An intermediate step in the process that ultimately produces sulfuric acid, is the catalytic oxidation of SO, to SO3. Vanadium(V) oxide is the catalyst. The three chemical species in the reaction are in equilibrium as follows: 250, (g) + O2(g) 2803(g) Which of the following are true statements about this reaction? 1. When SO, is mixed with O, in a container, the initial rate of the forward reaction (production of SO3) is faster than the initial rate of the reverse reaction (production of SO2). 2. As SO, is used up and SO3 accumulates, the rate of the forward reaction increases and the rate of the reverse reaction decreases. 3. At equilibrium the rate of production of SO3 reaches zero. 4. At equilibrium the concentration of SO, will no longer be changing. > View Available Hint(s) O 1 and 2 O 2 and 3 O 1 and 3 O 1 and 4

An intermediate step in the process that ultimately produces sulfuric acid, is the catalytic oxidation of SO, to SO3. Vanadium(V) oxide is the catalyst. The three chemical species in the reaction are in equilibrium as follows: 250, (g) + O2(g) 2803(g) Which of the following are true statements about this reaction? 1. When SO, is mixed with O, in a container, the initial rate of the forward reaction (production of SO3) is faster than the initial rate of the reverse reaction (production of SO2). 2. As SO, is used up and SO3 accumulates, the rate of the forward reaction increases and the rate of the reverse reaction decreases. 3. At equilibrium the rate of production of SO3 reaches zero. 4. At equilibrium the concentration of SO, will no longer be changing. > View Available Hint(s) O 1 and 2 O 2 and 3 O 1 and 3 O 1 and 4

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.9PAE: An equilibrium involving the carbonate and bicarbonate ions exists in natural waters: HCO5_(aq) «=*...

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Many sugars undergo a process called mutarotation, in which the sugar molecules interconvert between two isomeric forms, finally reaching an equilibrium between them. This is true for the simple sugar glucose, C6H12O6, which exists in solution in isomeric forms called alpha-glucose and beta-glucose. If a solution of glucose at a certain temperature is analyzed, and it is found that the concentration of alpha-glucose is twice the concentration of beta-glucose, what is the value of K for the interconversion reaction?
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?
Is a system at equilibrium if the rate constants of the forward and reverse reactions are equal?
Consider the reaction: A(g)+2B(g)+C(s)2D(g)At 25C, only A, B, and C are present. The partial pressures of A, B, and D are given as PA, PB, and PD. Equilibrium is established 18 minutes after the reaction starts. Use terms is less than (LT), is greater than (GT), is equal to (EQ), or insufficient information (X) to answer the following questions. (a) PD at 5 min PA. (b) PA at 21 min PA at 27 min. (c) PB at 7 min PB at 13 min.(d) After 20 min, more B is added. When equilibrium is reestablished, K before the addition K after the addition. (e) After 20 min, the temperature is increased to 35C. PA before the temperature increase PA after the temperature increase after equilibrium is reestablished.
Consider the system A(g)+2B(g)+C(g)2D(g)at 25C. At zero time, only A, B, and C are present. The reaction reaches equilibrium 10 min after the reaction is initiated. Partial pressures of A, B, and D are written as PA, PB, and PD. Answer the questions below, using LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more information required). (a) PD at 11 min PD at 12 min. (b) PA at 5 min PA at 7 min. (c) K for the forward reaction K for the reverse reaction. (d) At equilibrium, K Q. (e) After the system is at equilibrium, more of gas B is added. After the system returns to equilibrium, K before the addition of B K after the addition of B. (f) The same reaction is initiated, this time with a catalyst K for the system without a catalyst the system with a catalyst. (g) K for the formation of one mole of D K for the formation of two moles of D. (h) The temperature of the system is increased to 35C. PB at equilibrium at 25C PB at equilibrium at 35C. (i) Ten more grams of C are added to the system. PB before the addition of C PB after the addition of C.
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 reach equilibrium. (a) 2NH3(g)N2(g)+3H2(g) Kc=17;[NH3]=0.50M,[N2]=0.15M,[H2]=0.12M (b) 2NH3(g)N2(g)+3H2(g) Kp=6.8104 initial pressures NH3=2.00atm,N2=10.00atm,H2=10.00atm (c) 2SO3(g)2SO2(g)+O2(g) Kc=0.230;[SO3]=2.00M,[SO2]=2.00M,[O2]=2.00M (d) 2SO3(g)2SO2(g)+O2(g) Kp=16.5 initial pressures SO2=1.00atm,O2=1.130atm,SO3=0atm (e) 2NO(g)+CI2(g)2NOCI(g) Kp=2.5103 ; initial pressures; NO=1.00atm,CI2=1.00atm,NOCI=0atm (f) N2(g)+O2(g)2NO(g) Kc=0.050 ; [N2]=1.00M,[O2]=0.200M,[NO]=1.00M
At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
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.
When writing a chemical equation for a reaction that comes to equilibrium. how do we indicate symbolically that the reaction is reversible?
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.
At 25C, Kp. = 2.9 103 for the reaction NH4OCONH2(s)2NH3(g)+CO2(g) In an experiment carried out at 25C, a certain amount of NH4OCONH2 is placed in an evacuated rigid container and allowed to come to equilibrium. Calculate the total pressure in the container at equilibrium.
Dinitrogen trioxide decomposes to NO and NO2, in an endothermic process (rH = 40.5 kJ/mol-rxn). N2O3(g) NO(g) + NO2(g) Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. (a) adding more N2O3(g) (b) adding more NO2(g) (c) increasing the volume of the reaction flask (d) lowering the temperature