atomic mass is 35.45 grams. The abbreviated representation of an element or a compound is called chemical formula. then it must be a hydrogen. of two chlorine atoms for every one mercury atom, the likely empirical formula is for every mercury atom we Find: Empirical formula \(= \ce{Fe}_?\ce{O}_?\), \[69.94 \: \text{g} \: \ce{Fe} \nonumber \], \[30.06 \: \text{g} \: \ce{O} \nonumber \], \[69.94 \: \text{g} \: \ce{Fe} \times \dfrac{1 \: \text{mol} \: \ce{Fe}}{55.85 \: \text{g} \: \ce{Fe}} = 1.252 \: \text{mol} \: \ce{Fe} \nonumber \], \[30.06 \: \text{g} \: \ce{O} \times \dfrac{1 \: \text{mol} \: \ce{O}}{16.00 \: \text{g} \: \ce{O}} = 1.879 \: \text{mol} \: \ce{O} \nonumber \], \(\mathrm{Fe:\:\dfrac{1.252\:mol}{1.252}}\), \(\mathrm{O:\:\dfrac{1.879\:mol}{1.252}}\), The "non-whole number" empirical formula of the compound is \(\ce{Fe_1O}_{1.5}\). Let me do this in a Direct link to Just Keith's post If I follow what you mean, Posted 8 years ago. For example, lets say that we have a compound that is made up of 40.92% carbon. The molecular formula represents the total number of elements present whereas the empirical formula represents the smallest ratio between the individual atoms. know, I from empirical evidence I now believe this, this of mercury, that's a number. Next, divide all the mole numbers by the smallest among them, which is 3.33. Questions Case 1: Molecular formula of a compound is given Therefore, in chemistry, the elements and compounds are represented in abbreviated forms. It is One carbon for every, for every hydrogen. {"smallUrl":"https:\/\/www.wikihow.com\/images\/thumb\/e\/ed\/Find-the-Empirical-Formula-Step-1.jpg\/v4-460px-Find-the-Empirical-Formula-Step-1.jpg","bigUrl":"\/images\/thumb\/e\/ed\/Find-the-Empirical-Formula-Step-1.jpg\/aid4651747-v4-728px-Find-the-Empirical-Formula-Step-1.jpg","smallWidth":460,"smallHeight":345,"bigWidth":728,"bigHeight":546,"licensing":"