Carbon dioxide is a green house gas that is linked to global warming. it is released into the atmosphere through the combustion of octane (c8h18) in gasoline. write the balanced chemical equation for the combustion of octane. (use the lowest possible whole number coefficients. omit states-of-matter from your answer.)
calculate the mass of octane needed to release 3.50 mol co2.

The equation for combustion of octane is given below. The mass of octane needed is 49.87 g.

Explanation:

Combustion reaction is a type of reaction in which a hydrocarbon in the presence of air (oxygen) decomposes into carbon dioxide and water.

Chemical equation for the combustion of octane is given by:

As, oxygen is taken in excess. Therefore, octane is considered as limiting reagent because it limits the formation of product.

By Stoichiometry,

16 moles of carbon dioxide is produced by 2 moles of octane.

So, 3.5 moles of carbon dioxide is produced by = of octane.

To calculate the mass of octane needed, we use the formula:

Molar mass of octane = 114 g/mol

Number of moles of octane = 0.4375

Putting values in above equation, we get:

Mass of octane needed = 49.87 g

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.