PC Vnsab AVHSlide Show Record Review View HelpΑ' Α' ΑAO Search (Alt+Q)FontAaY!!!年主持Paragraph1. Consider the endothermic reaction;JA[]√D. RAISING THE TEMPERATUREHOMEWORK FOR CHEMICAL EQUILIBRIUM AND LE CHATELIER'S PRINCIPLEA. ADDING EXCESS C2H60 TO THE REACTION MIXTUREC. REMOVING C6H1202 AS SOON AS IT FORMSB. PERFORMING THE REACTION USING WET GLASSWAREC2H60 (1) + C4H802 (1)C6H1202 (1) + H20 (1)WHAT WILL BE THE EFFECT OF THE FOLLOWING ON THE EQUILIBRIUM (WILL THEREACTION SHIFT LEFT, RIGHT OR NO EFFECT.Shapes Arrange QuickStylesChisom Obidiegwu: NotesDrawing31999+10.S3FHO모C[

According to Le Chatelier's principle, if a dynamic equilibrium is upset by changing the conditions,…

1. Consider the endothermic reaction; C2H60 (1) + C4H802 (1) C6H1202 (1) + H20 (1) WHAT WILL BE THE EFFECT OF THE FOLLOWING ON THE EQUILIBRIUM (WILL THE REACTION SHIFT LEFT, RIGHT OR NO EFFECT. A. ADDING EXCESS C2H6O TO THE REACTION MIXTURE B. PERFORMING THE REACTION USING WET GLASSWARE C. REMOVING C6H1202 AS SOON AS IT FORMS D. RAISING THE TEMPERATURE

1. Consider the endothermic reaction; C2H60 (1) + C4H802 (1) C6H1202 (1) + H20 (1) WHAT WILL BE THE EFFECT OF THE FOLLOWING ON THE EQUILIBRIUM (WILL THE REACTION SHIFT LEFT, RIGHT OR NO EFFECT. A. ADDING EXCESS C2H6O TO THE REACTION MIXTURE B. PERFORMING THE REACTION USING WET GLASSWARE C. REMOVING C6H1202 AS SOON AS IT FORMS D. RAISING THE TEMPERATURE

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 16Q: Suppose a reaction has the equilibrium constant K = 1.7 108 at a particular temperature. Will there...

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What are homogeneous equilibria? Heterogeneous equilibria? What is the difference in writing K expressions for homogeneous versus heterogeneous reactions? Summarize which species are included in the K expression and which species are not included.
Suppose a reaction has the equilibrium constant K = 1.7 108 at a particular temperature. Will there be a large or small amount of unreacted starting material present when this reaction reaches equilibrium? Is this reaction likely to be a good source of products at this temperature?
Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.
7-64 As we shall see in Chapter 20, there are two forms of glucose, designated alpha and betawhich are in equilibrium in aqueous solution. The equilibrium constant for the reaction is 1.5 at 30°C. (a) If you begin with a fresh 1.0 M solution of D-glucose in water, what will be its concentration when equilibrium is reached? (b) Calculate the percentage of glucose and of glucose present at equilibrium in aqueous solution at 30°C.
7-17 If a certain reaction takes 16 h to go to completion at 10°C, what temperature should we run it if we want it to go to completion in 1 h?
7-29 The following reaction was allowed to reach equilibrium at 25°C. Under each component is its equilibrium concentration. Calculate the equilibrium constant, K, for this reaction.
Consider the decomposition equilibrium for dinitrogen pentoxide: 2N2O5(g)4NO2(g)+O2(g) At a certain temperature and a total pressure of 1.00 atm, the N2O5 is 0.50% decomposed (by moles) at equilibrium. a. If the volume is increased by a factor of 10.0. will the mole percent of N2O5 decomposed at equilibrium be greater than, less than. or equal to 0.50%? Explain your answer. b. Calculate the mole percent of N2O5 that will be decomposed at equilibrium if the volume is increased by a factor of 10.0.
Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that the hydrogen ion concentration she calculated is not correct. She looks up the equilibrium constant for the reaction HCO,-(aq) «=* H+(aq) + COf'(aq) Upon finding that the equilibrium constant for this reaction is 4.8 X 10“H, she decides that her answer in Exercise 12.39 is correct. Explain her reasoning. A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H,CO,(aq) 5=6 H+(aq) + HCO,'(aq) K = 4.4 X 10'7She starts with 0.1000 A1 carbonic acid. W hat are the concentrations of all species at equilibrium?
7-41 The equilibrium constant at 1127°C for the following endothermic reaction is 571: If the mixture is at equilibrium, what happens to K if we: (a) Add some H2S? (b) Add some H2? (c) Lower the temperature to 1000°C?
In Table 12.1 (←Sec. 12-3a) the equilibrium constant for the reaction ⇋ is given as 4.2 × 1052. If this reaction is so product-favored, why can large piles of yellow sulfur exist in our environment (as they do in Louisiana and Texas)?
. Suppose a reaction has the equilibrium constant K=1.7108at a particular temperature. Will there be a large or small amount of unreacted starting material present when this reaction reaches equilibrium? Is this reaction likely to be a good source of products at this temperature?
Data for the reaction [Mn(CO)5(CH3CN)]+ + NC5H5 (Mn(CO)5(NC5H5)]+ + CH3CN are given in the table. Calculate Ea from a plot of In k versus 1/T.