the process of respiration, glucose is oxidized completely. In fermentation, O2 is absent, and glucose is broken down into Co2 and H2o.
Calculate delta g for respiration of 1.00 g of glucose
Calculate delta g for fermentation of 1.00 g of glucose.
My answers:
-16.0 kJ and -1.26 kJ
what I need help with is:
Calculate delta g for oxidation of the ethanol from part C.
answer in kJ/g..............thanks!
To calculate ΔG (change in Gibbs free energy) for the oxidation of ethanol, we first need to know the chemical equation for the oxidation reaction. Since fermentation produces CO2 and H2O from glucose, we can assume that the ethanol is further oxidized to produce CO2.
The equation for the combustion of ethanol is as follows:
C2H5OH + 3O2 -> 2CO2 + 3H2O
To calculate ΔG, we need to know the standard Gibbs free energy change (ΔG°) for the reaction. Here are the values for ΔG° for the given compounds involved:
ΔG°f(C2H5OH) = -174.8 kJ/mol
ΔG°f(CO2) = -394.4 kJ/mol
ΔG°f(H2O) = -237.1 kJ/mol
Now, let's calculate ΔG for the oxidation of ethanol:
Reactant side:
1 mole of C2H5OH
Product side:
2 moles of CO2 + 3 moles of H2O
We can calculate ΔG using the formula:
ΔG = ΔG° (products) - ΔG° (reactants)
ΔG = [2 × ΔG°f(CO2) + 3 × ΔG°f(H2O)] - [ΔG°f(C2H5OH)]
Substituting the values, we get:
ΔG = [2 × (-394.4 kJ/mol) + 3 × (-237.1 kJ/mol)] - (-174.8 kJ/mol)
ΔG = -922.8 kJ/mol + -711.3 kJ/mol + 174.8 kJ/mol
ΔG = -1459.3 kJ/mol
Finally, to determine ΔG per gram of ethanol, we need to divide by the molar mass (46.07 g/mol) of ethanol:
ΔG per gram = ΔG / gram
ΔG per gram = (-1459.3 kJ/mol) / (46.07 g/mol)
ΔG per gram = -31.7 kJ/g (rounded to one decimal place)
Therefore, the ΔG for the oxidation of ethanol is approximately -31.7 kJ/g.