16. Chemical Equilibrium

Le Chatelier's Principle

16. Chemical Equilibrium

Le Chatelier's Principle

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Understanding Le Chatelier's Principle

Le Chatelier's Principle Example

Le Chatelier's Principle Example

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Le Châtelier’s Principle

Le Châtelier’s Principle

An Equilibrium View of Le Chatelier's Principle

Le Chatelier's Principle

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15.2 Le Chatelier's Principle | General Chemistry

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15.2 Le Chatelier's Principle | General Chemistry

Le Chatelier's Principle: Part 2 | Reactions | Chemistry | FuseSchool

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Le Chatelier's Principle Part 1 | Reactions | Chemistry | FuseSchool

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Le Chatelier's Principle Part 1 | Reactions | Chemistry | FuseSchool

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Le Chatelier's Principle

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Equilibrium: Crash Course Chemistry #28

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Practice this topic

Multiple Choice

Consider the reaction below:

CH₄ (g) + F₂ (g) ⇌ CF₄ (g) + HF (g) H = + 38.1 KJ/mol

The following changes will shift the equilibrium to the left except one. Which one would not cause a shift to the left?

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Multiple Choice

The following data was collected for the following reaction at equilibrium

2 A (g) + 3 B (g) ⇌ C (g)

At 25 ^oC K is 5.2 x 10^-4 and at 50^oC K is 1.7 x 10^-7. Which of the following statements is true?

a) The reaction is exothermic.

b) The reaction is endothermic.

c) The enthalpy change, ΔH, is equal to zero.

d) Not enough information is given.

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Multiple Choice

Which direction will the following reaction (in a 10.0 L flask) proceed if a catalyst is added to the system?

CaCO₃ (s) ⇌ CaO (s) + CO₂ (g) K_p = 3.2 x 10^-28

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Multiple Choice

Consider the following gas reaction of A₂ ( shaded spheres) and B₂ ( unshaded spheres)

A₂ (g) + B₂(g) ⇌ 2 AB (g)

Which container proceeds more to completion?

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Multiple Choice

Which of the following will NOT cause the reaction to shift toward the products?

H₂ (g) + I₂ (g) ⇆ 2 HI (g) ΔH = –9.42 kJ

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Multiple Choice

In which direction will the following reaction proceed when P_CO = 0.13 atm, P_H₂O = 0.56 atm, P_CO₂ = 0.62 atm, and P_H₂ = 0.43 atm. K_p for the reaction is 2.7.

CO (g) + H₂O (g) ⇆ CO₂ (g) + H₂ (g)

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Multiple Choice

At 445 ºC calculate the equilibrium concentration of HI when 0.500 M HI, 0.0200 M H₂, and 0.0200 M I₂ are placed in a sealed flask and allowed to reach equilibrium. K_c for this reaction is 50 at 445 ºC.

H₂ (g) + I₂ (g) ⇆ 2 HI (g)

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Multiple Choice

A container is charged with 2.00 mol of I₂ and is allowed to reach equilibrium. The I₂ decomposes to iodine atoms as shown in the following reaction:

I₂ (g) ⇆ 2 I (g)

After the reaction reaches equilibrium, an inert gas is introduced into the container under conditions of constant volume. Which of the following would you expect to happen?

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Multiple Choice

Select correct answer(s) that would yield more products in the following reaction.

CH₄(g) + 4 F₂(g) ⇌ CF₄(g) + 4 HF(g) ΔH = 38.2 kJ/mol

a) increase pressure c) add 0.31 moles of F₂ e) cool down reaction vessel
b) increase temperature d) add some Xenon gas f) decrease volume

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Multiple Choice

At 26°C K_p = 2.3 x 10^–12 and at 56°C K_p = 3.7 x 10^–5 for the hypothetical reaction. Determine if the reaction is endothermic or exothermic.

