Two moles of NH3 are initially present for the reaction: 2 NH3(g) ⇌ N2(g) + 3 H2(g) At equilibrium there is 1.00 mol NH3. How many moles of H2 are present at equilibrium?

A) 3.00 B) 1.00 C) 1.50 D) 0.67 E) 0.75 A) 3.00 B) 1.00 C) 1.50 D) 0.67 E) 0.75

For CO2(g) + H2(g) ⇌ CO(g) + H2O(g), Kc = [CO][H2]/[CO2][H2], if there are 1.43 mols each of CO and H2, 0.572 mol H2 and 4.572 mols CO2, in a 4.0 L container at equilibrium, what is Kc?

A) 0.547 B) 0.782 C) 1.28 D) 0.137 E) 2.34 A) 0.547 B) 0.782 C) 1.28 D) 0.137 E) 2.34

Consider the following equilibrium reaction: PCl3(g) + Cl2(g) ⇌ PCl5(g) Kc = 96.2 The equilibrium constant for the decomposition of PCl5(g) to PCl3(g) and Cl2(g) is ________.

A) -Kc B) C) D) E) A) -Kc B) C) D) E)

Choose the correct statement about the equilibrium: N2(g) + 3 H2(g) ⇌ 2 NH3(g), Kp = 1 × 10-4 atm-2

A) The rate constant for the forward reaction is greater than that of the reverse reaction. B) Since the reaction has a high activation energy, a catalyst is not needed. C) The equilibrium constant is given by Kp = [N2][H2]3/[NH3]2. D) Conducting the reaction under high pressures will increase the yield of ammonia. E) The Kp is independent of temperature. A) The rate constant for the forward reaction is greater than that of the reverse reaction. B) Since the reaction has a high activation energy, a catalyst is not needed. C) The equilibrium constant is given by Kp = [N2][H2]3/[NH3]2. D) Conducting the reaction under high pressures will increase the yield of ammonia. E) The Kp is independent of temperature.

For the reaction: H2(g) + I2(g) ⇌ 2 HI(g), Kc = 92.0 When equilibrium concentrations of HI and I2 are [HI] = 0.115 M and [I2] = 0.250 M, the equilibrium concentration of [H2] is:

A) 5.00 × 10-3 M B) 5.75 × 10-4 M C) 1.74 × 103 M D) 0.135 M E) 9.56 M A) 5.00 × 10-3 M B) 5.75 × 10-4 M C) 1.74 × 103 M D) 0.135 M E) 9.56 M

Given the following reactions, 2PCl3(g) ⇌ 2P(g) + 3Cl2(g) Kc = 0.0667 PCl3(g) + Cl2(g) ⇌ PCl5(g) Kc = 4.0 Calculate Kc for the reaction below. 2P(g) + 5Cl2(g) ⇌ 2PCl5(g)

A) 240 B) 1.1 C) 60 D) 23 A) 240 B) 1.1 C) 60 D) 23

For the reaction: CH4(g) + 2 H2O(g) ⇌ CO2(g) + 4 H2(g) ΔH° = +190 kJ when catalyst is added:

A) the reaction reacts to the right B) the reaction reacts to the left C) the ΔH° increases D) the temperature increases E) there is no change, catalyst changes reaction rate only A) the reaction reacts to the right B) the reaction reacts to the left C) the ΔH° increases D) the temperature increases E) there is no change, catalyst changes reaction rate only

For the following reaction O2(g) ⇌ 2O(g) What conditions favor production of oxygen atoms?

A) high temperature and low pressure B) high temperature and high pressure C) low temperature and low pressure D) low temperature and high pressure A) high temperature and low pressure B) high temperature and high pressure C) low temperature and low pressure D) low temperature and high pressure

At 35°C, Kp = 0.315 for the reaction N2O4(g) ⇌ 2 NO2(g), if the initial pressure of NO2(g) in a container is 3.00 atm, what is the equilibrium pressure of N2O4(g)?

A) 1.88 atm B) 0.315 atm C) 0.471 atm D) 1.19 atm E) 0.685 atm A) 1.88 atm B) 0.315 atm C) 0.471 atm D) 1.19 atm E) 0.685 atm

Exam 15: Principles of Chemical Equilibrium

Two moles of NH₃ are initially present for the reaction: 2 NH₃(g) ⇌ N₂(g) + 3 H₂(g) At equilibrium there is 1.00 mol NH₃. How many moles of H₂ are present at equilibrium?

