To calculate the Gibbs free energy change (ΔG) for a reaction, we need to know the standard Gibbs free energy change (ΔG°) and the reaction quotient (Q). The equation relating ΔG, ΔG°, and Q is as follows:
ΔG = ΔG° + RT ln(Q)
First, let's consider the reaction: CH3CH2OH + H2O → CH3COOH + 4H(+) + 4e-
The standard Gibbs free energy change (ΔG°) for this reaction can be obtained from thermodynamic data. However, since the specific values were not provided, I will use estimated values from a database.
Assuming standard conditions (25°C and 1 atm), the estimated ΔG° for the reaction is approximately -188 kJ/mol.
To calculate ΔG, we need to know the reaction quotient (Q), which is the ratio of the concentrations of products to reactants at a given point during the reaction.
For the given reaction, the reaction quotient (Q) can be expressed as:
Q = [CH3COOH][H+]^4 / [CH3CH2OH][H2O]
Note that the concentration of electrons (e-) does not appear in the expression for Q because it is treated as a standard state species.
To obtain the ΔG for the reaction, the values of Q and ΔG° would need to be known at a specific point in the reaction, along with the gas constant (R = 8.314 J/(mol·K)) and the temperature (T) in Kelvin.
Regarding the ethanol acid hydrolysis with an oxidizing agent (K2Cr2O7), more specific information is needed to calculate the Gibbs free energy change. The reaction conditions, concentrations, and other relevant data are required for an accurate calculation.