Be sure to answer all parts. methanol, a major industrial feedstock, is made by several catalyzed reactions, such as co (g) + 2h2 (g) → ch3oh (l) one concern about using ch3oh as an auto fuel is its oxidation in air to yield formaldehyde, ch2o (g), which poses a health hazard. calculate δg o at 230°c for this oxidation.

Given data,

Temperature, T = 230°C = 503 K

Consider the chemical reaction,

CH₃OH (l) + 1/2 O₂ (g) → CH₂O (g) + H₂O (l)

Calculate the enthalpy change for the reaction:

ΔH⁰rxn = ΣnΔH⁰f (products) - ΣmΔH⁰f (reactants)

Substitute the values from the table:

ΔH⁰rxn = { - 115.9 + (-285.8) } - {0 + (-238.7) }

= - 163.0 kJ

Calculate the entropy change for the reaction.

ΔS⁰rxn = (219 + 70) - (127.2 + 1/2 x 205.2) = 59.2 J/K

Consider the expression for free energy:

ΔG⁰rxn = ΔH⁰rxn - T ΔS⁰rxn

Substitute the values in the above equation

ΔG⁰rxn = - 163 x 10³ - (503 x 59.2)

= - 192777.6 J

= - 192.777 kJ