Problem: Methanol, a major industrial feedstock, is made by several catalyzed reaction, such as CO(g) + 2H2(g) ⟶ CH3OH(l).(c) One concern about using CH 3OH as an auto fuel is its oxidation in air to yield formaldehyde, CH2O(g), which poses a health hazard. Calculate ΔG° at 100.°C for this oxidation.

FREE Expert Solution

Step 1:


H°rxn =H°f, products - H°f, reactantsH°rxn =[1 mol(-238.6 kJmol)] - [1 mol(-110.5 kJmol)+0]H°rxn =-238.6 kJ + 110.5 kJ

ΔH°rxn = -128.1 kJ


Step 2:


S°rxn =S°products - S°reactantsS°rxn =[1 mol(126.8 Jmol·k)]                     - [1 mol(197.7 Jmol·k)+2 mol(130.7 Jmol·k)]S°rxn =126.8 J - 459.1 JS°rxn = - 332.3 J×1 kJ103 J

ΔS°rxn = - 0.3323 kJ


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Problem Details

Methanol, a major industrial feedstock, is made by several catalyzed reaction, such as CO(g) + 2H2(g) ⟶ CH3OH(l).

(c) One concern about using CH 3OH as an auto fuel is its oxidation in air to yield formaldehyde, CH2O(g), which poses a health hazard. Calculate ΔG° at 100.°C for this oxidation.

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