AB(s) + 2 B(g) ⇌ 3 BB (g) + C (g)

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Textbook Question

When lead(IV) oxide is heated above 300 C, it decomposes according to the following reaction PbO21s2Δ PbO1s2 + O21g2. Consider the two sealed vessels of PbO2 shown here. If both vessels are heated to 400 C and allowed to come to equilibrium, which of the following statements is true? (c) The amount of PbO2 remaining in each vessel will be the same. [Section 15.4]

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Textbook Question

When lead(IV) oxide is heated above 300 C, it decomposes according to the following reaction PbO21s2Δ PbO1s2 + O21g2. Consider the two sealed vessels of PbO2 shown here. If both vessels are heated to 400 C and allowed to come to equilibrium, which of the following statements is true? (a) There will be less PbO2 remaining in vessel A [Section 15.4]

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Textbook Question

When lead(IV) oxide is heated above 300 C, it decomposes according to the following reaction PbO21s2Δ PbO1s2 + O21g2. Consider the two sealed vessels of PbO2 shown here. If both vessels are heated to 400 C and allowed to come to equilibrium, which of the following statements is true? (b) There will be less PbO2 remaining in vessel B. [Section 15.4]

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Textbook Question

Consider the reaction A + B ∆ AB. The vessel on the right contains an equilibrium mixture of A molecules (red spheres), B molecules (blue spheres), and AB molecules. If the stopcock is opened and the contents of the two vessels are allowed to mix, will the reaction go in the forward or reverse direction? Explain.

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Textbook Question

The following pictures represent the composition of the equi- librium mixture for the reaction A + B ∆ AB at 300 K and at 400 K.

Is the reaction exothermic or endothermic? Explain using Le Châtelier's principle.

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Textbook Question

The following picture represents the composition of the equi- librium mixture for the endothermic reaction A2 ∆ 2 A at 500 K. Draw a picture that represents the equilibrium mixture after each of the following changes. (b) Increasing the volume

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Textbook Question

The following pictures represent the initial and equilibrium states for the exothermic decomposition of gaseous A mol- ecules (red) to give gaseous B molecules (blue). (b) Will the number of A molecules in the equilibrium mix- ture increase, decrease, or remain the same after each of the following changes? Explain. (3) Increasing the pressure by adding an inert gas

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Textbook Question

The value of Kw increases with increasing temperature. Is the autoionization of water endothermic or exothermic?

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Textbook Question

Consider the following equilibrium for which H 6 0 2 SO21g2 + O21g2 Δ 2 SO31g2 How will each of the following changes affect an equilibrium mixture of the three gases: (f) SO31g2 is removed from the system?

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Textbook Question

Consider the reaction 4 NH31g2 + 5 O21g2 Δ 4 NO1g2 + 6 H2O1g2, H = -904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (d) decrease the volume of the container in which the reaction occurs

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Textbook Question

Consider the reaction 4 NH31g2 + 5 O21g2 Δ 4 NO1g2 + 6 H2O1g2, H = -904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (f) increase temperature.

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Textbook Question

Consider the reaction 4 NH31g2 + 5 O21g2 Δ 4 NO1g2 + 6 H2O1g2, H = -904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (e) add a catalyst

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Textbook Question

Consider the reaction 4 NH31g2 + 5 O21g2 Δ 4 NO1g2 + 6 H2O1g2, H = -904.4 kJ Does each of the following increase, decrease, or leave unchanged the yield of NO at equilibrium? (c) decrease 3O24

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Textbook Question

Consider this reaction at equilibrium: 2 BrNO(g) ⇌ 2 NO(g) + Br2(g) Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance. b. BrNO is added to the reaction mixture.

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Textbook Question

Consider this reaction at equilibrium: 2 BrNO(g) ⇌ 2 NO(g) + Br2(g) Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance. c. Br2 is removed from the reaction mixture.

