Calculate deltaG from deltaH and deltaS. Use the table of standard thermodynamic data. calculate deltaG at 0 degrees C for CH3CH2CH3 + 5O2 --> 3CO2 + H2O.
CH3CH2CH3 + 5O2 --> 3CO2 + 4H2O
I've balanced the equation so far, I know that deltaG = delatH - T(deltaS) but my notes are a bit confusing when describing how to solve for deltaG.
Nevermind, I figured it out. :)
To calculate the change in Gibbs free energy (ΔG) using the equation ΔG = ΔH - TΔS, you need to know the values of ΔH (change in enthalpy) and ΔS (change in entropy) for the reaction of interest. In this case, you would like to calculate ΔG at 0 degrees Celsius for the reaction:
CH3CH2CH3 + 5O2 -> 3CO2 + 4H2O
1. Firstly, you need to find the respective values for ΔH and ΔS for each component in the reaction.
- Look up the standard enthalpy change (ΔH°) for each reactant and product involved in the reaction. Standard thermodynamic data for many compounds can be found in tables or online databases.
- Additionally, find the standard entropy change (ΔS°) for each compound.
2. Once you have gathered the required data, calculate the change in enthalpy (ΔH) for the overall reaction. This can be done by summing up the products' enthalpies and subtracting the reactants' enthalpies:
ΔH = ΣH(products) - ΣH(reactants)
3. Next, calculate the change in entropy (ΔS) for the reaction using the same approach:
ΔS = ΣS(products) - ΣS(reactants)
4. Finally, substitute the values of ΔH and ΔS into the equation ΔG = ΔH - TΔS. Be sure to convert temperature to Kelvin (0 degrees Celsius = 273 K) before calculating:
ΔG = ΔH - TΔS
By following these steps and substituting the given values, you can calculate the change in Gibbs free energy (ΔG) for the reaction at 0 degrees Celsius.