The addition of I2(g) to a fixed volume container with I2(g), H2(g), and HI(g) at equilibrium at a given temperature would cause H2(g) + I2(g) 2 HI(g)

A) the concentrations of both H2 and HI to decrease. B) the concentrations of both H2 and HI to increase. C) the concentration of H2 to increase and HI to decrease. D) the concentration of H2 to decrease and HI to increase. E) Not enough information is given to determine how the concentrations will change. A) the concentrations of both H2 and HI to decrease. B) the concentrations of both H2 and HI to increase. C) the concentration of H2 to increase and HI to decrease. D) the concentration of H2 to decrease and HI to increase. E) Not enough information is given to determine how the concentrations will change.

Assume that the reaction quotient, Qc, for the following reaction at 25°C is 1.0 x 10-8 2 NO2(g) 2 NO(g) + O2(g) &emsp; &emsp; Kc = 7.4 x 10-16 (at 25°C) From this we can conclude:

A) The reaction is at equilibrium. B) Equilibrium could be reached by adding enough NO or O2 to the system. C) The reaction must proceed from left to right to reach equilibrium. D) The reaction must proceed from right to left to reach equilibrium. E) The reaction can never reach equilibrium. A) The reaction is at equilibrium. B) Equilibrium could be reached by adding enough NO or O2 to the system. C) The reaction must proceed from left to right to reach equilibrium. D) The reaction must proceed from right to left to reach equilibrium. E) The reaction can never reach equilibrium.

What is the Ksp of PbBr2 if the concentration of PbBr2(aq) in a saturated solution is 1.3 x 10-2 moles/L?

A) 8.8 x 10 - 6 B) 1.3 x 10 - 2 C) 3.9 x 10 - 2 D) 2.2 x 10 - 2 E) none of the above A) 8.8 x 10 - 6 B) 1.3 x 10 - 2 C) 3.9 x 10 - 2 D) 2.2 x 10 - 2 E) none of the above

Ag2SO4(s) is in equilibrium with silver and sulfate ions in solution: Ag2SO4(s) 2Ag+(aq) + SO42-(aq) Which of the following will not increase the amount of solid Ag2SO4(s) present?

A) boiling off some of the water B) adding Na2SO4 to the solution C) adding AgNO3 to the solution D) adding NaCl to the solution E) All of the above will increase the amount of Ag2SO4 present. A) boiling off some of the water B) adding Na2SO4 to the solution C) adding AgNO3 to the solution D) adding NaCl to the solution E) All of the above will increase the amount of Ag2SO4 present.

Exam 10: An Introduction to Kinetics and Equilibrium

The addition of I₂(g) to a fixed volume container with I₂(g), H₂(g), and HI(g) at equilibrium at a given temperature would cause H₂(g) + I₂(g) 2 HI(g)

(Multiple Choice)

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Question 41

A solution is prepared in which the Ag⁺ ion concentration is 2.5 x 10^-3 M and the Cl^- ion concentration is 3.2 x 10^-4 M. Which of the following statements is true given that the K_sp for AgCl is 1.8 x 10^-10?

(Multiple Choice)

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Question 42

Which of the following equations correctly describes the relationship between the concentrations of Pb²⁺ and Br^- ions in a saturated solution of PbBr₂(s)?

(Multiple Choice)

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Question 43

Which of the following statements correctly describes the following reaction? 2 NH₃(g) $Which of the following statements correctly describes the following reaction? 2 NH3(g) N2(g) + 3 H2(g) \Delta H = 92.2 kJ$ N₂(g) + 3 H₂(g) $\Delta$ H = 92.2 kJ

(Multiple Choice)

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Question 44

A solution is 0.10 M in Ca(NO₃)₂. What would the concentration of NaOH need to be for a precipitate of Ca(OH)₂ to form? K_sp Ca(OH)₂ = 5.5 x 10^-6.

(Multiple Choice)

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Question 45

What would be the effect of decreasing the pressure on the following reaction after it reaches equilibrium? 2 NO₂(g) 2 NO(g) + O₂(g)

(Multiple Choice)

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Question 46

Assume that the reaction quotient, Q_c, for the following reaction at 25°C is 1.0 x 10^-8 2 NO₂(g) 2 NO(g) + O₂(g) K_c = 7.4 x 10^-16 (at 25°C) From this we can conclude:

(Multiple Choice)

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Question 47

What is the K_sp of PbBr₂ if the concentration of PbBr₂(aq) in a saturated solution is 1.3 x 10^-2 moles/L?