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Textbook Question

Consider this reaction at equilibrium: 2 BrNO(g) ⇌ 2 NO(g) + Br2(g) Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance. a. NO is added to the reaction mixture.

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Textbook Question

Methanol 1CH3OH2 can be made by the reaction of CO with H2: CO1g2 + 2 H21g2 Δ CH3OH1g2 (b) To maximize the equilibrium yield of methanol, would you use a high or low temperature?

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Textbook Question

Methanol 1CH3OH2 can be made by the reaction of CO with H2: CO1g2 + 2 H21g2 Δ CH3OH1g2 (c) To maximize the equilibrium yield of methanol, would you use a high or low pressure?

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Textbook Question

Consider this reaction at equilibrium: C(s) + H2O(g) ⇌ CO(g) + H2(g) Predict whether the reaction will shift left, shift right, or remain unchanged after each disturbance. a. C is added to the reaction mixture.

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Textbook Question

Ozone, O3, decomposes to molecular oxygen in the stratosphere according to the reaction 2 O31g2¡3 O21g2. Would an increase in pressure favor the formation of ozone or of oxygen?

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Textbook Question

Each reaction is allowed to come to equilibrium, and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. b. 2 H2S( g) ⇌ 2 H2( g) + S2( g) (volume is decreased)

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Textbook Question

Each reaction is allowed to come to equilibrium, and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. c. CaCO3(s) ⇌ CaO(s) + CO2( g) (volume is increased)

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Textbook Question

Each reaction is allowed to come to equilibrium, and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. a. CO( g) + H2O( g) ⇌ CO2( g) + H2( g) (volume is decreased)

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Textbook Question

The water–gas shift reaction CO1g2 + H2O1g2Δ CO21g2 + H21g2 is used industrially to produce hydrogen. The reaction enthalpy is H = -41 kJ. (b) Could you increase the equilibrium yield of hydrogen by controlling the pressure of this reaction? If so would high or low pressure favor formation of H2(g)?

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Textbook Question

Each reaction is allowed to come to equilibrium, and then the volume is changed as indicated. Predict the effect (shift right, shift left, or no effect) of the indicated volume change. b. PCl3( g) + Cl2( g) ⇌ PCl5( g) (volume is increased)

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Textbook Question

(b) If the temperature is raised by 100 K, does the equilibrium constant for this reaction increase or decrease?

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Textbook Question

Coal, which is primarily carbon, can be converted to natural gas, primarily CH4, by the exothermic reaction: C(s) + 2 H2(g) ⇌ CH4(g) Which disturbance will favor CH4 at equilibrium? c. raising the temperature of the reaction mixture

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Textbook Question

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Textbook Question

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Textbook Question

Coal can be used to generate hydrogen gas (a potential fuel) by the endothermic reaction: C(s) + H2O(g) ⇌ CO(g) + H2(g) If this reaction mixture is at equilibrium, predict whether each disturbance will result in the formation of additional hydrogen gas, the formation of less hydrogen gas, or have no effect on the quantity of hydrogen gas. e. adding a catalyst to the reaction mixture

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Textbook Question

When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2 : SO2Cl21g2 Δ SO21g2 + Cl21g2 (c) According to Le Châtelier's principle, would the percent of SO2Cl2 that decomposes increase, decrease or stay the same if the mixture were transferred to a 15.00-L vessel?

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Textbook Question

Consider the hypothetical reaction A1g2 Δ 2 B1g2. A flask is charged with 0.75 atm of pure A, after which it is allowed to reach equilibrium at 0 C. At equilibrium, the partial pressure of A is 0.36 atm. (c) What could we do to maximize the yield of B?

