QUANTITATIVE ANALYSIS. LIMITING REACTANT The reactant that is completely consumed during the reaction The reactant NOT consumed is referred to as excess.

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Presentation transcript:

QUANTITATIVE ANALYSIS

LIMITING REACTANT The reactant that is completely consumed during the reaction The reactant NOT consumed is referred to as excess reactant

DETERMINING LIMITING REACTANT Mg(s) + S(s)  MgS(s) Calculate the mass of MgS produced when 4.8g Mg is reacted with 4.8g S Convert both masses into mol MgS (It will be 2 separate calculations) The reactant with a lesser amount of mol is the limiting reagent

EX. LIMITING REAGENT N 2 +3H 2  2NH 3 Calculate the mol of NH 3 produced when 5.2g N 2 reacts with 6.0g H 2

THEORETICAL YIELD Amount of product that can be made in a chemical reaction based on the limiting reagent Calculated in the same manner as the limiting reagent

EX. THEORETICAL YIELD 2NO(g)+ 5H 2  2NH 3 +2H 2 O Calculate the theoretical yield in molof NH 3 when 5.0g NO reacts with 5.0g H 2

ACTUAL YIELD The amount of product ACTUALLY produced by a chemical reaction The data used is determined via experimentation

EX. ACTUAL YIELD Fe2O3(s)+ 3CO(g)  2Fe(s)+ 3CO2(g) In a laboratory procedure, you reacted 2.0g Fe2O3 and 2.0g CO. After weighing the product produced, you determined that 1.19g Fe resulted Determine the actual yield of Fe

PERCENT YIELD Is the relationship between the actual and theoretical yields It is calculated by: (Actual/ Theoretical)X100

EX. PERCENT YIELD Fe 2 O 3 (s)+ 3CO(g)  2Fe(s)+ 3CO 2 (g) In a laboratory procedure, you reacted 2.0g Fe 2 O 3 and 2.0g CO. After weighing the product produced, you determined that 1.19g Fe resulted Calculate the percent yield Fe

PRACTICE PROBLEMS Lead ions precipitate from a solution with KCl according to the following reaction: Pb 2+ (aq)+ 2KCl(aq)  PbCl 2 (s)+ 2K + (aq) During the procedure, 28.5g KCl was added to a solution containing 25.7g Pb 2+ and the PbCl 2 precipitate formed. The precipitate was then filtered and dried and the mass was found to be 29.4g. Determine the limiting reagent (in g), theoretical yield (in g), and percent yield for this reaction.

PRACTICE PROBLEMS For the reaction, 2Na(s)+ Br 2(g)  2NaBr(s) Determine the limiting reagent in mol for the following initial amounts A.2 mol Na and 2 mol Br 2 B.1.8 mol Na and 1.4 mol Br 2 C.2.5 mol Na and 1 mol Br 2 D.12.6 mol Na and 6.9 mol Br 2

PRACTICE PROBLEM For the reaction: 2Al(s)+ 3Cl 2 (g)  2AlCl 3 (s) Calculate the theoretical yield in grams of the following amounts A.2.0g Al and 2.0g Cl 2 B.7.5g Al and 24.8g Cl 2 C.0.235g Al and 1.15g Cl 2