# Problem: Consider two reactions for the production of ethanol:C2H4 (g) + H2O (g) → CH3CH2OH (l)C2H6 (g) + H2O (g) → CH3CH2OH (l) + H2 (g)Which would be the more thermodynamically feasible at standard conditions? Why?

###### FREE Expert Solution

We are asked which would be the more thermodynamically feasible at standard conditions among the two reactions for the production of ethanol.

C2H4 (g) + H2O (g) → CH3CH2OH (l)
C2H6 (g) + H2O (g) → CH3CH2OH (l) + H2 (g)

Calculate the ΔG:

C2H4 (g) + H2O (g) → CH3CH2OH (l)

Given:

ΔG f ° for C2H4 (g) =  +68.4 kJ/mol

ΔG f ° for H2O (g) = -228.5 kJ/mol

ΔG f ° for CH3CH2OH (l) = -172.8 kJ/mol

ΔG˚rxn = -12.7 kJ

96% (340 ratings) ###### Problem Details

Consider two reactions for the production of ethanol:

C2H4 (g) + H2O (g) → CH3CH2OH (l)
C2H6 (g) + H2O (g) → CH3CH2OH (l) + H2 (g)

Which would be the more thermodynamically feasible at standard conditions? Why?

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.