An equilibrium involving the carbonate and bicarbonate ions exist in natural waters.HCO3-(aq) -> H+(ag) + CO32-(aq)Assuming that the reactions in both directions are elementary processes, do the following write rate expressions for the forward and reverse reactions. Show all your work to receive full credit.1. An equilibrium involving the carbonate and bicarbonate ions exists in natural waters.HCO3 (a9) = H†(ag) + CO3²¯(ag)Assuming that the reactions in both directions are elementary processes, do the following.(a)Write rate expressions for the forward and reverse reactions.Forward rate = k+1%3DReverse rate = k-1(b)(b) Write an expression for the equilibrium constant based on the rates of the forward and reversereactions.

For elementary reactions, order of the reactants is equal to their respective stoichiometric…

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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An equilibrium involving the carbonate and bicarbonate ions exist in natural waters.

HCO3-(aq) -> H+(ag) + CO32-(aq)

Assuming that the reactions in both directions are elementary processes, do the following write rate expressions for the forward and reverse reactions.

Show all your work to receive full credit.
1. An equilibrium involving the carbonate and bicarbonate ions exists in natural waters.
HCO3 (a9) = H†(ag) + CO3²¯(ag)
Assuming that the reactions in both directions are elementary processes, do the following.
(a)
Write rate expressions for the forward and reverse reactions.
Forward rate = k+1
%3D
Reverse rate = k-1
(b)
(b) Write an expression for the equilibrium constant based on the rates of the forward and reverse
reactions.

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