CHEM 111 1st Edition Lecture 5 Past Lecture Review:Avogadro’s Number (6.022 x 1023), Mass Percentage Calculation, Converting Moles and Mass, Converting Moles and Entities, Oxidation/Reduction, Neutralization, Combustion Reactions.Current Lecture: 2/04/2014Molecular Formula: The molecular formula must be a whole multiple of the empirical formula.- If the empirical formula is CH2, the molecular formula is (CH2)n wheren = molar mass of compound / molar mass of empirical formulaEx: A compound has the empirical formula C4H8O. The molar mass of this compound is 216 g/mol. What is the molecular formula?First, you must find the molar mass of the empirical formula.C=12.011 (4) = 48.044 g/molH=1.008 (8) = 8.064 g/molO=15.999 g/molMolar mass of empirical formula = 72.107 g/mol216 g/mol / 72.107 g/mol = 3Therefore, the molecular formula of this compound is (C4H8O)3Guidelines for Reaction StoichiometryWrite the Balanced Equation.Calculate the number of moles of the species for which the mass is given.Use the coefficients in the equation to convert the moles of the given substance into moles of the substance desired.Calculate the mass of the desired species.These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.Reaction StoichiometryMass of A ---> Molar Mass of A ---> Moles of A ---> Coefficients in chemical equation ---> Molesof B ---> Molar Mass of B ---> Mass of B Current Lecture Review:Reaction Stoichiometry (rules and how to calculate), How to calculate Molecular