What is the fluoride ion concentration in a saturated solution of SrF2 if the strontium ion concentration is 5.8 x 10 - 4 M?

A) 5.8 x 10 - 4 B) 2.9 x 10 - 4 C) 1.2 x 10 - 3 D) 1.8 x 10 - 3 E) none of the above A) 5.8 x 10 - 4 B) 2.9 x 10 - 4 C) 1.2 x 10 - 3 D) 1.8 x 10 - 3 E) none of the above

What is the relationship between the changes in the concentration of NO2 and O2 as the following reaction comes to equilibrium? 2 NO2(g) 2 NO(g) + O2(g) &emsp; Kc = 7.4 x 10-16 &emsp; (at 25°C)

A) [NO2] = -[O2] B) [NO2] = -2 [O2] C) [O2] = -2 [NO2] D) There is no relationship between the changes in the concentrations of these substances. E) none of the above A) [NO2] = -[O2] B) [NO2] = -2 [O2] C) [O2] = -2 [NO2] D) There is no relationship between the changes in the concentrations of these substances. E) none of the above

If 6.5 x 10 - 5 moles of Ag2CrO4 will dissolve in 1.0 liter of water at 25 C, what is the Ksp of Ag2CrO4?

A) 6.5 x 10 - 5 B) 4.2 x 10 - 9 C) 2.7 x 10 - 13 D) 1.1 x 10 - 12 E) 3.3 x 10 - 5 A) 6.5 x 10 - 5 B) 4.2 x 10 - 9 C) 2.7 x 10 - 13 D) 1.1 x 10 - 12 E) 3.3 x 10 - 5

What would happen if Cl2 is added to the following system at equilibrium? H2(g) + Cl2(g) 2 HCl(g)

A) The concentrations of both H2 and HCl would remain the same. B) The concentrations of both H2 and HCl would increase. C) The concentrations of both H2 and HCl would decrease. D) The concentration of H2 would increase, but HCl would decrease. E) The concentration of H2 would decrease, but HCl would increase. A) The concentrations of both H2 and HCl would remain the same. B) The concentrations of both H2 and HCl would increase. C) The concentrations of both H2 and HCl would decrease. D) The concentration of H2 would increase, but HCl would decrease. E) The concentration of H2 would decrease, but HCl would increase.

If at any moment in time, we find that Qc is larger than Kc for the reaction Cl2(g) + 3 F2(g) 2 ClF3(g) We can conclude that:

A) The reaction is at equilibrium. B) The reaction cannot reach equilibrium. C) The reaction must shift to the right to reach equilibrium. D) The reaction must shift to the left to reach equilibrium. E) None of the above are possible. A) The reaction is at equilibrium. B) The reaction cannot reach equilibrium. C) The reaction must shift to the right to reach equilibrium. D) The reaction must shift to the left to reach equilibrium. E) None of the above are possible.

What would happen to the extent of the decomposition of PCl5 at a given temperature if the pressure on the system were decreased? PCl5(g) PCl3(g) + Cl2(g)

A) It would increase. B) It would decrease. C) It would remain constant. D) Not enough information is given to determine this. A) It would increase. B) It would decrease. C) It would remain constant. D) Not enough information is given to determine this.

Hidden Assumptions that make Equilibrium Calculations Easier What Do We Do When the Approximation Fails? based on the following reaction: 2HS1U1B12S1U1B0O(g) 2HS1U1B12S1U1B0(g) + OS1U1B12S1U1B0(g) KS1U1B1cS1U1B0 = 2 x 10S1U1P1-42S1S1P0 (at 25S1U1P1oS1S1P0C) -Starting with only 0.10 M H2O(g), which equation correctly shows the equilibrium concentrations of the reactants and products? ( $\Delta$ C represents the change in concentration of O2(g))

A) B) C) D) E) None of the above A) B) C) D) E) None of the above

Hidden Assumptions that make Equilibrium Calculations Easier What Do We Do When the Approximation Fails? based on the following reaction: 2HS1U1B12S1U1B0O(g) 2HS1U1B12S1U1B0(g) + OS1U1B12S1U1B0(g) KS1U1B1cS1U1B0 = 2 x 10S1U1P1-42S1S1P0 (at 25S1U1P1oS1S1P0C) -The equation below solves for the change in concentration for the given reaction assuming the initial concentration of H2O(g) is 0.10 M. Which equation will result if it is assumed that the change will be much smaller than the initial concentration of H2O(g)?

