Question

Consider the thermochemical equation for the combustion of acetone (c3h6o), the main ingredient in nail polish remover. c3h6o (l) + 4 o2 (g) à 3 co2 (g) + 3 h2o (g) ∆horxn = -1790 kj if a bottle of nail polish remover contains 177 ml of acetone, how much heat is released by its complete combustion? the density of acetone is 0.788 g/ml.

Answer 1

Answer:

-4.278 ×10³  kJ

Explanation:

The equation of the reaction is as follows:

$C_3H_6O_{(l)} + 4O_2_{(g)} ------> 3CO_{2(g)}+3H_2O_{(g)}$

The volume of acetone = 177mL

the density of acetone = 0.788 g/mL

Now;

To determine the mass of acetone ; we use the relation

$density = \frac {mass}{volume}$

mass = density × volume

mass = 177 mL × 0.788 g/mL

mass = 1.39 × 10² g

Since number of moles = $\frac{mass}{molar \ mass}$

number of moles of acetone = $\frac{1.39*10^2}{58.08 \ g/mol}$

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:

$2.39 * \frac{-1790 \ kJ}{1 mol}$

= -4278.1 J

= -4.278 ×10³  kJ