Methanol (CH3OH), which is used as a cooking fuel, undergoes combustion to produ

Question

Methanol (CH3OH), which is used as a cooking fuel, undergoes combustion to produce carbon dioxide and water; 2CH3OH(l)+3O2(g)-->2CO2(g)+4H2O(l) delta H = -726kJ. How many kilojoules are released when 75.0 g of mehtanol is burned?

Explanation / Answer

2CH3OH(l)+3O2(g)-->2CO2(g)+4H2O(l) delta H = -726kJ. Dividing both side by 2 CH3OH(l)+3/2 O2(g)-->CO2(g)+2H2O(l) delta H = -363kJ/mol Mole = mass/ molar mass Moles CH3Oh = 75.0g/32g/mol = 2.34 mol of Ch3OH Now 1 mol of CH3OH produces 363 kj So 2.34 mol CH3OH * ( 363 Kj/ 1 mol Ch3OH) 850.78 KJ

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