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 the delta G for oxidation of ethanol, we need to first understand the process of oxidation. In fermentation, glucose is broken down into ethanol (C2H5OH) and carbon dioxide (CO2). Oxidation of ethanol further breaks it down into carbon dioxide and water. The balanced equation for the oxidation of ethanol is as follows:
C2H5OH + O2 → CO2 + H2O
Now, to calculate the delta G for this reaction, we need to know the standard Gibbs free energy change (delta G°) for the reaction. However, since you haven't provided any values for delta G°, we cannot directly calculate the delta G for oxidation of ethanol.
Delta G is dependent on temperature and pressure, so we also need to know the conditions under which the reaction is taking place. Based on the information provided, we don't have enough data to calculate the delta G for the oxidation of ethanol.
If you have the necessary delta G° values or additional information, please provide them, and I'll be happy to help you calculate the delta G for the oxidation of ethanol.
To calculate the ΔG for the oxidation of ethanol, we first need to determine the balanced chemical equation for the reaction. The oxidation of ethanol (C2H5OH) can be represented as:
C2H5OH + O2 → CO2 + H2O
Next, we need to find the ΔG°f values (standard Gibbs free energy of formation) for each compound involved in the reaction. These values can be obtained from reference tables or online sources. Let's assume the following ΔG°f values:
ΔG°f (C2H5OH) = -174.8 kJ/mol (ethanol)
ΔG°f (CO2) = -394.4 kJ/mol
ΔG°f (H2O) = -237.13 kJ/mol
We also need to consider the stoichiometric coefficients in the reaction:
C2H5OH:CO2:H2O = 1:2:3
Now, we can calculate the ΔG for the oxidation of ethanol using the equation:
ΔG = Σ(ΔG°f products) - Σ(ΔG°f reactants)
ΔG = (2 × ΔG°f (CO2)) + (3 × ΔG°f (H2O)) - (ΔG°f (C2H5OH))
ΔG = (2 × -394.4) + (3 × -237.13) - (-174.8)
ΔG = -788.8 - 711.39 + 174.8
ΔG = -1,325.39 kJ/mol
To calculate ΔG in kJ/g, we need to convert the ΔG value to kJ/g by dividing by the molar mass of ethanol. The molar mass of ethanol (C2H5OH) is approximately 46.07 g/mol.
ΔG (kj/g) = -1,325.39 kJ/mol / 46.07 g/mol
ΔG (kj/g) ≈ -28.73 kJ/g
Therefore, the ΔG for the oxidation of ethanol is approximately -28.73 kJ/g.