(Multiple Choice)

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Question 48

What would happen if O₂ were removed from the following system at equilibrium at 25°C? 2 NO₂(g) 2 NO(g) + O₂(g) K_c = 7.4 x 10^-1 at 25^oC

(Multiple Choice)

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Question 49

Of the compounds in the table below, _ is the $\underline{\text{ least }}$ soluble. $Of the compounds in the table below, _ is the \underline{\text{ least }} soluble.$

(Multiple Choice)

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Question 50

Which one of the following graphs best represents the relationship between the concentration of reactants and products with respect to time for the following chemical reaction? 2 NO₂(g) 2 NO(g) + O₂(g)

(Multiple Choice)

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Question 51

Approximately how many grams of Ag₂CO₃ will dissolve in 1.0 liter of a solution that is 0.10 M in Na₂CO₃? The K_sp of Ag₂CO₃ is 6.2 x 10^-12.

(Multiple Choice)

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Question 52

Ag₂SO₄(s) is in equilibrium with silver and sulfate ions in solution: Ag₂SO₄(s) 2Ag⁺(aq) + SO₄^2-(aq) Which of the following will not increase the amount of solid Ag₂SO₄(s) present?

(Multiple Choice)

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Question 53

If a solution has a Mg²⁺ ion concentration of 5.0 x 10^-3 M and an OH^- concentration of 0.010 M, will a precipitate form? K_sp Mg(OH)₂ = 1.7 x 10^-6.

(Essay)

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Question 54

-Which of the following will be true concerning the K_c of the reaction described by the graph above?

(Multiple Choice)

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Question 55

Which of the following equilibria would not be affected by changes in pressure?

(Multiple Choice)

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Question 56

The following reaction was carried out: Ni(CO)₄ + PPh₃(g) $\rightarrow$ PPh₃Ni(CO)₃ + CO Over 200 seconds, the concentration of Ni(CO)4 dropped from 10 M to 2.5 M. What is the average rate of the reaction in M/s over this time period?

(Multiple Choice)

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Question 57

Which of the following equations describes the relationship between the solubility product for AgCl and the solubility of this compound?

(Multiple Choice)

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Question 58

What is the solubility in moles per liter of AgBr in water given that the K_sp is 5.0 x 10^-13?

(Multiple Choice)

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Question 59

Describe the relationship between the rate constants k_f and k_r for the following one step reaction at equilibrium.

(Multiple Choice)

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Question 60

Showing 41 - 60 of 94

The addition of I₂(g) to a fixed volume container with I₂(g), H₂(g), and HI(g) at equilibrium at a given temperature would cause H₂(g) + I₂(g) 2 HI(g)

A solution is prepared in which the Ag⁺ ion concentration is 2.5 x 10^-3 M and the Cl^- ion concentration is 3.2 x 10^-4 M. Which of the following statements is true given that the K_sp for AgCl is 1.8 x 10^-10?

Which of the following equations correctly describes the relationship between the concentrations of Pb²⁺ and Br^- ions in a saturated solution of PbBr₂(s)?

Which of the following statements correctly describes the following reaction? 2 NH₃(g) $Which of the following statements correctly describes the following reaction? 2 NH<sub>3</sub>(g) N<sub>2</sub>(g) + 3 H<sub>2</sub>(g) \Delta H = 92.2 kJ$ N₂(g) + 3 H₂(g) $\Delta$ H = 92.2 kJ

A solution is 0.10 M in Ca(NO₃)₂. What would the concentration of NaOH need to be for a precipitate of Ca(OH)₂ to form? K_sp Ca(OH)₂ = 5.5 x 10^-6.

What would be the effect of decreasing the pressure on the following reaction after it reaches equilibrium? 2 NO₂(g) 2 NO(g) + O₂(g)

Assume that the reaction quotient, Q_c, for the following reaction at 25°C is 1.0 x 10^-8 2 NO₂(g) 2 NO(g) + O₂(g) K_c = 7.4 x 10^-16 (at 25°C) From this we can conclude:

What is the K_sp of PbBr₂ if the concentration of PbBr₂(aq) in a saturated solution is 1.3 x 10^-2 moles/L?

