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

the answer is a. co2, this would be colder than the : )

explanation: