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

-4.278 ×10³ kJ

Step-by-step 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 =
`(mass)/(molar \ mass)`

number of moles of acetone =
`(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 * (-1790 \ kJ)/(1 mol)`

= -4278.1 J

= -4.278 ×10³ kJ