Concept explainers
Interpretation:
From the given options, the correct statement for the equilibrium shift to left for the given reaction has to be chosen.
Concept Introduction:
Le Chatelier’s principle:
If some forces applied, the system at equilibrium will get disrupted. This change in equilibrium can be due to the change in pressure or temperature. The change in reactant concentration can also disrupt the equilibrium. Over time, the forward and backward reaction become equal and will attain a new equilibrium. The equilibrium will shifts to right, if more products are formed and the system will shifts to left, if more reactants are formed.
The principle states that if some stress is applied to the system at equilibrium, the system will adjust itself in a direction which reduces the stress.
There are four types of stress or changes which affects the system:
Concentration Changes:
Addition of reactant or product or removal of reactant or product from a system at equilibrium will affects the equilibrium. If some reactant is added to a system at equilibrium, then the equilibrium will shifts to the product side, so that the added reactant get consumed. If product is added then the equilibrium will shift towards left side.
Example
If
If
If
Temperature Changes:
Heat is one of the product in exothermic reaction and heat is used up in endothermic reaction.
Consider an exothermic reaction;
If heat is added up, then the reaction will shift to left so that the amount of heat will decrease.
Lowering the temperature will makes the reaction to shift towards right.
Consider an endothermic reaction;
Increase in temperature will shift the reaction towards right. If heat is added up, then the reaction will shift towards right.
Pressure Changes:
Only the gaseous reactants and products get affected by the pressure change.
Consider the reaction:
3 moles of reactant gives 2 moles of product.
Increase in pressure will shift the reaction towards the side which have fewer molecules.
Want to see the full answer?
Check out a sample textbook solutionChapter 9 Solutions
General, Organic, and Biological Chemistry
- Which of the following is the correct equilibrium constant expression for the reaction 3C(g)A(g)+2B(g) a. [A] [2B]/[3C] b. [3C]/[A] [2B] c. [A] [B]/[C] d. no correct responsearrow_forwardExercise 17.5 For the exothermic reaction 2SO2(g)+O2(g)2SO3(g)predict the equilibrium shift caused by each of the following changes. a. SO2is added. b. SO3is removed. c. The volume is decreased. d. The temperature is decreased.arrow_forwardReaction: 1 A + 1B → 3C The initial [A] is 0.80 M and [B] is 4.90 M. At equilibrium, [A] is 0.40 M. What is the value of K? Answer: 19.44 (0.96)arrow_forward
- Hydrogen sulfide, a colorless gas with a foul odor, dissociates on heating: 2H2S(g)2H2(g)+S2(g) When 0.100 mol H2S was put into a 10.0-L vessel and heated to 1132C, it gave an equilibrium mixture containing 0.0285 mol H2. What is the value of Kc at this temperature?arrow_forwardPhosphorus pentachloride gives an equilibrium mixture of PCl5 PCl3, and Cl2 when heated. PCl5(g)PCl3(g)+Cl2(g) A 1.00-L vessel contains an unknown amount of PCl5 and 0.020 mol each of PCl3 and Cl2 at equilibrium at 250C. How many moles of PCl5 are in the vessel if Kc for this reaction is 0.0415 at 250C?arrow_forwardConsider the following hypothetical reactions. The equilibrium constants K given for each reaction are defined in terms of a concentration unit of molecules per liter. A(g)B(g)K=2X(g)2Y(g)K=62C(g)D(g)K=1 Assume that the reactions have reached equilibrium. Match each of these reactions with one of the containers I to IV (each of which has a volume of 1 L). Identify the color of each molecule (for example, is A red or blue?).arrow_forward
- Synthesis gas (a mixture of CO and H2) is increased in the concentration of hydrogen by passing it with steam over a catalyst. This is the so-called watergas shift reaction. Some of the CO is converted to CO2, which can be removed: CO(g)+H2O(g)CO2(g)+H2(g) Suppose you start with a gaseous mixture containing 1.00 mol CO and 1.00 mol H2O. When equilibrium is reached at 1000C, the mixture contains 0.43 mol H2. What is the molar composition of the equilibrium mixture?arrow_forwardCarbon monoxide and hydrogen react in the presence of a catalyst to form methanol, CH3OH: CO(g)+2H2(g)CH3OH(g) An equilibrium mixture of these three substances is suddenly compressed so that the concentrations of all substances initially double. In what direction does the reaction go as a new equilibrium is attained?arrow_forwardKnowing2 SO₂ (g) + O₂ (g) ⇄ 2 SO₃ (g) Kc=355what is the value of the equilibrium constant for the following?SO₃ (g) ⇄ SO₂ (g) + ½ O₂ (g) Kc= Answerarrow_forward
- Exercise: At 373 K, the equilibrium constant for the reaction COCl2(g) D CO(g) + Cl2(g) is 2.9x10-10. The concentrations of the gases in a 1-L reaction flask are [COCl2]= 3.50x10-3 M, [Cl2]=3.25x10-6 M, and [CO]=1.11x10-5 M. (a) Is the mixture of gases at equilibrium? Answer should be supported with calculations. (b) If not, which direction will the reaction proceed to reach equilibrium?arrow_forwardEquilibrium Learning Check #1 Sulfuric acid is an important industrial chemical that is usually produced by a series of reactions. One of these involves and equilibrium between gaseous sulfur dioxide, oxygen and sulfur trioxide. 2SO2(g) + O2(g) 2SO3(g) If 2.5 mol of sulfur dioxide gas and 2.0 mol of oxygen gas are placed in a sealed 1.0L container and allowed to reach equilibrium, 0.75 mol of sulfur dioxide remains at equilibrium. Use an ICE table to determine the concentration of the other gases at equilibrium.arrow_forwardWhat is the equilibrium composition of a reaction mixture if you start with 0.500 mol each of H2 and I2 in a 1.0-L vessel? The reaction is H2(g)+I2(g)2HI(g)Kc=49.7at458Carrow_forward
- General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning