The equilibrium constant for the dissociation of acetic acid at 25°C is 1.80 x 10-5. If you add0.100 mol of undissociated HAC and 0.500 mol of NaAc to 1.00 L of dissociated water ([H+]=[OH-] = 1.00 x 10-7), in which direction will the acetic acid reaction proceed spontaneously?

Given that- At 250 C the equilibrium constant of acetic acid (HAc) is, Keq=1.80 x 10-5 The…

Answered: The equilibrium constant for the…

Introduction to Chemical Engineering Thermodynamics

8th Edition

ISBN:9781259696527

Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart

Chapter1: Introduction

Section: Chapter Questions

Problem 1.1P

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Answer only no. 3
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2) Is it possible to have a reaction where Kc = Kp? If so, under what conditions would this relationship hold? a) No b) Yes, if the pressure is constant c) Yes, if the number of moles of gaseous product = number of moles of gaseous reactant d) Yes, under all conditions
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Write out the gibbs phase rule equation & calculate the degrees of freedom. Air (02 & N2) w/ water vapor, in equilibrium w/ a container that holds liquid water and solid water (Ice) & no reactions Ethanol & acetic acid to form ethyl acetate & water. Reaction occurs in the liquid phase, but both liquid & vapor are present.
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The equilibrium constant for the dissociation of acetic acid at 25°C is 1.80 x 10-5. If you add 0.100 mol of undissociated HAC and 0.500 mol of NaAc to 1.00 L of dissociated water ([H*]= [OH-] = 1.00 x 10-7), in which direction will the acetic acid reaction proceed spontaneously?