Answer:
-4.278 ×10³ kJ
Explanation:
The equation of the reaction is as follows:
[tex]C_3H_6O_{(l)} + 4O_2_{(g)} ------> 3CO_{2(g)}+3H_2O_{(g)}[/tex]
The volume of acetone = 177mL
the density of acetone = 0.788 g/mL
Now;
To determine the mass of acetone ; we use the relation
[tex]density = \frac {mass}{volume}[/tex]
mass = density × volume
mass = 177 mL × 0.788 g/mL
mass = 1.39 × 10² g
Since number of moles = [tex]\frac{mass}{molar \ mass}[/tex]
number of moles of acetone = [tex]\frac{1.39*10^2}{58.08 \ g/mol}[/tex]
number of moles of acetone = 2.39 moles
Given that -1790 kJ of heat is released for one mole of combustion of acetone. To calculate the amount of heat released with 2.39 moles of acetone; we have:
[tex]2.39 * \frac{-1790 \ kJ}{1 mol}[/tex]
= -4278.1 J
= -4.278 ×10³ kJ
