IIIO Kinetics and EquilibriumWriting the concentration equilibrium expression for a heterogeneous...Write the concentration equilibrium constant expression for this reaction.Cr₂0 (aq)+61 (aq)+14 H(aq)-31,(s)+2 Cr (aq)+7H₂O(1)号G0/5

Equilibrium constant (Keq ):Equilibrium constant is the ratio of equilibrium concentration of…

Answered: III O Kinetics and Equilibrium Writing…

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 13CR

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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)?
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.
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.
The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction] in which each system will proceed to leach equilibrium. (a) 2NH3(g)N2(g)+3H2(g) Kc=17;[NH3]=0.20M,[N2]=1.00M,[H2]=1.00M (b) 2NH3(g)N2(g)+3H2(g) Kp=6.8104 initial pressures NH3=3.0atm,N2=2.0atm,H2=1.0atm (c) 2SO3(g)2SO2(g)+O2(g) Kc=0.230;[SO3]=0.00M,[SO2]=1.00M,[O2]=1.00M (d) 2SO3(g)2SO2(g)+O2(g) Kp=16.5 initial pressures SO3=1.00atm,SO2=1.00atm,O2=1.00atm (e) 2NO(g)+CI2(g)2NOCI(g) Kc=4.6104;[NO]=1.00M,[CI2]=1.00M,[NOCI]=0M (f) N2(g)+O2(g)2NO(g) Kp=0.050 initial pressures NO=1.00atm,N2=O2=5atm
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
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.
The following series of diagrams represent the reaction XY followed over a period of time. The X molecules are red and the Y molecules are green. At the end of the time period depicted, has the reaction system reached equilibrium? Justify your answer with a one-sentence explanation.
Which reaction mechanism assumptions are unimportant in describing simple ionic reactions between cations and anions? Why?
What is the law of mass action? Is it true that the value of K depends on the amounts of reactants and products mixed together initially? Explain. Is it true that reactions with large equilibrium constant values are very fast? Explain. There is only one value of the equilibrium constant for a particular system at a particular temperature, but there is an infinite number of equilibrium positions. Explain.
. Suppose that for the reaction 2N2O(g)+O2(g)4NO((g))it is determined, at a particular temperature, that the equilibrium concentrations arc [NO(g)]=0.00341M,[N2O(g)]=0.0293M, and [O2(g)]=0.0325M. Calculate the value of K for the reaction at this temperature.
In a particular experiment, the equilibrium constant measured for the reaction, Cl2(g)+NO2(g)Cl2NO2(g), is 2.8. Based on this measurement, calculate AG° for this reaction. Calculate AG° using data from Appendix E at the back of the book and discuss the agreement between your two calculations.

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III O Kinetics and Equilibrium Writing the concentration equilibrium expression for a heterogeneous... Write the concentration equilibrium constant expression for this reaction. Cr₂0 (aq)+61 (aq)+14 H(aq)-31,(s)+2 Cr (aq)+7H₂O(1) 号 G 0/5