(Multiple Choice)

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Question 61

Choose the correct statement about a container in which the chemical equilibrium is established: 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) + heat

(Multiple Choice)

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Question 62

For CO₂(g) + H₂(g) ⇌ CO(g) + H₂O(g), Kc = [CO][H₂]/[CO₂][H₂], if there are 1.43 mols each of CO and H₂, 0.572 mol H₂ and 4.572 mols CO₂, in a 4.0 L container at equilibrium, what is Kc?

(Multiple Choice)

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Question 63

Consider the equilibrium system: N₂O₄(g) ⇌ 2 NO₂(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 58.03 kJ/mol. Assuming that the total pressure inside the container is 1.00 atm at equilibrium and that initially only N₂O₄ was present inside the container, compute PNO₂ at equilibrium.

(Multiple Choice)

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Question 64

Consider the following equilibrium reaction: PCl₃(g) + Cl₂(g) ⇌ PCl₅(g) Kc = 96.2 The equilibrium constant for the decomposition of PCl₅(g) to PCl₃(g) and Cl₂(g) is ________.

(Multiple Choice)

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Question 65

Which of the following keep the equilibrium position unchanged?

(Multiple Choice)

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Question 66

Choose the correct statement about the equilibrium: N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g), Kp = 1 × 10^-4atm-2

(Multiple Choice)

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Question 67

Changes in temperature cause change in the equilibrium position.

(True/False)

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Question 68

For the reaction: H₂(g) + I₂(g) ⇌ 2 HI(g), Kc = 92.0 When equilibrium concentrations of HI and I₂ are [HI] = 0.115 M and [I₂] = 0.250 M, the equilibrium concentration of [H₂] is:

(Multiple Choice)

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Question 69

Consider the following gas phase reaction at 25°C. N₂(g) + C₂H₂(g) ⇌ 2 HCN(g) 600 mol N₂(g) and 1.750 mol C₂H₂(g) are placed in a 1.000 L vessel and the mixture is allowed to react. At equilibrium, there are 1.587 mol N₂(g) in the mixture. What is Kc for this reaction at 25 °C?

(Multiple Choice)

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Question 70

Given the following reactions, 2PCl₃(g) ⇌ 2P(g) + 3Cl₂(g) Kc = 0.0667 PCl₃(g) + Cl₂(g) ⇌ PCl₅(g) Kc = 4.0 Calculate Kc for the reaction below. 2P(g) + 5Cl₂(g) ⇌ 2PCl₅(g)

(Multiple Choice)

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Question 71

Write the equilibrium constant expression for the reaction: 3 Sn(s) + 4 HNO₃(aq) + H₂O(l) ⇌ 3 H₂SnO₃(s) + 4 NO(g)

(Multiple Choice)

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Question 72

For the reaction: CH₄(g) + 2 H₂O(g) ⇌ CO₂(g) + 4 H₂(g) ΔH° = +190 kJ when catalyst is added:

(Multiple Choice)

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Question 73

For the following reaction O₂(g) ⇌ 2O(g) What conditions favor production of oxygen atoms?

(Multiple Choice)

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Question 74

Write the equilibrium expression Kc for the reaction: sodium sulfite(aq) + chloric acid (aq) ⇌ sodium chlorite(aq) + sulfur dioxide(g) + water(l).

(Multiple Choice)

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Question 75

Consider the equilibrium system: N₂O₄(g) ⇌ 2NO₂(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 58.03 kJ/mol. Assuming that the total pressure inside the container is 10 atm at equilibrium and that initially only N₂O₄ was present inside the container, compute PNO₂ at equilibrium.

(Multiple Choice)

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Question 76

At 35°C, Kp = 0.315 for the reaction N₂O₄(g) ⇌ 2 NO₂(g), if the initial pressure of NO₂(g) in a container is 3.00 atm, what is the equilibrium pressure of N₂O₄(g)?

(Multiple Choice)

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Question 77

A mixture containing 0.0392 M A(g) and 0.0452 M B(g) is allowed to come to equilibrium at 300 K. The reaction: 3 A(g) + 2 B(g) ⇌ C(g) + D(g) occurs. At equilibrium, [C] = 0.00128 M. What is the value of Kc?

