03:23Le Chatelier's Principle: Part 2 | Reactions | Chemistry | FuseSchoolFuseSchool - Global Education378views
04:15Le Chatelier's Principle Part 1 | Reactions | Chemistry | FuseSchoolFuseSchool - Global Education616views
Multiple ChoiceConsider the reaction below:CH4 (g) + F2 (g) ⇌ CF4 (g) + HF (g) H = + 38.1 KJ/molThe following changes will shift the equilibrium to the left except one. Which one would not cause a shift to the left?1141views3rank8comments
Multiple ChoiceThe 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. 1019views3rank6comments
Multiple ChoiceWhich 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) Kp = 3.2 x 10-28807views3rank1comments
Multiple ChoiceConsider 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? 869views4rank4comments
Multiple ChoiceWhich of the following will NOT cause the reaction to shift toward the products? H2 (g) + I2 (g) ⇆ 2 HI (g) ΔH = –9.42 kJ217views
Multiple ChoiceIn which direction will the following reaction proceed when PCO = 0.13 atm, PH2O = 0.56 atm, PCO2 = 0.62 atm, and PH2 = 0.43 atm. Kp for the reaction is 2.7. CO (g) + H2O (g) ⇆ CO2 (g) + H2 (g)216views
Multiple ChoiceAt 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. Kc for this reaction is 50 at 445 ºC. H2 (g) + I2 (g) ⇆ 2 HI (g)292views
Multiple ChoiceA 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?210views
Multiple ChoiceSelect 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/mola) increase pressure c) add 0.31 moles of F2 e) cool down reaction vesselb) increase temperature d) add some Xenon gas f) decrease volume268views3rank
Multiple ChoiceAt 26°C Kp = 2.3 x 10–12 and at 56°C Kp = 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)260views3rank
Textbook QuestionWhen 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]298views
Textbook QuestionWhen 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]311views
Textbook QuestionWhen 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] 703views
Textbook QuestionConsider 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. 548views
Textbook QuestionThe 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.374views
Textbook QuestionThe 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 volume303views
Textbook QuestionThe 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 gas345views
Textbook QuestionThe value of Kw increases with increasing temperature. Is the autoionization of water endothermic or exothermic?2583views
Textbook QuestionConsider 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?395views
Textbook QuestionConsider 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 occurs482views
Textbook QuestionConsider 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.405views
Textbook QuestionConsider 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 catalyst299views
Textbook QuestionConsider 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 3O24293views
Textbook QuestionConsider 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.769views
Textbook QuestionConsider 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.1917views
Textbook QuestionConsider 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.811views
Textbook QuestionMethanol 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?579views
Textbook QuestionMethanol 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?429views
Textbook QuestionConsider 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.5782views
Textbook QuestionOzone, 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?802views
Textbook QuestionEach 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)1204views
Textbook QuestionEach 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)650views
Textbook QuestionEach 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)453views
Textbook QuestionThe 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)?1392views1rank
Textbook QuestionEach 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)372views
Textbook Question(b) If the temperature is raised by 100 K, does the equilibrium constant for this reaction increase or decrease?620views
Textbook QuestionCoal, 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 mixture1681views
Textbook QuestionCoal, 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? e. adding a catalyst to the reaction mixture446views
Textbook QuestionCoal, 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? b. adding more H2 to the reaction mixture859views
Textbook QuestionCoal 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 mixture1282views1rank
Textbook QuestionWhen 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?552views
Textbook QuestionConsider 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?470views
Textbook QuestionConsider 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 Cl22110views
Textbook QuestionConsider 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 mixture1511views
Textbook QuestionThe 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?373views
Textbook QuestionAt 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?293views
Textbook QuestionConsider 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+324views
Textbook QuestionFor 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.612views
Textbook QuestionConsider 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.381views
Textbook QuestionThe 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 gold289views
Textbook QuestionThe 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)?10024views
Textbook QuestionThe 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?465views
Textbook QuestionCarbon 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?8612views
Textbook QuestionBaking soda (sodium bicarbonate) decomposes when it is heated: 2 NaHCO31s2 ∆ Na2CO31s2 + CO21g2 + H2O1g2 ΔH° = + 136 kJ Consider an equilibrium mixture of reactants and products in a closed container. How does the number of moles of CO2 change when the mixture is disturbed by the following: (b) Adding water vapor1097views
Textbook QuestionA platinum catalyst is used in automobile catalytic convert- ers to hasten the oxidation of carbon monoxide: 2 CO1g2 + O 1g2 ∆Pt 2 CO 1g2 ΔH° = - 566 kJ Suppose that you have a reaction vessel containing an equilibrium mixture of CO1g2, O21g2, and CO21g2. Under the following conditions, will the amount of CO increase, decrease, or remain the same? (e) The pressure is increased by adding O2 gas.489views
Textbook QuestionIn automobile catalytic converters, the air pollutant nitric oxide is converted to nitrogen and oxygen. Listed in the table are forward and reverse rate constants for the reac- tion 2 NO1g2 ∆ N21g2 + O21g2. Temperature (K) kf1M — 1 s-12 kr1M-1 s — 12 1400 0.29 1.1 * 10-6 1500 1.3 1.4 * 10-5 Is the reaction endothermic or exothermic? Explain in terms of kinetics.424views
Textbook QuestionGiven the Arrhenius equation, k = Ae-Ea>RT, and the rela- tion between the equilibrium constant and the forward and reverse rate constants, Kc = kf>kr, explain why Kc for an exothermic reaction decreases with increasing temperature.402views
Textbook QuestionAt 1000 K, Kp = 2.1 * 106 and ΔH° = - 107.7 kJ for the reaction H21g2 + Br21g2 ∆ 2 HBr1g2. (b) For the equilibrium in part (a), each of the following changes will increase the equilibrium partial pressure of HBr. Choose the change that will cause the greatest increase in the pressure of HBr, and explain your choice. (ii) Adding 0.10 mol of Br2483views
Textbook QuestionThe equilibrium constant Kc for the gas-phase thermal decom-position of cyclopropane to propene is 1.0 * 105 at 500 K: (c) Can you alter the ratio of the two concentrations at equilibrium by adding cyclopropane or by decreasing the volume of the container? Explain.436views
Textbook QuestionFor the decomposition reaction PCl51g2 ∆ PCl31g2 + Cl21g2, Kp = 381 at 600 K and Kc = 46.9 at 700 K. (a) Is the reaction endothermic or exothermic? Explain. Does your answer agree with what you would predict based on bond energies?301views