Exactly 1.0 mol N2O4 is placed in an empty 1.0-L container and allowed to reach equilibrium described by the equation N2O4(g) 2NO2(g).If at equilibrium the N2O4 is 28.0% dissociated,what is the value of the equilibrium constant,Kc,for the reaction under these conditions?

A) 0.44 B) 2.3 C) 0.31 D) 0.78 E) 0.11 A) 0.44 B) 2.3 C) 0.31 D) 0.78 E) 0.11

Assume that the following chemical reaction is at equilibrium. 2 ICl(g) I2(g)+ Cl2(g)$~~~~~~~~$ $~~~~~~~~$ $\Delta$HS1U1P1$\circ$S1S1P0 = +26.9 kJ At 25 S1U1P1$\circ$S1S1P0C,Kp = 2.0 $\times$ 105.If the temperature is increase to 45 S1U1P1$\circ$S1S1P0C,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.

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 C?

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 NO(g)+ ½ O2(g) NO2(g)at 750°C,what is the relationship between Kc and Kp?

A) Kc = Kp B) Kc = Kp $\times$ (RT)-½ C) Kc = Kp = 1.0 D) Kc = Kp $\times$ (RT)¾ E) Kc = Kp $\times$ (RT)½ A) Kc = Kp B) Kc = Kp $\times$ (RT)-½ C) Kc = Kp = 1.0 D) Kc = Kp $\times$ (RT)¾ E) Kc = Kp $\times$ (RT)½

Which of the following is always true for a reaction where Kc is at 25S1U1P1$\circ$S1S1P0C?

A) The reaction mixture contains mostly products at equilibrium. B) The reaction mixture contains mostly reactants at equilibrium. C) The rate of reaction is very fast. D) There are approximately equal moles of reactants and products at equilibrium. E) Both A and C. A) The reaction mixture contains mostly products at equilibrium. B) The reaction mixture contains mostly reactants at equilibrium. C) The rate of reaction is very fast. D) There are approximately equal moles of reactants and products at equilibrium. E) Both A and C.

For which of the following reactions are the numerical values of Kp and Kc the same? 1. 2SOS1U1B12S1U1B0(g) + OS1U1B12S1U1B0(g) 2SO3(g) 2. N2(g) + O2(g) 2NO(g) 3. H2(g)+ I2(g) 2HI(g)

A) 1 only B) 2 only C) 1 and 2 D) 2 and 3 E) 1,2,and 3 A) 1 only B) 2 only C) 1 and 2 D) 2 and 3 E) 1,2,and 3

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 3.6 $\times$ 10-2 atm at equilibrium.What is the partial pressure of NO2 at equilibrium?

A) 4.9 atm B) 24 atm C) 0.0017 atm D) 0.0054 atm E) 0.073 atm A) 4.9 atm B) 24 atm C) 0.0017 atm D) 0.0054 atm E) 0.073 atm

Assume that the following $\underline{\text{ endothermic }}$chemical reaction is at equilibrium. C(s)+ H2O(g) H2(g)+ CO(g) Which of the following statements is/are CORRECT? 1)Increasing the concentration of H2(g)will cause the reaction to proceed in the backward direction,increasing the equilibrium concentration of H2O(g). 2)Decreasing the temperature will cause the reaction to proceed in the forward direction,increasing the equilibrium concentration of CO(g). 3)Increasing the amount of C(s)will cause the reaction to proceed in the forward direction,increasing the equilibrium concentration of CO(g).

A) 1 only B) 2 only C) 3 only D) 1 and 2 E) 1,2,and 3 A) 1 only B) 2 only C) 3 only D) 1 and 2 E) 1,2,and 3

A mixture of nitrogen and hydrogen was allowed to come to equilibrium at a given temperature. 3H2 + N2 2NH3 An analysis of the mixture at equilibrium revealed 2.1 mol N2,3.2 mol H2,and 1.8 mol NH3.How many moles of H2 were present at the beginning of the reaction?

A) 3.2 B) 4.8 C) 5.0 D) 5.9 E) 4.4 A) 3.2 B) 4.8 C) 5.0 D) 5.9 E) 4.4

Exam 16: Principles of Reactivity: Chemical Equilibria

Exactly 1.0 mol N₂O₄ is placed in an empty 1.0-L container and allowed to reach equilibrium described by the equation N₂O₄(g) 2NO₂(g).If at equilibrium the N₂O₄ is 28.0% dissociated,what is the value of the equilibrium constant,K_c,for the reaction under these conditions?

