Question 4A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide, SO3, from sulfur dioxide, SO, and oxygen,0, shown here. At high temperatures, the rate of formation of SO, is higher, but the equilibrium amount (concentration or partialpressure) of SO, is lower than it would be at lower temperatures. The balanced reaction equation is 2S0, (g) +0,(g) → 2SO,(g)What does the equilibrium constant for this reaction do as the temperature increases?A Remains the sameIncreasesDecreasesResetsQuestion 5For a precipitation reaction to be useful in a gravimetric analysis, the product of the reaction must be insoluble.TrueB) FalseQuestion 6Analysis of the gases in a sealed reaction vessel containing NH3, N2, and H2 at equilibrium at 400° C established the concentrationof N2 to be 1.2 M and the concentration of H, to be 0.24 M.N,(g) + 3H,(g) =2NH,(g)K¸=0.50 at 400° C_ What is the equilibrium molar concentration of NH, ?A0.091B) 0.00910.00830.24

Equilibrium constant of an equilibrium reaction is given by aA + bB ↔cC +dDKeq = [C]c[D]d[A]a[B]b

A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide, SO3, from sulfur dioxide, SO, and oxygen, 02, shown here. At high temperatures, the rate of formation of SO, is higher, but the equilibrium amount (concentration or partial pressure) of SO, is lower than it would be at lower temperatures. The balanced reaction equation is 2SO,(g) + O,(g) → 250,(g) . What does the equilibrium constant for this reaction do as the temperature increases? A Remains the same B Increases Decreases Resets

A necessary step in the manufacture of sulfuric acid is the formation of sulfur trioxide, SO3, from sulfur dioxide, SO, and oxygen, 02, shown here. At high temperatures, the rate of formation of SO, is higher, but the equilibrium amount (concentration or partial pressure) of SO, is lower than it would be at lower temperatures. The balanced reaction equation is 2SO,(g) + O,(g) → 250,(g) . What does the equilibrium constant for this reaction do as the temperature increases? A Remains the same B Increases Decreases Resets

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 12.41PAE: Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go...

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For the reaction A2 + 2B 2AB, diagram I depicts an initial reaction mixture, where A2 molecules are red and B atoms are green. Which of the diagrams II through IV is a possible equilibrium state for the reaction system? There may be more than one correct answer.
For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.
For the reaction A2 + B2 2AB, diagram I depicts an initial reaction mixture, where A2 molecules are red and B2 molecules are green. Which of the diagrams II through IV is a possible equilibrium state for the reaction system? There may be more than one correct answer.
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?
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.
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For the reaction NH3(g)+H2S(g)NH4HS(s) K = 400. at 35.0C. If 2.00 moles each of NH3, H2S, and NH4HS are placed in a 5.00-L vessel, what mass of NH4HS will be present at equilibrium? What is the pressure of H2S at equilibrium?
A mixture of N2, H2, and NH3 is at equilibrium [according to the equationN2(g)+3H2(g)2NH3(g)] as depicted below: The volume is suddenly decreased (by increasing the external pressure) and a new equilibrium is established as depicted below: a. If the volume of the final equilibrium mixture is 1.00 L, determine the value of the equilibrium constant, K. for the reaction. Assume temperature is constant. b. Determine the volume of the initial equilibrium mixture assuming a final equilibrium volume of 1.00 L and assuming a constant temperature.
Heating a metal carbonate leads to decomposition. BaCO3(s) BaO(s) + CO2(g) Predict the effect on the equilibrium of each change listed below. Answer by choosing (i) no change, (ii) shifts left or (iii) shifts right. (a) add BaCO3 (b) add CO2 (c) add BaO (d) raise the temperature (e) increase the volume of the flask containing the reaction