Stoichiometry Chemistry Ms. Piela

Stoichiometry The quantitative study of reactants and products in a chemical reaction Chemical reactions give info about how molecules combine, and can be used to determine amounts of substances that form

Mole to Mole Calculations When using a chemical equation to determine the amount of the substance, you must relate them by their mole ratios Example #1: ____ H2 + ____ O2 → ____ H2O If you start with 4 moles of O2 how many moles of H2O would form?

Mole to Mole Calculations Example #2: ___ Fe + ____ S → ___Fe2S3   How many moles of iron (III) sulfide, Fe2S3, forms if the reaction initially starts with 8 moles of iron, Fe?

Mass to Mass Calculations Example #1: ___ H2 + ___ O2 → ___ H2O If 2.4 g of O2 are reacted with excess H2 gas, how many moles of H2O would form? 0.15 mol H2O

Mass to Mass Calculations Example #2: ___ H2 + ___ O2 → ___ H2O In the above equation, if I started with 3 grams of H2, how many grams of H2O would form? 26.8 g H2O

Mass to Mass Calculations Example #3: _ NH3 (g) + _ CO2 (g) → _ (NH2)2CO(aq) + _H2O(l) When 2.00 grams of ammonia, NH3, react with excess CO2, what mass of water (in grams) is formed? 1.06 g H2O

Limiting Reactant The reactant used up first in a chemical reaction Also called limiting reagent After a reaction, excess reactants are left These are reactants present in greater quantities that remain after a reaction takes place

4 legs + 1 seat + 10 screws → 1 chair Limiting Reactant Chair analogy: It’s your lucky day! Mr. Nelson has hired you to make chairs! The chairs follow the “reaction”: 4 legs + 1 seat + 10 screws → 1 chair Here are the supplies you have: 10 legs, 5 seats, and 100 screws. How many chairs be made? What is the limiting reactant?

Limiting Reactant Simulation http://phet.colorado.edu/en/simulation/reacta nts-products-and-leftovers

Limiting Reactant The limiting reactant can be found by determining which of the starting amounts yields the least amount of product

Limiting Reactant Example Problem Sodium chloride can be prepared by the reaction of sodium with chlorine gas: 2Na (s) + Cl2 (g) ® 2NaCl (s) Suppose that 6.70 mol Na reacts with 3.2 mol Cl2 How many moles of NaCl will be formed in this reaction? What is the limiting reactant? Cl2 6.4 mol NaCl

Limiting Reactant Practice Problem 2.70 mol C2H4 is reacted with 6.30 mol of O2. Calculate the amount in moles of water that forms, and identify the limiting reactant. C2H4 (g) + 3O2 (g) ® 2CO2 (g) + 2H2O (g) 4.2 mol H2O

Limiting Reactant Example Problem Urea is prepared by reacting ammonia with carbon dioxide: 2 NH3 (g) + CO2 (g) → (NH2)2CO(aq) + H2O(l) In one process, 637.2 g of NH3 are treated with 1142 g of CO2. Calculate the mass of urea, (NH2)2CO, formed. 1122 g urea

Limiting Reactant Practice Problem Calculate the number of grams of NH3 produced by the reaction of 5.40 g of hydrogen with 8.25 g of nitrogen. The balanced equation is: N2 + 3 H2 ® 2 NH3 9.97 g NH3

Percent Yield Theoretical yield is the amount of product that would result if all the limiting reagent reacted Actual yield is the amount actually obtained in lab from a reaction Actual yield is almost always less than theoretical

Percent Yield Percent yield describes proportion of actual yield to theoretical yield.

Percent Yield Example Problem When 84.8 g of iron (III) oxide reacts with an excess of carbon monoxide, 54.3 g of iron is produced. What is the percent yield of this reaction? Fe2O3 (s) + 3CO (g) ® 2 Fe (s) + 3CO2 (g) 91.6%

Percent Yield Practice Problem If 25 grams of carbon dioxide gas can be produced in the following reaction, how many grams of sodium hydroxide should be produced? If 10.7 grams of sodium hydroxide are actually produced, what is the percent yield? NaHCO3 ® NaOH + CO2 22.7 g NaOH / 41.1%