# Chapter 11 Empirical and Molecular Formulas

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Chapter 11 Empirical and Molecular Formulas
Chemistry Chapter 11 Empirical and Molecular Formulas

Empirical Formulas The simplest whole number ratio of the elements in a compound (not necessarily the actual formula for a compound) Ex H2O2 = HO H2O= H2O C6H12 = CH2 C8H16 = CH2 Can be calculated from % composition

Empirical Formula (Cheat Sheet)
1. % composition (if = 100%) converts to mass Convert from mass to moles Calculate simplest ratio (divide all # mol by the smallest # moles) 3 ½. If not all whole numbers, multiply all by a whole # to create whole #’s 4. Use simplest ratio as subscripts

Examples 11.2 % Hydrogen and 88.8% Oxygen

Examples 36.84% N and 63.16% O

Examples 60% C, 4.44%H, and 35.56% Oxygen

Molecular Formula Actual number of moles of each element in a compound
Need more info than just % comp Need molar mass of the empirical formula Need an experimental mass of the actual compound

Molecular Formula (Cheat Sheet)
Use steps to calculate empirical formula Calculate molar mass of empirical formula The question will give you experimental mass of the compound Experimental mass Empirical form. Molar mass = 5. Multiply subscripts in empirical by your answer (whole number)

Example A colorless liquid is found to be composed of 46.68% N and 53.32% O and has a molar mass of g/mol. What is the molecular formula?