Industrial production of ethanol requires fermentation using Saccbaromyces cere-

Question

Industrial production of ethanol requires fermentation using Saccbaromyces cere-visiae, a type of yeast. The elemental formula of S. cerevisiae is CH_1.83O0.56N_0.56 Suppose you want to produce ethanol (C_2H_6O) in a batch process at 25degreeC. You plan to add 0.25 lb_m NH_3 and 5.0 lb_m glucose to the yeast for the following (unbalanced) reaction: Note that I mol glucose produces 0.5 mol glycerol and that the ratio of NH_3 to H_20 is 1:1. During preparation, you accidentally add too much glucose. However, you decide to let the bioreactor run anyway. After the reaction goes to completion (at least one of the starting reactants is used up), you discover that 1.4 lbm ethanol had been produced. How much heat had been produced and subsequently removed from the system? How much glucose did you initially

Explanation / Answer

Delta H of reaction = Sum of delta H of formation of products - Sum of delta H of formation of reactants

Delat H of reaction = [delta HC3H8O3 + delta HC2H6O + delta HCO2 + delta HH2O - [delta HC6H12O6 + delta HNH3]

Delta H of reaction = [-669.6 - 277.63 - 393.51 - 285.84] - [ -1274 - 46.191]

Delta H of reaction = -1626.58 + 1320.19 = -306.39 KJ / mole

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