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Textbook Question

Consider the exothermic reaction: C2H4(g) + Cl2(g) ⇌ C2H4Cl2(g) If you were trying to maximize the amount of C2H4Cl2 produced, which tactic might you try? Assume that the reaction mixture reaches equilibrium. a. increasing the reaction volume b. removing C2H4Cl2 from the reaction mixture as it forms c. lowering the reaction temperature d. adding Cl2

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Textbook Question

Consider the endothermic reaction: C2H4(g) + I2(g) ⇌ C2H4I2(g) If you were trying to maximize the amount of C H I produced, 242 which tactic might you try? Assume that the reaction mixture reaches equilibrium. a. decreasing the reaction volume b. removing I2 from the reaction mixture c. raising the reaction temperature d. adding C2H4 to the reaction mixture

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Textbook Question

The valuable polymer polyurethane is made by a condensa- tion reaction of alcohols (ROH) with compounds that con- tain an isocyanate group (RNCO). Two reactions that can generate a urethane monomer are shown here: (i)

(ii)

(c) If you wanted to promote the formation of the isocya- nate intermediate in each reaction, what could you do, using Le Châtelier's principle?

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Textbook Question

At a temperature of 700 K, the forward and reverse rate constants for the reaction 2 HI1g2 ΔH21g2 + I21g2 are kf = 1.8 * 10-3 M-1 s-1 and kr = 0.063 M-1 s-1. (b) Is the forward reaction endothermic or exothermic if the rate constants for the same reaction have values of kf = 0.097 M-1 s-1 and kr = 2.6 M-1 s-1 at 800 K?

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Textbook Question

Consider the following equilibrium: Ag + 1aq2 + Cl-1aq2 ∆ AgCl1s2 Use Le Châtelier's principle to predict how the amount of solid silver chloride will change when the equilibrium is disturbed by: (c) Adding NO3, which reacts with Ag + to form the com- plex ion Ag1NH322+

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Textbook Question

For the water–gas shift reaction CO1g2 + H2O1g2 ∆ CO21g2 + H21g2, ΔH° = - 41.2 kJ does the amount of H2 in an equilibrium mixture increase or decrease when the temperature is increased? How does Kc change when the temperature is decreased? Justify your answers using Le Châtelier's principle.

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Textbook Question

Consider the exothermic reaction CoCl 2-1aq2 + 6 H O1l2 ∆ Co1H O2 2 + 1aq2 + 4 Cl-1aq2 which interconverts the blue CoCl 2- ion and the pink Co 2 +CoCl 2- increase or decrease when the following changes occur?(c) The solution is diluted with water.

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Textbook Question

The following reaction is important in gold mining: 4 Au1s2 + 8 CN-1aq2 + O21g2 + 2 H2O1l2 ∆ 4 Au1CN22-1aq2 + 4 OH-1aq2For a reaction mixture at equilibrium, in which direction would the reaction go to reestablish equilibrium after each of the following changes? (a) Adding gold

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Textbook Question

The binding of oxygen by hemoglobin in the blood involves the equilibrium reaction: HbH+(aq) + O2(aq)HbO2(aq) + H+(aq) In this equation, Hb is hemoglobin. The pH of normal human blood is highly controlled within a range of 7.35 to 7.45. Given the above equilibrium, why is this important? What would happen to the oxygen-carrying capacity of hemoglobin if blood became too acidic (a dangerous condition known as acidosis)?

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Textbook Question

The equilibrium constant Kp for the reaction PCl51g2 ∆ PCl31g2 + Cl21g2 is 3.81 * 102 at 600 K and 2.69 * 103 at 700 K. (b) How are the equilibrium amounts of reactants and products affected by (iii) addition of a catalyst?

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Textbook Question

Carbon dioxide dissolves in water according to the equations: CO2( g) + H2O(l )H2CO3(aq) H2CO3(aq) + H2O(l)HCO3-(aq) + H3O+(aq) Carbon dioxide levels in the atmosphere have increased about 20% over the last century. Given that Earth's oceans are exposed to atmospheric carbon dioxide, what effect might the increased CO2 be having on the pH of the world's oceans? What effect might this change be having on the limestone structures (primarily CaCO3) of coral reefs and marine shells?

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