Calculate the deltaG0 for the oxidation of ethanol by NAD+. Urgent Thank You
To calculate the standard free energy change (ΔG°) for the oxidation of ethanol by NAD+, you will need to use the relevant thermodynamic data and apply the equation:
ΔG° = ΔG°f(products) - ΔG°f(reactants)
1. First, identify the balanced chemical equation for the oxidation of ethanol by NAD+. The balanced equation is:
Ethanol + NAD+ ⟶ Acetaldehyde + NADH + H+
2. Calculate the ΔG°f (standard free energy change of formation) for each compound involved in the reaction. ΔG°f values can be found in thermodynamic tables. Here are the values for each compound required:
- ΔG°f(ethanol) = -174.8 kJ/mol
- ΔG°f(NAD+) = -268.4 kJ/mol
- ΔG°f(acetaldehyde) = -167.4 kJ/mol
- ΔG°f(NADH) = -87.5 kJ/mol
- ΔG°f(H+) = 0 kJ/mol (since it is an ion)
3. Substitute these values into the equation:
ΔG° = [ΔG°f(acetaldehyde) + ΔG°f(NADH) + ΔG°f(H+)] - [ΔG°f(ethanol) + ΔG°f(NAD+)]
ΔG° = [-167.4 + (-87.5) + 0] - [-174.8 + (-268.4)]
4. Simplify and calculate the value:
ΔG° = -254.9 kJ/mol - (-443.2 kJ/mol)
ΔG° = -254.9 kJ/mol + 443.2 kJ/mol
ΔG° = 188.3 kJ/mol
Therefore, the standard free energy change (ΔG°) for the oxidation of ethanol by NAD+ is 188.3 kJ/mol.