A) B) C) D) E) None of the above A) B) C) D) E) None of the above

Exam 10: An Introduction to Kinetics and Equilibrium

A 50.0 mL solution of 0.015 M of Ca(NO₃)₂ is added to 50.0 mL of 0.010 M NaF. Write a net ionic equation that shows the formation of a precipitate of CaF₂(s). Given that the K_sp of CaF₂(s) is 4.0 x 10^-11, will a precipitate form from this mixture?

(Essay)

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Question 21

Which is the correct reaction for the solubility constant expression (K_sp) of CaF₂(s)?

(Multiple Choice)

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Question 22

Which of the following statements is correct?

(Multiple Choice)

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Question 23

What is the effect of increasing the temperature on the following reaction? 2 CO(g) + O₂(g) 2 CO₂(g) + heat

(Multiple Choice)

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Question 24

Suppose that the reaction quotient, Q_c, for a chemical reaction was found to be close to unity (Q_c $\approx$ 1). Given this information we can accurately predict

(Multiple Choice)

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Question 25

What is the fluoride ion concentration in a saturated solution of SrF₂ if the strontium ion concentration is 5.8 x 10 ^- ⁴M?

(Multiple Choice)

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Question 26

What is the relationship between the changes in the concentration of NO₂ and O₂ as the following reaction comes to equilibrium? 2 NO₂(g) 2 NO(g) + O₂(g) K_c = 7.4 x 10^-16 (at 25°C)

(Multiple Choice)

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Question 27

If 6.5 x 10 ^- ⁵ moles of Ag₂CrO₄ will dissolve in 1.0 liter of water at 25 C, what is the K_sp of Ag₂CrO₄?

(Multiple Choice)

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Question 28

What is the correct solubility constant expression of Ba₃(PO₄)₂?

(Multiple Choice)

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Question 29

One of the products of the reaction between NO₂ and CO is CO₂. By writing the equation for the reaction (Hint: the coefficients for all reactants and products are 1), decide whether an increase in pressure:

(Multiple Choice)

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Question 30

What would happen if Cl₂ is added to the following system at equilibrium? H₂(g) + Cl₂(g) 2 HCl(g)

(Multiple Choice)

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Question 31

Which of the following changes will shift the following equilibrium to the right? AgCl(s) $Which of the following changes will shift the following equilibrium to the right? AgCl(s) Ag+(aq) + Cl-(aq) \Delta H = 65.4 kJ/molrxn$ Ag⁺(aq) + Cl^-(aq) $\Delta$ H = 65.4 kJ/mol_rxn

(Multiple Choice)

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Question 32

For the reaction 2 NOCl(g) 2 NO(g) + Cl₂ K_c = 5.6 x 10^-6 (at 400 K) What is the relationship between the magnitude of the changes in the concentrations of NOCl and Cl₂ as this reaction comes to equilibrium?

(Multiple Choice)

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Question 33

The equilibrium constant for the following reaction becomes larger as the temperature at which the reaction is run increases. 2 NOCl(g) 2 NO(g) + Cl₂(g) K_c = 5.6 x 10^-6 at 400 K What does this tell us about the reaction?

(Multiple Choice)

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Question 34

If at any moment in time, we find that Q_c is larger than K_c for the reaction Cl₂(g) + 3 F₂(g) 2 ClF₃(g) We can conclude that:

(Multiple Choice)

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Question 35

Which of the following equations correctly describes the relationship between the concentrations of Sr²⁺ and PO₄^3- ions in a saturated solution of Sr₃(PO₄)₂(s)?

(Multiple Choice)

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Question 36

What would happen to the extent of the decomposition of PCl₅ at a given temperature if the pressure on the system were decreased? PCl₅(g) PCl₃(g) + Cl₂(g)

(Multiple Choice)

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Question 37

Hidden Assumptions that make Equilibrium Calculations Easier What Do We Do When the Approximation Fails? based on the following reaction: 2H₂O(g) 2H₂(g) + O₂(g) K_c = 2 x 10^-42 (at 25^oC) -When solving a problem with the initial conditions outlined below, we rearrange the problem to give an intermediate set of conditions where the concentration of one of the reactants or products is equal to zero. Fe(CO)₅ Fe(CO)₄ + CO Initial: 0.10 M 0.10 M 0.005 M Our choice of whether to push the reaction all the way to the right or all the way to the left is determined by which of the following goals?

