Answer to Question #152949 in General Chemistry for Aziz Fatih

Question

Butane C4H10(l) boils at -0.5°C; 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). (ΔHf

o

H2O(g) =

–285.83 kJ/mol, ΔHf

o

CO2(g) = –393.5 kJ/mol, ΔHf

o

C4H10(g) = –124.7 kJ/mol,

ΔHvapo

C4H10 = 22.44 kJ/mol, C4H10 =58.12 g/mol).

(Hint: Write the balanced combustion reaction of C4H10(l).)

Answer 1

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