From combustion analysis, a 100.0 g sample of a compound that consists of C, H, and O was found to contain 70.6 g C (from CO2) and 5.92 g H (from H2O). What is the empirical formula for this compound?

The empirical formula for the given compound is

Explanation:

The chemical equation for the combustion of hydrocarbon having carbon, hydrogen and oxygen follows:

where, 'x', 'y' and 'z' are the subscripts of Carbon, hydrogen and oxygen respectively.

We are given:

Mass of

Mass of

We know that:

Molar mass of carbon dioxide = 44 g/mol

Molar mass of water = 18 g/mol

For calculating the mass of carbon:

In 44 g of carbon dioxide, 12 g of carbon is contained.

So, in 70.6 g of carbon dioxide, of carbon will be contained.

For calculating the mass of hydrogen:

In 18 g of water, 2 g of hydrogen is contained.

So, in 5.92 g of water, of hydrogen will be contained.

Mass of oxygen in the compound = (100.0) - (19.25 + 0.658) = 80.092 g

To formulate the empirical formula, we need to follow some steps:

Moles of Carbon =

Moles of Hydrogen =

Moles of Oxygen =

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.658 moles.

For Carbon =

For Hydrogen =

For Oxygen =

The ratio of C : H : O = 2 : 1 : 8

Hence, the empirical formula for the given compound is

in chemistry, adhesion and cohesion are attractive forces that exist between molecules. they hold the molecules together from each other. they are different in that adhesive force exists between molecules of different substance while cohesive force happens between molecules of same substance.

adhesion between water and glass causes water molecules at the edge of water and glass interface to climb up the wall in a narrow glass tube. this is called capillary action. cohesion is what gives glass its shape and causes water to form a droplet.