6 At 298K, the equilibrium constant for the following reaction is 4.20×10-7:H2CO3(aq) + H2O=H30*(aq) + HCO3"(aq)The equilibrium constant for a second reaction is 4.80x10-11:HCO3 (aq) + H2O= H30*(aq) + CO3²-(aq)Use this information to determine the equilibrium constant for the reaction:H2CO3(aq) + 2H20= 2H30*(aq) + CO32-(aq)K =

Required equation: H2CO3(aq) + 2H2O <-------> 2H3O+ + CO3 2-(aq) Rate constant=?

At 298K, the equilibrium constant for the following reaction is 4.20x10-7: H2CO3(aq) + H2O= H30*(aq) + HCO3"(aq) The equilibrium constant for a second reaction is 4.80x10-11: HCO3 (aq) + H20= H30*(aq) + CO32-(aq) Use this information to determine the equilibrium constant for the reaction: H2CO3(aq) + 2H20= 2H30*(aq) + CO32-(aq) K =

At 298K, the equilibrium constant for the following reaction is 4.20x10-7: H2CO3(aq) + H2O= H30(aq) + HCO3"(aq) The equilibrium constant for a second reaction is 4.80x10-11: HCO3 (aq) + H20= H30(aq) + CO32-(aq) Use this information to determine the equilibrium constant for the reaction: H2CO3(aq) + 2H20= 2H30*(aq) + CO32-(aq) K =

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 7QRT

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