(Multiple Choice)

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Question 78

Write the equilibrium constant expression for the following reaction: 2 KI(aq) + H₂O₂(aq) ⇌ 2 KOH(aq) + I₂(aq)

(Multiple Choice)

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Question 79

For the reaction: 2 Cl₂(g) + 2 H₂O(g) ⇌ 4 HCl(g) + O₂(g), Kp = 6.4 × 10^-6 at 500 K. If a fixed volume is filled with initial concentrations of these gases at 227°C such that [Cl₂] = 0.5 M, [H₂O] = 0.40 M, [HCl] = 0.5 M, and [O₂] = 0.015 M, in which direction will the reaction proceed?

(Multiple Choice)

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Question 80

Showing 61 - 80 of 99

Exam 15: Principles of Chemical Equilibrium

Two moles of NH3 are initially present for the reaction: 2 NH3(g) ⇌ N2(g) + 3 H2(g) At equilibrium there is 1.00 mol NH3. How many moles of H2 are present at equilibrium?

Choose the correct statement about a container in which the chemical equilibrium is established: 2 SO2(g) + O2(g) ⇌ 2 SO3(g) + heat

For CO2(g) + H2(g) ⇌ CO(g) + H2O(g), Kc = [CO][H2]/[CO2][H2], if there are 1.43 mols each of CO and H2, 0.572 mol H2 and 4.572 mols CO2, in a 4.0 L container at equilibrium, what is Kc?

Consider the equilibrium system: N2O4(g) ⇌ 2 NO2(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 58.03 kJ/mol. Assuming that the total pressure inside the container is 1.00 atm at equilibrium and that initially only N2O4 was present inside the container, compute PNO2 at equilibrium.

Consider the following equilibrium reaction: PCl3(g) + Cl2(g) ⇌ PCl5(g) Kc = 96.2 The equilibrium constant for the decomposition of PCl5(g) to PCl3(g) and Cl2(g) is ________.

Which of the following keep the equilibrium position unchanged?

Choose the correct statement about the equilibrium: N2(g) + 3 H2(g) ⇌ 2 NH3(g), Kp = 1 × 10-4 atm-2

Changes in temperature cause change in the equilibrium position.

For the reaction: H2(g) + I2(g) ⇌ 2 HI(g), Kc = 92.0 When equilibrium concentrations of HI and I2 are [HI] = 0.115 M and [I2] = 0.250 M, the equilibrium concentration of [H2] is:

Consider the following gas phase reaction at 25°C. N2(g) + C2H2(g) ⇌ 2 HCN(g) 600 mol N2(g) and 1.750 mol C2H2(g) are placed in a 1.000 L vessel and the mixture is allowed to react. At equilibrium, there are 1.587 mol N2(g) in the mixture. What is Kc for this reaction at 25 °C?

Given the following reactions, 2PCl3(g) ⇌ 2P(g) + 3Cl2(g) Kc = 0.0667 PCl3(g) + Cl2(g) ⇌ PCl5(g) Kc = 4.0 Calculate Kc for the reaction below. 2P(g) + 5Cl2(g) ⇌ 2PCl5(g)

Write the equilibrium constant expression for the reaction: 3 Sn(s) + 4 HNO3(aq) + H2O(l) ⇌ 3 H2SnO3(s) + 4 NO(g)

For the reaction: CH4(g) + 2 H2O(g) ⇌ CO2(g) + 4 H2(g) ΔH° = +190 kJ when catalyst is added:

For the following reaction O2(g) ⇌ 2O(g) What conditions favor production of oxygen atoms?

Write the equilibrium expression Kc for the reaction: sodium sulfite(aq) + chloric acid (aq) ⇌ sodium chlorite(aq) + sulfur dioxide(g) + water(l).

Consider the equilibrium system: N2O4(g) ⇌ 2NO2(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 58.03 kJ/mol. Assuming that the total pressure inside the container is 10 atm at equilibrium and that initially only N2O4 was present inside the container, compute PNO2 at equilibrium.

At 35°C, Kp = 0.315 for the reaction N2O4(g) ⇌ 2 NO2(g), if the initial pressure of NO2(g) in a container is 3.00 atm, what is the equilibrium pressure of N2O4(g)?

A mixture containing 0.0392 M A(g) and 0.0452 M B(g) is allowed to come to equilibrium at 300 K. The reaction: 3 A(g) + 2 B(g) ⇌ C(g) + D(g) occurs. At equilibrium, [C] = 0.00128 M. What is the value of Kc?

