In one of the oldest examples of chemical warfare on the planet, yeast produces

Question

In one of the oldest examples of chemical warfare on the planet, yeast produces ethanol and carbon dioxide when fermenting glucose. C_6H_12O_6 rightarrow 2 C_2 H_6 O(l) + 2 CO_2(g) a) Using the following data, calculate Delta_rxn H degree Delta_rxn S and Delta G degree for this reaction at 25 degree C. b) Does this reaction favor reactants or products? c) What does your answer in Part b) tell you about the relative size of the equilibrium constant for this reaction? (Will K_eq greater than 1, less than 1, or equal to 1 ?)

Explanation / Answer

a)

Horxn = 2*Hof(C2H6O) + 2*Hof(CO2) - Hof(C6H12O6)

Horxn = 2*(-277.0) + 2*(-393.509) - (-1269.0)

Horxn = - 72.018 KJ/mole

Sorxn = 2*Sof(C2H6O) + 2*Sof(CO2) - Sof(C6H12O6)

Sorxn = 2*(160.7) + 2*(213.74) - (289)

Sorxn = - 459.88 J/k.mole

Gorxn = 2*Gof(C2H6O) + 2*Gof(CO2) - Gof(C6H12O6)

Gorxn = 2*(-174.7) + 2*(-394.359) - (-918.8)

Gorxn = - 219.318 KJ/mole

b)

since Gorxn is negative, the reaction favours the product

c)

since Gorxn is negative, Keq will be greater than 1

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