Methanol's combustion enthalpy can be calculated at -540 (kJ mol-1).
Methanol, the most basic form of alcohol (CH3OH), serves as the chemical basis for countless items used in daily life, such as paints, plastics, auto parts, and building supplies. Additionally, methanol is a renewable resource that powers fuel cells, boilers, cook stoves, ships, automobiles, trucks, and buses.
Energy required to dissociate the bonds connecting reactants
3 × 413 + 358 + 464 + 1.5 × 498 (kJ mol-1) / 2808 (kJ mol-1);
Total energy released when products form bonds
4 × 464 + 2 × 746 (kJ mol-1) / 3348 (kJ mol-1);
∆H = -540 (kJ mol-1).
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The complete question is -
Methanol is made in large quantities as it is used in the production of polymers and in fuels.
The enthalpy of combustion of methanol can be determined theoretically or experimentally.
CH₃OH(l) + 1 O₂(g) → CO₂(g) + 2H₂O(g)
Using the information from Table 10 of the Data Booklet, determine the theoretical enthalpy of combustion of methanol.
