Answer:
1383.34 kJ/mol is the energy released on combustion of the organic compound.
Explanation:
Mass of an organic compound = 0.6654 g
Molar mass of organic compound = 46.07 g/mol
Moles of an organic compound = [tex]\frac{0.6654 g}{46.07 g/mol}=0.01444 mol[/tex]
Let heat evolved during burning of 0.6654 grams of an organic compound be -Q.
Heat absorbed by calorimeter = Q' = -Q
The total heat capacity of the calorimeter all its contents = C
C = 3576 J/°C
Change in temperature of the calorimeter =
ΔT = 30.589°C - 25.000°C = 5.589°C
[tex]Q'=C\times \Delta T[/tex]
[tex]Q'=3576 J/^oC\times 5.589^oC=19,975.536 J=19.975 kJ[/tex]
Q' = 19.975 kJ
Q = -19.975 kJ (negative sign; energy released)
0.01444 moles of an organic compound gives 19.975 kilo Joule.
The 1 mole of an organic compound will give : [tex]\Delta H_{comb}[/tex]
[tex]\Delta H_{comb}=\frac{-19.975 kilo Joule}{0.01444 mol}[/tex]
[tex]=-1383.34 kJ/mol[/tex]
