2C2H2(g) + 3O2(g) 4CO(g) + 2H2O(g)
What is delta G° for this reaction in J/mol?
(T = 298.17 K)
dGorxn = (n*dGo products) - (n*dGo reactants
To determine the standard Gibbs free energy change (ΔG°) for a reaction, you can use the equation:
ΔG° = ΣnΔG°f(products) - ΣnΔG°f(reactants)
Where ΔG°f is the standard molar Gibbs free energy of formation for each compound, and n is the stoichiometric coefficient of each compound in the balanced equation.
First, you need to find the values of ΔG°f for each compound involved in the reaction. These values are typically given in tables or can be looked up.
Assuming you have the values for ΔG°f for CO(g) and H2O(g), you need to subtract the sum of the standard molar Gibbs free energy of formation of the reactants from the sum of the standard molar Gibbs free energy of formation of the products.
ΔG°f(CO(g)) = ? (look up the value in a table)
ΔG°f(H2O(g)) = ? (look up the value in a table)
ΔG° = (4 * ΔG°f(CO(g)) + 2 * ΔG°f(H2O(g))) - (2 * ΔG°f(C2H2(g)) + 3 * ΔG°f(O2(g)))
Substitute the values of the ΔG°f for each compound into the equation and perform the necessary calculations for each term.
Finally, calculate the ΔG° for the reaction. Remember to include the units of J/mol since ΔG° is an energy change per mole.
Note: Make sure that all the ΔG°f values you use are for the same temperature (in this case, 298.17 K) to ensure accuracy.