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Straighterline Chemistry Final- deck 5| Questions Answered 100% Correct/Verified Solutions

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Straighterline Chemistry Final- deck 5|
Questions Answered 100%
Correct/Verified Solutions

Acetic acid is a very important industrial chemical and is produced by this reaction:


CH3OH(l) + CO(g) à CH3COOH(l)



Calculate the value of the standard Gibbs Free Energy change for this reaction. Is acetic acid
thermodynamically stable compared with liquid water at standard conditions? Explain.


Compound


Standard Gibbs Free Energy (kJ/mol)


H2O (l)

, -237.1


CH3COOH


-389.9


CH3OH (I)


-166.6


CO (g)


-137.3



A. ΔG°rxn = -86.0 kJ; At standard conditions, acetic acid is less thermodynamically stable than
water because it has a more negative value of ΔG°.



B. ΔG°rxn = -86.0 kJ; At standard conditions, acetic acid is more thermodynamically stable
than water because it has a more negative value of ΔG°.



C. ΔG°rxn = +86.0 kJ; At standard conditions, acetic acid is less thermodynamically stable
than water because it has a more negative value of ΔG°.



D. . ΔG°rxn = -0.017 kJ; At standard conditions, acetic - ANSWER A. ΔG°rxn = -86.0 kJ; At
standard conditions, acetic acid is less thermodynamically stable than water because it has
a more negative value of ΔG°.

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