Calculate the free-energy change at 25度 of burning 2.30 g O2 as the following reaction: CH4(g)+2O2(g)→CO2(g)+2H2O(g)

To calculate the free-energy change (ΔG) at 25°C for the combustion of CH4(g) with 2.30 g O2(g), we need to know the standard free-energy changes (ΔG°) for the reactants and products at 25°C.

The standard free-energy change of a reaction can be calculated using the following equation:

ΔG° = ΔG°(products) - ΔG°(reactants)

For the reaction CH4(g) + 2O2(g) → CO2(g) + 2H2O(g), we need the ΔG° values for CH4, O2, CO2, and H2O.

These values can typically be found in a thermodynamic data table in a chemistry textbook or online.

Once we have these values, we can plug them into the equation to find ΔG° for the reaction.

However, the question asks for the free-energy change for burning 2.30 g O2, not for the reaction as written.

To find this, we need to convert the mass of O2 to moles using its molar mass (32.00 g/mol), and then use the stoichiometry of the reaction to find the moles of CH4 that react with this amount of O2.

Finally, we multiply the ΔG° for the reaction by the moles of CH4 to find the total ΔG for burning 2.30 g O2.

Please note that without the specific ΔG° values for the substances involved, I can't provide a numerical answer.