Calculate the enthalpy change (ΔH) for the combustion of 2 moles of ethanol (C2H5OH) to produce carbon dioxide (CO2) and water (H2O), given the heat of combustion (ΔHcomb) is -1368 kJ/mol.
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The balanced chemical equation for the combustion of ethanol is:
C2H5OH + 3 O2 -> 2 CO2 + 3 H2O
From the balanced equation, we can see that for every 2 moles of ethanol combusted, we produce 2 moles of CO2 and 3 moles of H2O.
Therefore, the enthalpy change (ΔH) for the combustion of 2 moles of ethanol can be calculated as follows:
ΔH = (2 mol CO2 × ΔHcomb) + (3 mol H2O × ΔHcomb)
= (2 mol CO2 × -1368 kJ/mol) + (3 mol H2O × -1368 kJ/mol)
= -2736 kJ - 4104 kJ
= -6840 kJ
Therefore, the enthalpy change (ΔH) for the combustion of 2 moles of ethanol is -6840 kJ.
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