A 1.2569 -g sample of a new compound has been analyzed and...

Name: Problem 121, Chapter 8: Introductory Chemistry
Uploaded: 2020-07-01T13:17:36-08:00
Duration: 5 min 50 s
Channel: Temi Ajayi
Description: A 1.2569 -g sample of a new compound has been analyzed and found to contain the following masses of elements: carbon, 0.7238 g; hydrogen, 0.07088 g; nitrogen, 0.1407 g; oxygen, 0.3214 g. Calculate the empirical formula of the compound.

A 1.2569 -g sample of a new compound has been analyzed and found to contain the following masses of elements: carbon, 0.7238 g; hydrogen, 0.07088 g; nitrogen, 0.1407 g; oxygen, 0.3214 g. Calculate the empirical formula of the compound.

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Key Concepts

Conversion of Mass to Moles

This concept involves dividing the mass of an element by its atomic mass to determine the number of moles present. This step is crucial in empirical formula calculations as it provides a standardized measure (moles) that reflects the actual number of atoms, independent of their masses.

Empirical Formula

The empirical formula represents the simplest whole-number ratio of atoms in a compound. It is derived by converting the masses of each element present in the compound to moles, then dividing by the smallest number of moles to obtain the simplest integer ratio, which forms the empirical formula.

Mole Concept

The mole concept is fundamental in chemistry for converting between the mass of a substance and the number of atoms or molecules present. By using the atomic or molar mass of each element, one can convert the measured mass to moles, which allows for a meaningful comparison between different elements in a compound.

Simplification to Whole-Number Ratios

After converting the masses to moles, the resulting mole amounts are divided by the smallest among them to find the simplest ratio. If the ratios are not whole numbers, they may be multiplied by an appropriate factor to convert them to whole numbers, which are then used to write the empirical formula.