What would happen if O₂ were removed from the following system at equilibrium at 25°C? 2 NO₂(g) 2 NO(g) + O₂(g) K_c = 7.4 x 10^-1 at 25^oC

Of the compounds in the table below, _ is the $\underline{\text{ least }}$ soluble. $Of the compounds in the table below, _ is the \underline{\text{ least }} soluble.$

Which one of the following graphs best represents the relationship between the concentration of reactants and products with respect to time for the following chemical reaction? 2 NO₂(g) 2 NO(g) + O₂(g)

Approximately how many grams of Ag₂CO₃ will dissolve in 1.0 liter of a solution that is 0.10 M in Na₂CO₃? The K_sp of Ag₂CO₃ is 6.2 x 10^-12.

Ag₂SO₄(s) is in equilibrium with silver and sulfate ions in solution: Ag₂SO₄(s) 2Ag⁺(aq) + SO₄^2-(aq) Which of the following will not increase the amount of solid Ag₂SO₄(s) present?

If a solution has a Mg²⁺ ion concentration of 5.0 x 10^-3 M and an OH^- concentration of 0.010 M, will a precipitate form? K_sp Mg(OH)₂ = 1.7 x 10^-6.

-Which of the following will be true concerning the K_c of the reaction described by the graph above?

Which of the following equilibria would not be affected by changes in pressure?

The following reaction was carried out: Ni(CO)₄ + PPh₃(g) $\rightarrow$ PPh₃Ni(CO)₃ + CO Over 200 seconds, the concentration of Ni(CO)4 dropped from 10 M to 2.5 M. What is the average rate of the reaction in M/s over this time period?

Which of the following equations describes the relationship between the solubility product for AgCl and the solubility of this compound?

What is the solubility in moles per liter of AgBr in water given that the K_sp is 5.0 x 10^-13?

Describe the relationship between the rate constants k_f and k_r for the following one step reaction at equilibrium.

Elements Compounds

The Mole

Structure of the Atom

The Covalent Bond

Ionic and Metallic Bonds

Gases

Making and Breaking of Bonds

Liquids and Solutions

Solids

Acids and Bases

Oxidation-Reduction Reactions

Chemical Thermodynamics

Kinetics

Nuclear Chemistry

Organic Chemistry

Filters

Exam 10: An Introduction to Kinetics and Equilibrium

The addition of I2(g) to a fixed volume container with I2(g), H2(g), and HI(g) at equilibrium at a given temperature would cause H2(g) + I2(g) 2 HI(g)

A solution is prepared in which the Ag+ ion concentration is 2.5 x 10-3 M and the Cl- ion concentration is 3.2 x 10-4 M. Which of the following statements is true given that the Ksp for AgCl is 1.8 x 10-10?

Which of the following equations correctly describes the relationship between the concentrations of Pb2+ and Br- ions in a saturated solution of PbBr2(s)?

Which of the following statements correctly describes the following reaction? 2 NH3(g) N2(g) + 3 H2(g) Δ\DeltaΔ H = 92.2 kJ

A solution is 0.10 M in Ca(NO3)2. What would the concentration of NaOH need to be for a precipitate of Ca(OH)2 to form? Ksp Ca(OH)2 = 5.5 x 10-6.

What would be the effect of decreasing the pressure on the following reaction after it reaches equilibrium? 2 NO2(g) 2 NO(g) + O2(g)

Assume that the reaction quotient, Qc, for the following reaction at 25°C is 1.0 x 10-8 2 NO2(g) 2 NO(g) + O2(g) Kc = 7.4 x 10-16 (at 25°C) From this we can conclude:

What is the Ksp of PbBr2 if the concentration of PbBr2(aq) in a saturated solution is 1.3 x 10-2 moles/L?

What would happen if O2 were removed from the following system at equilibrium at 25°C? 2 NO2(g) 2 NO(g) + O2(g) Kc = 7.4 x 10-1 at 25oC

Of the compounds in the table below, _______ is the least ‾\underline{\text{ least }} least ​ soluble.

Which one of the following graphs best represents the relationship between the concentration of reactants and products with respect to time for the following chemical reaction? 2 NO2(g) 2 NO(g) + O2(g)

Approximately how many grams of Ag2CO3 will dissolve in 1.0 liter of a solution that is 0.10 M in Na2CO3? The Ksp of Ag2CO3 is 6.2 x 10-12.

Ag2SO4(s) is in equilibrium with silver and sulfate ions in solution: Ag2SO4(s) 2Ag+(aq) + SO42-(aq) Which of the following will not increase the amount of solid Ag2SO4(s) present?

If a solution has a Mg2+ ion concentration of 5.0 x 10-3 M and an OH- concentration of 0.010 M, will a precipitate form? Ksp Mg(OH)2 = 1.7 x 10-6.

