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{"ops":[{"insert":"Butane C4H10(l) boils at -0.5\u00b0C; at this temperature it has a density of 0.60 g/cm3. Theenthalpy of vaporization of C4H10(l) is 22.44 kJ/mol. Calculate the enthalpy change when 1 L of liquid C4H10(l) is burned in air to give CO2(g) and H2O(g). (\u0394Hf\no\nH2O(g) =\n\u2013285.83 kJ/mol, \u0394Hf\no\nCO2(g) = \u2013393.5 kJ/mol, \u0394Hf\no\nC4H10(g) = \u2013124.7 kJ/mol,\n\u0394Hvapo\nC4H10 = 22.44 kJ/mol, C4H10 =58.12 g/mol).\n(Hint: Write the balanced combustion reaction of C4H10(l).)\n"}]}
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