(Multiple Choice)

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Question 41

Assume that the following chemical reaction is at equilibrium. 2 ICl(g) $Assume that the following chemical reaction is at equilibrium. 2 ICl(g) I2(g)+ Cl2(g) \Delta H \circ = +26.9 kJ At 25 \circ C,Kp = 2.0 \times 105.If the temperature is increase to 45 \circ C,which statement applies?$ I₂(g)+ Cl₂(g) $$ $$ $\Delta$ H^$\circ$ = +26.9 kJ At 25 ^$\circ$C,K_p = 2.0 $\times$ 10⁵.If the temperature is increase to 45 ^$\circ$C,which statement applies?

(Multiple Choice)

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Question 42

What is the reaction quotient,Q,for the equilibrium SCN^-(aq) When 0.4257 L of M Ag⁺ is combined with 0.2376 L of M SCN^- in the presence of an excess of AgSCN(s)?

(Multiple Choice)

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Question 43

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 C?

(Multiple Choice)

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Question 44

In an experiment,0.42 mol H₂ and 0.42 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 45

At 25 ^$\circ$C,0.138 mg AgBr dissolves in 10.0 L of water.What is the equilibrium constant for the reaction below? $At 25 \circ C,0.138 mg AgBr dissolves in 10.0 L of water.What is the equilibrium constant for the reaction below?$

(Multiple Choice)

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Question 46

The reaction quotient,Q,for a system is .If the equilibrium constant for the system at some temperature is ,what will happen as the reaction mixture returns to equilibrium?

(Multiple Choice)

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Question 47

What is the K_c expression for the following equilibrium?

(Multiple Choice)

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Question 48

For the reaction NO(g)+ ½ O₂(g) NO₂(g)at 750°C,what is the relationship between K_c and K_p?

(Multiple Choice)

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Question 49

The symbol Q is called the ________.

(Short Answer)

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Question 50

Which of the following is always true for a reaction where K_c is $Which of the following is always true for a reaction where Kc is at 25 \circ C?$ at 25^$\circ$C?

(Multiple Choice)

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Question 51

For which of the following reactions are the numerical values of Kp and Kc the same? 1. 2SO₂(g) + O₂(g) 2SO3(g) 2. N2(g) + O2(g) 11ea8937_ab81_0f67_a16d_5b4ecfd630df_TB4499_11 2NO(g) 3. H₂(g)+ I₂(g) 11ea8937_ab81_0f67_a16d_5b4ecfd630df_TB4499_11 2HI(g)

(Multiple Choice)

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Question 52

For the equilibrium N₂O₄(g) $For the equilibrium N2O4(g) 2NO2(g),at 298 K,Kp = 0.15.For this reaction system,it is found that the partial pressure of N2O4 is 3.6 \times 10-2 atm at equilibrium.What is the partial pressure of NO2 at equilibrium?$ 2NO₂(g),at 298 K,K_p = 0.15.For this reaction system,it is found that the partial pressure of N₂O₄ is 3.6 $\times$ 10^-2 atm at equilibrium.What is the partial pressure of NO₂ at equilibrium?

(Multiple Choice)

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Question 53

Write the expression for K for the reaction of hydrofluoric acid with water.

(Multiple Choice)

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Question 54

Assume that the following $\underline{\text{ endothermic }}$ chemical reaction is at equilibrium. C(s)+ H₂O(g) $Assume that the following \underline{\text{ endothermic }} chemical reaction is at equilibrium. C(s)+ H2O(g) H2(g)+ CO(g) Which of the following statements is/are CORRECT? 1)Increasing the concentration of H2(g)will cause the reaction to proceed in the backward direction,increasing the equilibrium concentration of H2O(g). 2)Decreasing the temperature will cause the reaction to proceed in the forward direction,increasing the equilibrium concentration of CO(g). 3)Increasing the amount of C(s)will cause the reaction to proceed in the forward direction,increasing the equilibrium concentration of CO(g).$ H₂(g)+ CO(g) Which of the following statements is/are CORRECT? 1)Increasing the concentration of H₂(g)will cause the reaction to proceed in the backward direction,increasing the equilibrium concentration of H₂O(g). 2)Decreasing the temperature will cause the reaction to proceed in the forward direction,increasing the equilibrium concentration of CO(g). 3)Increasing the amount of C(s)will cause the reaction to proceed in the forward direction,increasing the equilibrium concentration of CO(g).

(Multiple Choice)

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Question 55

A mixture of nitrogen and hydrogen was allowed to come to equilibrium at a given temperature. 3H₂ + N₂ 2NH₃ An analysis of the mixture at equilibrium revealed 2.1 mol N₂,3.2 mol H₂,and 1.8 mol NH₃.How many moles of H₂ were present at the beginning of the reaction?

(Multiple Choice)

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Question 56

Which of the following statements is/are CORRECT? 1)For a chemical system,if the reaction quotient (Q)is greater than K,reactant must be converted to products to reach equilibrium. 2)For a chemical system at equilibrium,the forward and reverse rates of reaction are equal. 3)For a chemical system at equilibrium,the concentrations of products divided by the concentrations of reactants equals one.