-Which of the following will be true concerning the Kc of the reaction described by the graph above?

Which of the following equilibria would not be affected by changes in pressure?

The following reaction was carried out: Ni(CO)4 + PPh3(g) →\rightarrow→ PPh3Ni(CO)3 + CO Over 200 seconds, the concentration of Ni(CO)4 dropped from 10 M to 2.5 M. What is the average rate of the reaction in M/s over this time period?

Which of the following equations describes the relationship between the solubility product for AgCl and the solubility of this compound?

What is the solubility in moles per liter of AgBr in water given that the Ksp is 5.0 x 10-13?

Describe the relationship between the rate constants kf and kr for the following one step reaction at equilibrium.

Elements Compounds

The Mole

Structure of the Atom

The Covalent Bond

Ionic and Metallic Bonds

Gases

Making and Breaking of Bonds

Liquids and Solutions

Solids

Acids and Bases

Oxidation-Reduction Reactions

Chemical Thermodynamics

Kinetics

Nuclear Chemistry

Organic Chemistry

Filters

The addition of I₂(g) to a fixed volume container with I₂(g), H₂(g), and HI(g) at equilibrium at a given temperature would cause H₂(g) + I₂(g) 2 HI(g)

A solution is prepared in which the Ag⁺ ion concentration is 2.5 x 10^-3 M and the Cl^- ion concentration is 3.2 x 10^-4 M. Which of the following statements is true given that the K_sp for AgCl is 1.8 x 10^-10?

Which of the following equations correctly describes the relationship between the concentrations of Pb²⁺ and Br^- ions in a saturated solution of PbBr₂(s)?

Which of the following statements correctly describes the following reaction? 2 NH₃(g) $Which of the following statements correctly describes the following reaction? 2 NH<sub>3</sub>(g) N<sub>2</sub>(g) + 3 H<sub>2</sub>(g) \Delta H = 92.2 kJ$ N₂(g) + 3 H₂(g) $\Delta$ H = 92.2 kJ

A solution is 0.10 M in Ca(NO₃)₂. What would the concentration of NaOH need to be for a precipitate of Ca(OH)₂ to form? K_sp Ca(OH)₂ = 5.5 x 10^-6.

What would be the effect of decreasing the pressure on the following reaction after it reaches equilibrium? 2 NO₂(g) 2 NO(g) + O₂(g)

Assume that the reaction quotient, Q_c, for the following reaction at 25°C is 1.0 x 10^-8 2 NO₂(g) 2 NO(g) + O₂(g) K_c = 7.4 x 10^-16 (at 25°C) From this we can conclude:

What is the K_sp of PbBr₂ if the concentration of PbBr₂(aq) in a saturated solution is 1.3 x 10^-2 moles/L?

What would happen if O₂ were removed from the following system at equilibrium at 25°C? 2 NO₂(g) 2 NO(g) + O₂(g) K_c = 7.4 x 10^-1 at 25^oC

Of the compounds in the table below, _ is the $\underline{\text{ least }}$ soluble. $Of the compounds in the table below, _ is the \underline{\text{ least }} soluble.$

Which one of the following graphs best represents the relationship between the concentration of reactants and products with respect to time for the following chemical reaction? 2 NO₂(g) 2 NO(g) + O₂(g)

Approximately how many grams of Ag₂CO₃ will dissolve in 1.0 liter of a solution that is 0.10 M in Na₂CO₃? The K_sp of Ag₂CO₃ is 6.2 x 10^-12.

Ag₂SO₄(s) is in equilibrium with silver and sulfate ions in solution: Ag₂SO₄(s) 2Ag⁺(aq) + SO₄^2-(aq) Which of the following will not increase the amount of solid Ag₂SO₄(s) present?

If a solution has a Mg²⁺ ion concentration of 5.0 x 10^-3 M and an OH^- concentration of 0.010 M, will a precipitate form? K_sp Mg(OH)₂ = 1.7 x 10^-6.

-Which of the following will be true concerning the K_c of the reaction described by the graph above?

The following reaction was carried out: Ni(CO)₄ + PPh₃(g) $\rightarrow$ PPh₃Ni(CO)₃ + CO Over 200 seconds, the concentration of Ni(CO)4 dropped from 10 M to 2.5 M. What is the average rate of the reaction in M/s over this time period?

What is the solubility in moles per liter of AgBr in water given that the K_sp is 5.0 x 10^-13?

Describe the relationship between the rate constants k_f and k_r for the following one step reaction at equilibrium.