Write the equilibrium constant expression for the following reaction: 2 KI(aq) + H2O2(aq) ⇌ 2 KOH(aq) + I2(aq)

For the reaction: 2 Cl2(g) + 2 H2O(g) ⇌ 4 HCl(g) + O2(g), Kp = 6.4 × 10-6 at 500 K. If a fixed volume is filled with initial concentrations of these gases at 227°C such that [Cl2] = 0.5 M, [H2O] = 0.40 M, [HCl] = 0.5 M, and [O2] = 0.015 M, in which direction will the reaction proceed?

Matter - Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Additional Aspects

Intermolecular Forces: Liquids and Solids

Solutions and Their Physical Properties

Chemical Kinetics

Acids and Bases

Additional Aspects of Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Spontaneous Change: Entropy and Free Energy

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Main Group Elements I: Groups 1, 2, 13, and 14

Main Group Elements II: Groups 18, 17, 16, 15, and Hydrogen

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Two moles of NH₃ are initially present for the reaction: 2 NH₃(g) ⇌ N₂(g) + 3 H₂(g) At equilibrium there is 1.00 mol NH₃. How many moles of H₂ are present at equilibrium?

Choose the correct statement about a container in which the chemical equilibrium is established: 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g) + heat

For CO₂(g) + H₂(g) ⇌ CO(g) + H₂O(g), Kc = [CO][H₂]/[CO₂][H₂], if there are 1.43 mols each of CO and H₂, 0.572 mol H₂ and 4.572 mols CO₂, in a 4.0 L container at equilibrium, what is Kc?

Consider the equilibrium system: N₂O₄(g) ⇌ 2 NO₂(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 58.03 kJ/mol. Assuming that the total pressure inside the container is 1.00 atm at equilibrium and that initially only N₂O₄ was present inside the container, compute PNO₂ at equilibrium.

Consider the following equilibrium reaction: PCl₃(g) + Cl₂(g) ⇌ PCl₅(g) Kc = 96.2 The equilibrium constant for the decomposition of PCl₅(g) to PCl₃(g) and Cl₂(g) is ________.

Choose the correct statement about the equilibrium: N₂(g) + 3 H₂(g) ⇌ 2 NH₃(g), Kp = 1 × 10^-4atm-2

For the reaction: H₂(g) + I₂(g) ⇌ 2 HI(g), Kc = 92.0 When equilibrium concentrations of HI and I₂ are [HI] = 0.115 M and [I₂] = 0.250 M, the equilibrium concentration of [H₂] is:

Consider the following gas phase reaction at 25°C. N₂(g) + C₂H₂(g) ⇌ 2 HCN(g) 600 mol N₂(g) and 1.750 mol C₂H₂(g) are placed in a 1.000 L vessel and the mixture is allowed to react. At equilibrium, there are 1.587 mol N₂(g) in the mixture. What is Kc for this reaction at 25 °C?

Given the following reactions, 2PCl₃(g) ⇌ 2P(g) + 3Cl₂(g) Kc = 0.0667 PCl₃(g) + Cl₂(g) ⇌ PCl₅(g) Kc = 4.0 Calculate Kc for the reaction below. 2P(g) + 5Cl₂(g) ⇌ 2PCl₅(g)

Write the equilibrium constant expression for the reaction: 3 Sn(s) + 4 HNO₃(aq) + H₂O(l) ⇌ 3 H₂SnO₃(s) + 4 NO(g)

For the reaction: CH₄(g) + 2 H₂O(g) ⇌ CO₂(g) + 4 H₂(g) ΔH° = +190 kJ when catalyst is added:

For the following reaction O₂(g) ⇌ 2O(g) What conditions favor production of oxygen atoms?

Consider the equilibrium system: N₂O₄(g) ⇌ 2NO₂(g) for which Kp = 0.1134 at 25°C and ΔH°rxn = 58.03 kJ/mol. Assuming that the total pressure inside the container is 10 atm at equilibrium and that initially only N₂O₄ was present inside the container, compute PNO₂ at equilibrium.

At 35°C, Kp = 0.315 for the reaction N₂O₄(g) ⇌ 2 NO₂(g), if the initial pressure of NO₂(g) in a container is 3.00 atm, what is the equilibrium pressure of N₂O₄(g)?

Write the equilibrium constant expression for the following reaction: 2 KI(aq) + H₂O₂(aq) ⇌ 2 KOH(aq) + I₂(aq)