3/6/2018. Limiting Reactant. Reacting Amounts. Reacting Amounts. Limiting Reactants. Example of Everyday Limiting Reactant.

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1 Chapter 9 Lecture Limiting Reactant Chapter 9 Chemical Quantities in Reactions 9.4 Limiting Reactants Fifth Edition A limiting reactant in a chemical reaction is the substance that is used up first stops the reaction limits the amount of product that can form Learning Goal Identify a limiting reactant when given the quantities of two reactants; calculate the amount of product formed from the limiting reactant. 2 Reacting Amounts In a table setting, there are 1 fork, 1 knife, and 1 spoon. How many table settings are possible from 6 forks, 4 spoons, and 7 knives? What is the limiting item? Reacting Amounts Four table settings are possible. Initially Used Extra forks spoons knives The limiting item is the spoon. 3 4 Example of Everyday Limiting Reactant How many peanut butter sandwiches can be made from 8 slices of bread and 1 jar of peanut butter? With 8 slices of bread, only 4 sandwiches can be made. The bread is the limiting reactant. Limiting Reactants When 4.00 mol of H 2 is mixed with 2.00 mol of Cl 2, how many moles of HCl can form? H 2 (g) + Cl 2 (g) 2HCl (g) 4.00 mol 2.00 mol??? Mol 5 6 1

2 Limiting Reactants Using Checking Calculations Calculate the moles of product from each reactant, H 2 and Cl 2. moles of HCl from moles of H mol H 2 x 2 mol HCl = 8.00 mol of HCl 1 mol H 2 (not possible) moles of HCl from moles of Cl mol Cl 2 x 2 mol HCl = 4.00 mol of HCl 1 mol Cl 2 (smaller number) The limiting reactant is Cl 2 because it produces the smaller number of moles of HCl. Initial React/ Form Left after reaction Reactants H mol Cl mol Product 2HCl 0 mol 2.00 mol 2.00 mol mol 2.00 mol Excess 0 mol Limiting 4.00 mol 7 8 Calculating Mass of Product from a Limiting Reactant Calculate the of water produced when 2.00 g of H 2 and 2.00 g of O 2 react? 9 10 STEP 1 Use molar to convert the grams of each reactant to moles. Given 2.00 g of H 2 and 2.00 g of O 2 Need grams 2.00 g H 2 x 1 mol H 2 = mol of H g H g O 2 x 1 mol O 2 = mol of O g O 2 STEP 2 Write mole-mole factors using the coefficients in the equation. 1 mol of O 2 = 2 mol 1 mol O 2 and 2 mol H 2 O 2 mol H 2 O 1 mol O 2 2 mol of H 2 = 2 mol 2 mol H 2 and 2 mol H 2 O 2 mol H 2 O 2 mol H

3 STEP 3 Calculate moles of product from each reactant and determine the limiting reactant. moles from moles of H mol H 2 x 2 mol H 2 O = mol 2 mol H 2 (not possible) moles from moles of O mol O 2 x 2 mol H 2 O = mol 1 mol O 2 (smaller number) STEP 4 Determine the moles of product or calculate grams of product using molar mol H 2 O x g H 2 O = 2.25 g 1 mol H 2 O The limiting reactant is O 2 because it produces the smaller moles (0.125 mol) Learning Check Calculate the of water produced when 8.00 g of H 2 and 24.0 g of O 2 react. Calculate the of water produced when 8.00 g of H 2 and 24.0 g of O 2 react. STEP 1 State the given and needed quantities (grams). Given: 8.00 g of H 2, 24.0 g of O 2 Need: grams of Copyright H 2 O 2011 Pearson Education, Inc. STEP 2 Write a plan to convert the grams of each reactant to grams of product. of H 2 of H 2 Mole mole factor 1 mole of H 2 = 2.02 g of H 2 of O 2 of O 2 Mole mole factor 3

4 1 mole of O 2 = g of O 2 1 mole = g 2 moles of H 2 = 2 moles 1 mole of O 2 = 2 moles STEP 4 Calculate the grams of product from each reactant; the smaller number is the limiting reactant. Practice grams of potassium metal reacts with grams of Water, What is the limiting reactant? 4

5 Practice Challenge: What of S 2 Cl 2 gas can be prepared from 32.0 grams of sulfur and 71.0 grams of chlorine gas at STP? What remains in the reaction vessel after 150. grams of carbon tetrachloride liquid reacts with 100. grams of solid antimony(iii) fluoride to form difluorodichloromethane (CCl 2 F 2 ) gas and antimony(iii) chloride solid? 5

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