PCI3(g) + Cl2(g) PCI5(g) + Heat Fill in the table below by indicating what direction the equilibrium will shift when the changes indicated are made, and the shift will have on each species in the reaction mixture. You may use left and right arrows for the shift, and up and down arrows to indicate concentration changes. Indicate no change by writing NC. Stress Eq Shift PCI3 conc. Cl2 Conc. PCI5 conc. Addition of Cl2 Removal of PCI5 Increase in Temperature Addition of a Catalyst

PCI3(g) + Cl2(g) PCI5(g) + Heat Fill in the table below by indicating what direction the equilibrium will shift when the changes indicated are made, and the shift will have on each species in the reaction mixture. You may use left and right arrows for the shift, and up and down arrows to indicate concentration changes. Indicate no change by writing NC. Stress Eq Shift PCI3 conc. Cl2 Conc. PCI5 conc. Addition of Cl2 Removal of PCI5 Increase in Temperature Addition of a Catalyst

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 13QAP: Consider the following reaction at 250C: A(s)+2B(g)C(s)+2D(g) (a) Write an equilibrium constant...

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Consider the following reaction at 250C: A(s)+2B(g)C(s)+2D(g) (a) Write an equilibrium constant expression for the reaction. Call the equilibrium constant K1. (b) Write an equilibrium constant expression for the formation of one mole of B(g) and call the equilibrium constant K2. (c) Relate K1 and K2.
Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?
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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?
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