(Multiple Choice)

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Question 38

Hidden Assumptions that make Equilibrium Calculations Easier What Do We Do When the Approximation Fails? based on the following reaction: 2H₂O(g) $Hidden Assumptions that make Equilibrium Calculations Easier What Do We Do When the Approximation Fails? based on the following reaction: 2H2O(g) 2H2(g) + O2(g) Kc = 2 x 10-42 (at 25oC) -Starting with only 0.10 M H2O(g), which equation correctly shows the equilibrium concentrations of the reactants and products? ( \Delta C represents the change in concentration of O2(g))$ 2H₂(g) + O₂(g) K_c = 2 x 10^-42 (at 25^oC) -Starting with only 0.10 M H₂O(g), which equation correctly shows the equilibrium concentrations of the reactants and products? ( $\Delta$ C represents the change in concentration of O₂(g))

(Multiple Choice)

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Question 39

Hidden Assumptions that make Equilibrium Calculations Easier What Do We Do When the Approximation Fails? based on the following reaction: 2H₂O(g) 2H₂(g) + O₂(g) K_c = 2 x 10^-42 (at 25^oC) -The equation below solves for the change in concentration for the given reaction assuming the initial concentration of H₂O(g) is 0.10 M. Which equation will result if it is assumed that the change will be much smaller than the initial concentration of H₂O(g)?

(Multiple Choice)

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Question 40

Showing 21 - 40 of 94

A 50.0 mL solution of 0.015 M of Ca(NO₃)₂ is added to 50.0 mL of 0.010 M NaF. Write a net ionic equation that shows the formation of a precipitate of CaF₂(s). Given that the K_sp of CaF₂(s) is 4.0 x 10^-11, will a precipitate form from this mixture?

Which is the correct reaction for the solubility constant expression (K_sp) of CaF₂(s)?

Which of the following statements is correct?

What is the effect of increasing the temperature on the following reaction? 2 CO(g) + O₂(g) 2 CO₂(g) + heat

Suppose that the reaction quotient, Q_c, for a chemical reaction was found to be close to unity (Q_c $\approx$ 1). Given this information we can accurately predict

What is the fluoride ion concentration in a saturated solution of SrF₂ if the strontium ion concentration is 5.8 x 10 ^- ⁴M?

What is the relationship between the changes in the concentration of NO₂ and O₂ as the following reaction comes to equilibrium? 2 NO₂(g) 2 NO(g) + O₂(g) K_c = 7.4 x 10^-16 (at 25°C)

If 6.5 x 10 ^- ⁵ moles of Ag₂CrO₄ will dissolve in 1.0 liter of water at 25 C, what is the K_sp of Ag₂CrO₄?

What is the correct solubility constant expression of Ba₃(PO₄)₂?

One of the products of the reaction between NO₂ and CO is CO₂. By writing the equation for the reaction (Hint: the coefficients for all reactants and products are 1), decide whether an increase in pressure:

What would happen if Cl₂ is added to the following system at equilibrium? H₂(g) + Cl₂(g) 2 HCl(g)

For the reaction 2 NOCl(g) 2 NO(g) + Cl₂ K_c = 5.6 x 10^-6 (at 400 K) What is the relationship between the magnitude of the changes in the concentrations of NOCl and Cl₂ as this reaction comes to equilibrium?

The equilibrium constant for the following reaction becomes larger as the temperature at which the reaction is run increases. 2 NOCl(g) 2 NO(g) + Cl₂(g) K_c = 5.6 x 10^-6 at 400 K What does this tell us about the reaction?

If at any moment in time, we find that Q_c is larger than K_c for the reaction Cl₂(g) + 3 F₂(g) 2 ClF₃(g) We can conclude that:

Which of the following equations correctly describes the relationship between the concentrations of Sr²⁺ and PO₄^3- ions in a saturated solution of Sr₃(PO₄)₂(s)?

What would happen to the extent of the decomposition of PCl₅ at a given temperature if the pressure on the system were decreased? PCl₅(g) PCl₃(g) + Cl₂(g)

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

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Exam 10: An Introduction to Kinetics and Equilibrium

A 50.0 mL solution of 0.015 M of Ca(NO3)2 is added to 50.0 mL of 0.010 M NaF. Write a net ionic equation that shows the formation of a precipitate of CaF2(s). Given that the Ksp of CaF2(s) is 4.0 x 10-11, will a precipitate form from this mixture?

Which is the correct reaction for the solubility constant expression (Ksp) of CaF2(s)?

Which of the following statements is correct?

What is the effect of increasing the temperature on the following reaction? 2 CO(g) + O2(g) 2 CO2(g) + heat

Suppose that the reaction quotient, Qc, for a chemical reaction was found to be close to unity (Qc ≈\approx≈ 1). Given this information we can accurately predict

What is the fluoride ion concentration in a saturated solution of SrF2 if the strontium ion concentration is 5.8 x 10 - 4 M?

