Question

GASBUGS INC. is actually a division of a much larger alternate, fuel-generating corporation known as BIOFUELS INTERNATIONAL. One thing this company produces is ethanol (C₂H₆O) from an industrial process that uses a type of yeast (Saccharomyces cerevisiae). The elemental formula of S. cerevisiae is CH_1.83 O_0.56 N_0.17and it has a heat of combustion of approximately -21.2 kJ/g. In their batch process, .25lb_mNH₃ and 5.0lb_m glucose are combined with the yeast at 25^oC. After the reaction goes to completion (at least one of the starting reactants is used up), 1. 4 lb_m of ethanol is produced. The unbalanced reaction for this process is:

C₂H₆O (s) + NH₃ (g) → C₃H₈O₃ (l) + C₂H₆O (l) + CH_1.83 O_0.56 N_0.17+ CO₂(g)+ H₂O (l)

Note: 1 mol of glucose produces .5 mole glycerol (C₃H₈O₃₎ and that the ration of NH₃ to H₂O is 1:1.

1. How much excess glucose was being added to the reactor?
2. What is the ideal amount needed?
3. How much heat was produced and subsequently removed from the system?

Answer 1