Consider the thermochemical equation for the combustion of acetone (c3h6o), the main ingredient in nail polish remover: c3h6o(l)+4 o2(g)→3 co2(g)+3 h2o(g)δh°rxn=−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.

the energy produced or released = 2.4 X (-1790) = -4296 kJ

Explanation:

In the given question the heat of combustion is given as H°rxn = −1790 kJ

Thus when one mole of acetone undergoes complete combustion, it gives this much of energy.

The volume of acetone present in nail polish remover = 177 mL

The density of acetone = 0.788 g/mL

The mass of acetone present in nail polish remover = density X volume

the mass of acetone = 0.788 X 177 = 139.48 grams

the moles of acetone present =

The energy produced = moles present X enthalpy of reaction

the energy produced or released = 2.4 X (-1790) = -4296 kJ

  the   balanced   equation   for   reaction of   ca metal   with   o2 to   produce   cao   is as below

2 ca+ o2→ 2 cao2

  explanation

the reaction is   balanced     since the   number of atoms   in reactant side is   equal to   number of atoms   in   product side.   for   example   they   are 2   atom of   ca in   reactant   side   and   2   atoms of ca   in   the product side.

  the   process   is a   meet the   requirement   of   redox   reaction because :     calcium   is   oxidized   from   oxidation state 0   to 2+   while   oxygen   is reduced from   oxidation   state   0   to 2-