It has been proposed that wood alcohol, CH3OH, a relatively inexpensive fuel to produce, be decomposed to produce methane. Methane is a natural gas, commonly used for heating homes. is a decomposition from wood alcohol to methane and oxygen thermodynamically feasible at 25 degrees celsius and 1 atm.

Look in your text for Go, then

delta Go(rxn) = delta Go(products) - delta Go(reactants). + not sponeaneous, - is spontaneous.

To determine the thermodynamic feasibility of decomposing wood alcohol (CH3OH) into methane (CH4) and oxygen (O2) at 25 degrees Celsius and 1 atm, we need to calculate the change in Gibbs free energy (ΔG) for the reaction. The Gibbs free energy change can be determined using the Gibbs-Helmholtz equation:

ΔG = ΔH - TΔS

where ΔH is the enthalpy change of the reaction, ΔS is the entropy change of the reaction, and T is the temperature.

First, we need to know the standard enthalpy change (ΔH°) and the standard entropy change (ΔS°) for the reaction. Let's assume that the ΔH° and ΔS° values are known.

Next, we calculate the ΔG° (standard Gibbs free energy change) using the given equation:

ΔG° = ΔH° - TΔS°

Substituting the known values and converting the temperature to Kelvin (25°C = 298 K), we can calculate the ΔG°.

Now, to determine whether the decomposition reaction is thermodynamically feasible at 25 degrees Celsius and 1 atm, we compare the ΔG° value to zero. If ΔG° is negative, the reaction is thermodynamically feasible. If ΔG° is positive, the reaction is not thermodynamically feasible.

Keep in mind that this calculation assumes standard conditions (1 atm pressure, 298 K temperature) and does not take into account any kinetic factors that may affect the reaction rate.