kp,given that Kc = 2.5 ×\times× 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.

If a stress is applied to an equilibrium system,the system will respond in such a way as to relieve that stress.This is a statement of ________ principle.

At 25 ∘\circ∘ C,the decomposition of dinitrogen tetraoxide N2O4(g) 2 NO2(g) Has an equilibrium constant (Kp)of 0.144.At equilibrium,the total pressure of the system is 0.0758 atm.What is the partial pressure of each gas?

For which one of the following reactions does Kp equal Kc?

What is the balanced equation for the following equilibrium expression?

Given the following chemical equilibrium, COCl2(g) CO(g)+ Cl2(g) Calculate the value of Kc,given that Kp = 6.5 ×\times× 1011 at 298 K.(R = 0.08206 L.atm/mol.K)

Consider the following reaction: Given that 1.00 mol of HF(g),0.389 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.

A 3.00-liter flask initially contains 3.00 mol of gas A and 1.50 mol of gas B.Gas A decomposes according to the following reaction: The equilibrium concentration of gas C is 0.146 mol/L.Determine the value of the equilibrium constant,Kc.

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

Consider the following equilibrium: Suppose 15.6 g each of CH4,C2H6,C5H12,and C6H14 are placed in a 45.0-L reaction vessel at 500 K.Which of the following statements is correct?

At 800 K,the equilibrium constant,Kp,for the following reaction is 3.2 ×\times× 10-7.2 H2S(g) 2 H2(g)+ S2(g) A reaction vessel at 800 K initially contains 3.00 atm of H2S.If the reaction is allowed to equilibrate,what is the equilibrium pressure of S2?

Given the equilibrium constants for the equilibria, 2NH4+(aq)+ 2H2O(l) 2NH3(aq)+ 2H3O+(aq); Kc = CH3COOH(aq)+ H2O(l) CH3COO-(aq)+ H3O+(aq); Kc = Determine Kc for the following equilibrium. CH3COOH(aq)+ NH3(aq) CH3COO-(aq)+ NH4+(aq)

Write the expression for K for the reaction below.

If Kc = 0.152 for A2 + 2B 2AB,what is the value of Kc for the reaction 4AB 2A2 + 4B?

What is the expression for Kc for the following equilibrium?

A sample of solid NH4NO3 was placed in an evacuated container and then heated so that it decomposed explosively according to the following equation: At equilibrium the total pressure in the container was found to be 2.81 atm at a temperature of 500.°C.Calculate Kp.

Basic Concepts of Chemistry

Mathlets 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 Chemistry of Solids

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

The Chemistry of Acids and Bases

Principles of Reactivity: Other Aspects of Aqueous Equilibria

Entropy and Free Energy

Principles of 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

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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.

For which one of the following reactions does K_p equal K_c?

Consider the following reaction: Given that 1.00 mol of HF(g),0.389 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.

A 3.00-liter flask initially contains 3.00 mol of gas A and 1.50 mol of gas B.Gas A decomposes according to the following reaction: The equilibrium concentration of gas C is 0.146 mol/L.Determine the value of the equilibrium constant,K_c.

Consider the following equilibrium: Suppose 15.6 g each of CH₄,C₂H₆,C₅H₁₂,and C₆H₁₄ are placed in a 45.0-L reaction vessel at 500 K.Which of the following statements is correct?

Given the equilibrium constants for the equilibria, 2NH₄⁺(aq)+ 2H₂O(l) 2NH₃(aq)+ 2H₃O⁺(aq); K_c = CH₃COOH(aq)+ H₂O(l) CH₃COO^-(aq)+ H₃O⁺(aq); K_c = Determine K_c for the following equilibrium. CH₃COOH(aq)+ NH₃(aq) CH₃COO^-(aq)+ NH₄⁺(aq)

If K_c = 0.152 for A₂ + 2B 2AB,what is the value of K_c for the reaction 4AB 2A₂ + 4B?

What is the expression for K_c for the following equilibrium?

A sample of solid NH₄NO₃ was placed in an evacuated container and then heated so that it decomposed explosively according to the following equation: At equilibrium the total pressure in the container was found to be 2.81 atm at a temperature of 500.°C.Calculate K_p.