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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Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter18: Chemical Equilibrium

Section: Chapter Questions

Problem 14E

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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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