The following molar enthalpies of formation are given in kJ/mol: Hfo[CH3OH (l)] = –239.2; Hfo[CO2(g)] = –393.5; Hfo[H2O(g)] = –241.8 (a) Calculate the enthalpy change (H; in kJ) for the combustion of methanol, CH3OH, according to the following equation. 2CH3OH (l) + 3 O2(g) 2CO2(g) + 4H2O(g); (b) How many kilojoules of heat is produced burning 1.00 g of methanol? (c) How much energy (in kJ) is required to heat 946 g of water from 21.0oC to 100.0oC? (d) How many grams of methanol must be burned to provide enough energy that is required to heat the water in part (c)? (specific heat of water = 4.184 J/g.oC)
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