Question

In a constant

Answer 1

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 = $\frac{0.6654 g}{46.07 g/mol}=0.01444 mol$

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

$Q'=C\times \Delta T$

$Q'=3576 J/^oC\times 5.589^oC=19,975.536 J=19.975 kJ$

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 : $\Delta H_{comb}$

$\Delta H_{comb}=\frac{-19.975 kilo Joule}{0.01444 mol}$

$=-1383.34 kJ/mol$