Chemistry · Structure 1: Models of the particulate nature of matter. The idea in plain words, the rules to remember, the mistake to avoid and a worked example, written and checked by Mega Lecture.
Atoms are too small to count, so chemists count them in moles. One mole of any substance contains 6.02 × 1023 particles (the Avogadro constant, L). The molar mass M is the mass of one mole in g mol−1; its number is the same as the relative formula mass, found by adding the relative atomic masses in the formula.
The amount in moles links mass, number of particles, concentration of a solution and volume of a gas. Most problems are solved by changing what you are given into moles first.
The empirical formula is the simplest whole-number ratio of atoms in a compound. The molecular formula is a whole-number multiple of it.
Leaving the volume in cm3 when using c = n ÷ V. Divide cm3 by 1000 to get dm3 first.
Answer: C2H6O
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