CCL 1110 1st Edition Lecture 7 Outline of Last Lecture II. Empirical formulasIII. Combustion AnalysisOutline of Current Lecture IV. StoichiometryV. Limiting Reactants in ReactionsCurrent LectureI. Stoichiometrya. Stoichiometry- the quantitative study of the reactants and products of a chemicalreactionb. Strategy:i. Begin with a balanced chemical equationii. Deduce molar ratiosc. You can’t measure moles; instead, you measure mass or volume and then convert to molesd. Nearly all stoichiometry problems involve figuring out the relationship between two or more of your reactantsi. Moles of reactant 1 -- moles of reactant 2, where the arrow is a balanced chemical equatione. Often the data and the result are masses (i.e. going from mass of reactant 1 to moles of reactant 1 to moles of reactant 2 to mass of reactant 2)II. Limiting Reactants in Reactionsa. Let’s think back to the example that was in the lecture. Let’s say that you have 8 bicycle wheels, but only 3 frames. You can’t make 4 complete bikes because you only have 3 frames, so instead, you have 3 complete bikes and 2 bicycle wheels left. We can relate this back to chemistry by thinking about limiting and excess reactants. In this case, the bicycle frames are the limiting reactant and the wheels are the excess reactant. b. Theoretical yield- the maximum possible yield of product, predicted by the balanced equation and reactant limitationsThese 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.i. In carrying out a reaction, chemists rarely obtain as much product as predicted by the theoretical yieldii. Percent yield = (actual yield/theoretical yield) x 1001. Actual and theoretical values are most often masses, but this equation works for moles as wellTHIS CONCLUDES ALL THE MATERIAL NEEDED FOR THE FIRST