What is the relationship between the changes in the concentration of NO2 and O2 as the following reaction comes to equilibrium? 2 NO2(g) 2 NO(g) + O2(g) Kc = 7.4 x 10-16 (at 25°C)

If 6.5 x 10 - 5 moles of Ag2CrO4 will dissolve in 1.0 liter of water at 25 C, what is the Ksp of Ag2CrO4?

What is the correct solubility constant expression of Ba3(PO4)2?

One of the products of the reaction between NO2 and CO is CO2. By writing the equation for the reaction (Hint: the coefficients for all reactants and products are 1), decide whether an increase in pressure:

What would happen if Cl2 is added to the following system at equilibrium? H2(g) + Cl2(g) 2 HCl(g)

Which of the following changes will shift the following equilibrium to the right? AgCl(s) Ag+(aq) + Cl-(aq) Δ\DeltaΔ H = 65.4 kJ/molrxn

For the reaction 2 NOCl(g) 2 NO(g) + Cl2 Kc = 5.6 x 10-6 (at 400 K) What is the relationship between the magnitude of the changes in the concentrations of NOCl and Cl2 as this reaction comes to equilibrium?

The equilibrium constant for the following reaction becomes larger as the temperature at which the reaction is run increases. 2 NOCl(g) 2 NO(g) + Cl2(g) Kc = 5.6 x 10-6 at 400 K What does this tell us about the reaction?

If at any moment in time, we find that Qc is larger than Kc for the reaction Cl2(g) + 3 F2(g) 2 ClF3(g) We can conclude that:

Which of the following equations correctly describes the relationship between the concentrations of Sr2+ and PO43- ions in a saturated solution of Sr3(PO4)2(s)?

What would happen to the extent of the decomposition of PCl5 at a given temperature if the pressure on the system were decreased? PCl5(g) PCl3(g) + Cl2(g)

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

A 50.0 mL solution of 0.015 M of Ca(NO₃)₂ is added to 50.0 mL of 0.010 M NaF. Write a net ionic equation that shows the formation of a precipitate of CaF₂(s). Given that the K_sp of CaF₂(s) is 4.0 x 10^-11, will a precipitate form from this mixture?

Which is the correct reaction for the solubility constant expression (K_sp) of CaF₂(s)?

What is the effect of increasing the temperature on the following reaction? 2 CO(g) + O₂(g) 2 CO₂(g) + heat

Suppose that the reaction quotient, Q_c, for a chemical reaction was found to be close to unity (Q_c $\approx$ 1). Given this information we can accurately predict

What is the fluoride ion concentration in a saturated solution of SrF₂ if the strontium ion concentration is 5.8 x 10 ^- ⁴M?

What is the relationship between the changes in the concentration of NO₂ and O₂ as the following reaction comes to equilibrium? 2 NO₂(g) 2 NO(g) + O₂(g) K_c = 7.4 x 10^-16 (at 25°C)

If 6.5 x 10 ^- ⁵ moles of Ag₂CrO₄ will dissolve in 1.0 liter of water at 25 C, what is the K_sp of Ag₂CrO₄?

What is the correct solubility constant expression of Ba₃(PO₄)₂?

One of the products of the reaction between NO₂ and CO is CO₂. By writing the equation for the reaction (Hint: the coefficients for all reactants and products are 1), decide whether an increase in pressure:

What would happen if Cl₂ is added to the following system at equilibrium? H₂(g) + Cl₂(g) 2 HCl(g)

For the reaction 2 NOCl(g) 2 NO(g) + Cl₂ K_c = 5.6 x 10^-6 (at 400 K) What is the relationship between the magnitude of the changes in the concentrations of NOCl and Cl₂ as this reaction comes to equilibrium?

The equilibrium constant for the following reaction becomes larger as the temperature at which the reaction is run increases. 2 NOCl(g) 2 NO(g) + Cl₂(g) K_c = 5.6 x 10^-6 at 400 K What does this tell us about the reaction?

If at any moment in time, we find that Q_c is larger than K_c for the reaction Cl₂(g) + 3 F₂(g) 2 ClF₃(g) We can conclude that:

Which of the following equations correctly describes the relationship between the concentrations of Sr²⁺ and PO₄^3- ions in a saturated solution of Sr₃(PO₄)₂(s)?

What would happen to the extent of the decomposition of PCl₅ at a given temperature if the pressure on the system were decreased? PCl₅(g) PCl₃(g) + Cl₂(g)