(Multiple Choice)

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Question 57

Nitrosyl bromide decomposes according to the chemical equation below.2 NOBr(g) 2 NO(g)+ Br₂(g) When 0.260 atm of NOBr is sealed in a flask and allowed to reach equilibrium,22% of the NOBr decomposes.What is the equilibrium constant,K_p,for the reaction?

(Multiple Choice)

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Question 58

Which of the following statements is/are CORRECT? 1)Product concentrations appear in the numerator of an equilibrium constant expression. 2)A reaction favors the formation of products if K >> 1. 3)Stoichiometric coefficients are used as exponents in an equilibrium constant expression.

(Multiple Choice)

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Question 59

Consider the reaction A(aq) $Consider the reaction A(aq) 2 B(aq)where Kc = 4.1 at 25 \circ C.If 0.50 M A(aq)and 1.5 M B(aq)are initially present in a 1.0 L flask at 25 \circ C,what change in concentrations (if any)will occur in time?$ 2 B(aq)where K_c = 4.1 at 25 ^$\circ$C.If 0.50 M A(aq)and 1.5 M B(aq)are initially present in a 1.0 L flask at 25 ^$\circ$C,what change in concentrations (if any)will occur in time?

(Multiple Choice)

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Question 60

Showing 41 - 60 of 82

Exactly 1.0 mol N₂O₄ is placed in an empty 1.0-L container and allowed to reach equilibrium described by the equation N₂O₄(g) 2NO₂(g).If at equilibrium the N₂O₄ is 28.0% dissociated,what is the value of the equilibrium constant,K_c,for the reaction under these conditions?

What is the reaction quotient,Q,for the equilibrium SCN^-(aq) When 0.4257 L of M Ag⁺ is combined with 0.2376 L of M SCN^- in the presence of an excess of AgSCN(s)?

In an experiment,0.42 mol H₂ and 0.42 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)

At 25 ^$\circ$C,0.138 mg AgBr dissolves in 10.0 L of water.What is the equilibrium constant for the reaction below? $At 25 <sup> \circ </sup>C,0.138 mg AgBr dissolves in 10.0 L of water.What is the equilibrium constant for the reaction below?$

The reaction quotient,Q,for a system is .If the equilibrium constant for the system at some temperature is ,what will happen as the reaction mixture returns to equilibrium?

What is the K_c expression for the following equilibrium?

For the reaction NO(g)+ ½ O₂(g) NO₂(g)at 750°C,what is the relationship between K_c and K_p?

The symbol Q is called the ________.

Which of the following is always true for a reaction where K_c is $Which of the following is always true for a reaction where K<sub>c</sub> is at 25<sup> \circ </sup>C?$ at 25^$\circ$C?

For which of the following reactions are the numerical values of Kp and Kc the same? 1. 2SO₂(g) + O₂(g) 2SO3(g) 2. N2(g) + O2(g) 11ea8937_ab81_0f67_a16d_5b4ecfd630df_TB4499_11 2NO(g) 3. H₂(g)+ I₂(g) 11ea8937_ab81_0f67_a16d_5b4ecfd630df_TB4499_11 2HI(g)

Write the expression for K for the reaction of hydrofluoric acid with water.

A mixture of nitrogen and hydrogen was allowed to come to equilibrium at a given temperature. 3H₂ + N₂ 2NH₃ An analysis of the mixture at equilibrium revealed 2.1 mol N₂,3.2 mol H₂,and 1.8 mol NH₃.How many moles of H₂ were present at the beginning of the reaction?

Nitrosyl bromide decomposes according to the chemical equation below.2 NOBr(g) 2 NO(g)+ Br₂(g) When 0.260 atm of NOBr is sealed in a flask and allowed to reach equilibrium,22% of the NOBr decomposes.What is the equilibrium constant,K_p,for the reaction?

Which of the following statements is/are CORRECT? 1)Product concentrations appear in the numerator of an equilibrium constant expression. 2)A reaction favors the formation of products if K >> 1. 3)Stoichiometric coefficients are used as exponents in an equilibrium constant expression.

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Exam 16: Principles of Reactivity: Chemical Equilibria

Exactly 1.0 mol N2O4 is placed in an empty 1.0-L container and allowed to reach equilibrium described by the equation N2O4(g) 2NO2(g).If at equilibrium the N2O4 is 28.0% dissociated,what is the value of the equilibrium constant,Kc,for the reaction under these conditions?

Assume that the following chemical reaction is at equilibrium. 2 ICl(g) I2(g)+ Cl2(g) ~~~~~~~~ ~~~~~~~~ Δ\DeltaΔ H ∘\circ∘ = +26.9 kJ At 25 ∘\circ∘ C,Kp = 2.0 ×\times× 105.If the temperature is increase to 45 ∘\circ∘ C,which statement applies?

