This chemical equation represents a reaction: 2 ICl (9) L (9) + 3Cl (g) Suppose a closed flask contains only gaseous ICl,, and the concentration of ICl, is 0.10 M. How will these initial conditions affect the progress of the reaction? The concentration of the reactant will decrease, and the concentrations of the products will increase, until the concentration of each product equals 0.10 M. O The concentrations of the reactant and the products will increase until the concentration of each product equals 0.10 M. The concentration of the reactant will decrease, and the concentrations of the products will increase, until the rate of the forward reaction equais the rate of the reverse reaction The concentrations of the reactant and the products will increase until the rate of the forward reaction equals the rate of the reverse reaction

This chemical equation represents a reaction: 2 ICl (9) L (9) + 3Cl (g) Suppose a closed flask contains only gaseous ICl,, and the concentration of ICl, is 0.10 M. How will these initial conditions affect the progress of the reaction? The concentration of the reactant will decrease, and the concentrations of the products will increase, until the concentration of each product equals 0.10 M. O The concentrations of the reactant and the products will increase until the concentration of each product equals 0.10 M. The concentration of the reactant will decrease, and the concentrations of the products will increase, until the rate of the forward reaction equais the rate of the reverse reaction The concentrations of the reactant and the products will increase until the rate of the forward reaction equals the rate of the reverse reaction

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 10CR: . Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why...

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. Suppose K=4.5103at a certain temperature for the reaction PCl5(g)PCl3(g)+Cl2(g)If it is found that the concentration of PCl5is twice the concentration of PCl3, what must be the concentration of Cl2under these conditions?
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?
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
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In the reaction in Exercise 12.33, another trial was carried out. The reaction began with an initial concentration of N2 equal to the initial concentration of NO. Each had a concentration of 0.100 mol L-1. WTat were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L'1 ofO2, what were the equilibrium concentrations of all species?
An equilibrium involving the carbonate and bicarbonate ions exists in natural waters: HCO5_(aq) «=* H+(aq) + COf-(aq) Assuming that the reactions in both directions are elementary' processes: Write rate expressions for the forward and reverse reactions. Write an expression for the equilibrium constant based on the rates of the forward and reverse reactions.
. Explain what it means that a reaction has reached a state of chemical equilibrium. Explain why equilibrium is a dynamic state: Does a reaction really “stop” when the system reaches a state of equilibrium? Explain why, once a chemical system has reached equilibrium, the concentrations of all reactants remain constant with time. Why does this constancy of concentration not contradict our picture of equilibrium as being dynamic? What happens to the rates of the forward and reverse reactions as a system proceeds to equilibrium from a starting point where only reactants are present?
The experiment in Exercise 12.33 was redesigned so that the reaction started with 0.15 mol each of N2 and O2 being injected into a 1.0-L container at 2500 K. The equilibrium constant at 2500 K is 3.6 X 10“’. What was the composition of the reaction mixture after equilibrium was attained? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?
Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?
The creation of shells by mollusk species is a fascinating process. By utilizing the Ca2+ in their food and aqueous environment, as well as some complex equilibrium processes, a hard calcium carbonate shell can be produced. One important equilibrium reaction in this complex process is HCO3(aq)H+(aq)+CO32(aq)K=5.61011 If 0.16 mole of HCO3 is placed into 1.00 L of solution, what will be the equilibrium concentration of CO32?
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