What is the reaction quotient,Q,for the equilibrium SCN-(aq) When 0.4257 L of M Ag+ is combined with 0.2376 L of M SCN- in the presence of an excess of AgSCN(s)?

In an experiment,0.42 mol H2 and 0.42 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)

At 25 ∘\circ∘ C,0.138 mg AgBr dissolves in 10.0 L of water.What is the equilibrium constant for the reaction below?

The reaction quotient,Q,for a system is .If the equilibrium constant for the system at some temperature is ,what will happen as the reaction mixture returns to equilibrium?

What is the Kc expression for the following equilibrium?

For the reaction NO(g)+ ½ O2(g) NO2(g)at 750°C,what is the relationship between Kc and Kp?

The symbol Q is called the ________.

Which of the following is always true for a reaction where Kc is at 25 ∘\circ∘ C?

For which of the following reactions are the numerical values of Kp and Kc the same? 1. 2SO2(g) + O2(g) 2SO3(g) 2. N2(g) + O2(g) 11ea8937_ab81_0f67_a16d_5b4ecfd630df_TB4499_11 2NO(g) 3. H2(g)+ I2(g) 11ea8937_ab81_0f67_a16d_5b4ecfd630df_TB4499_11 2HI(g)

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 3.6 ×\times× 10-2 atm at equilibrium.What is the partial pressure of NO2 at equilibrium?

Write the expression for K for the reaction of hydrofluoric acid with water.

A mixture of nitrogen and hydrogen was allowed to come to equilibrium at a given temperature. 3H2 + N2 2NH3 An analysis of the mixture at equilibrium revealed 2.1 mol N2,3.2 mol H2,and 1.8 mol NH3.How many moles of H2 were present at the beginning of the reaction?

Nitrosyl bromide decomposes according to the chemical equation below.2 NOBr(g) 2 NO(g)+ Br2(g) When 0.260 atm of NOBr is sealed in a flask and allowed to reach equilibrium,22% of the NOBr decomposes.What is the equilibrium constant,Kp,for the reaction?

Which of the following statements is/are CORRECT? 1)Product concentrations appear in the numerator of an equilibrium constant expression. 2)A reaction favors the formation of products if K >> 1. 3)Stoichiometric coefficients are used as exponents in an equilibrium constant expression.

Consider the reaction A(aq) 2 B(aq)where Kc = 4.1 at 25 ∘\circ∘ C.If 0.50 M A(aq)and 1.5 M B(aq)are initially present in a 1.0 L flask at 25 ∘\circ∘ C,what change in concentrations (if any)will occur in time?

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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Exactly 1.0 mol N₂O₄ is placed in an empty 1.0-L container and allowed to reach equilibrium described by the equation N₂O₄(g) 2NO₂(g).If at equilibrium the N₂O₄ is 28.0% dissociated,what is the value of the equilibrium constant,K_c,for the reaction under these conditions?

What is the reaction quotient,Q,for the equilibrium SCN^-(aq) When 0.4257 L of M Ag⁺ is combined with 0.2376 L of M SCN^- in the presence of an excess of AgSCN(s)?

In an experiment,0.42 mol H₂ and 0.42 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)

At 25 ^$\circ$C,0.138 mg AgBr dissolves in 10.0 L of water.What is the equilibrium constant for the reaction below? $At 25 <sup> \circ </sup>C,0.138 mg AgBr dissolves in 10.0 L of water.What is the equilibrium constant for the reaction below?$

What is the K_c expression for the following equilibrium?

For the reaction NO(g)+ ½ O₂(g) NO₂(g)at 750°C,what is the relationship between K_c and K_p?

Which of the following is always true for a reaction where K_c is $Which of the following is always true for a reaction where K<sub>c</sub> is at 25<sup> \circ </sup>C?$ at 25^$\circ$C?

For which of the following reactions are the numerical values of Kp and Kc the same? 1. 2SO₂(g) + O₂(g) 2SO3(g) 2. N2(g) + O2(g) 11ea8937_ab81_0f67_a16d_5b4ecfd630df_TB4499_11 2NO(g) 3. H₂(g)+ I₂(g) 11ea8937_ab81_0f67_a16d_5b4ecfd630df_TB4499_11 2HI(g)

A mixture of nitrogen and hydrogen was allowed to come to equilibrium at a given temperature. 3H₂ + N₂ 2NH₃ An analysis of the mixture at equilibrium revealed 2.1 mol N₂,3.2 mol H₂,and 1.8 mol NH₃.How many moles of H₂ were present at the beginning of the reaction?

Nitrosyl bromide decomposes according to the chemical equation below.2 NOBr(g) 2 NO(g)+ Br₂(g) When 0.260 atm of NOBr is sealed in a flask and allowed to reach equilibrium,22% of the NOBr decomposes.What is the equilibrium constant,K_p,for the reaction?