Chapter 9Stoichiometry

Unit Essential Question:

What numerical information can we find from a balanced chemical reaction?

Lesson Essential Question:

How can we tell the amounts of substances involved in a reaction?

Section 1: Calculating Quantities in Reactions

Coefficients of balanced equations show proportions (ratios) of substances in reactions.

Similar to amounts in a recipe.Use this information to adjust amount of product(s) made or reactants needed.

Relative amounts (coefficients) in equation = moles.Example: 2 C8H18 + 25 O2 16 CO2 + 18 H2O

2 moles of C8H18 react with 25 moles of O2 to form 16 moles of CO2 and 18 moles of H2O

StoichiometryDeals with quantities of substances in chemical reactions.Compare amounts (moles) and also masses.

Limiting reactants and percent yield

can be calculated.Can be useful for everyday activities such as baking.

Mole RatioNeeded in order to perform calculations!Allows you to convert between substances.Set up using fractions and conversion factors.

Use dimensional analysis.Get ratios from balanced equation.

Ex: 2H2 + O2 2H2OMole ratio examples: 2mol H2/1mol O2,

1mol O2/2mol H2O, or 2molH2/2molH2O

Steps to Converting Between Amounts of

SubstancesStep 1: Balance the chemical equation.Step 2: Convert given amount to moles.

Remember- always start with your given!Step 3: Use a mole ratio from the balanced equation to convert from the amount of one substance to the amount of another substance.Use dimensional analysis for all conversions!

Step 4: Convert out of moles if asked for grams or the number of particles.

Sample Problem #1Consider the reaction for the commercial

preparation of ammonia:N2 + 3 H2 2 NH3

How many moles of hydrogen are needed to prepare 312 moles of ammonia?

Notice that mole ratios convert between substances and units stay the same (all moles)!

Moles of nitrogen needed?

Sample Problem #2What mass of NH3 can be made from

1,221 g of H2 and excess N2?N2 + 3 H2 2 NH3

Sample Problem #3How many grams of C5H8 form from 1.89 x 1024 molecules C5H12?C5H12 (l) C5H8 (l) + 2 H2 (g)

Lesson Essential Question:

How can we calculate the amount of products made in a reaction?

Section 2: Limiting Reactants and Percent Yield

Limiting reactant – substances that limit the amount of product that can be formed.Limiting reactants run out first!

Excess reactant – substances that are not used up in the reaction. There are some left over.Do not limit the amount of product that

can be formed.Think back to the sandwich activity- what

were...LR [limiting reagent(s)]?ER [excess reagent(s)]?

Theoretical & Actual YieldTheoretical: the amount that should be able

to be produced based on the limiting reactant.If everything in the reaction went according

to plan, and all of the reactant(s) reacted, this is how much product should be made.

This is NOT the same as the actual yield- amount that is produced based on an experiment Error occurs, so actual yield is less than the

theoretical yield.Can never be greater than the theoretical

yield.

This is what we have been calculating in practice problems so far!

Determining the Limiting Reactant

You will be given amounts of two or more reactants.Convert all amounts to moles.Use mole ratios in the balanced chemical equation to determine the number of moles of a product that will be produced.

Convert all reactant amounts into the same product!

Convert the moles of product to grams of product.Do this for each reactant amount given and see

how much product each produces.Whichever produces LESS product is your limiting

reactant- it will be completely consumed first.

Sample Problem #5 Identify the limiting reactant and the

theoretical yield of phosphorus acid, H3PO3, if 225 g of PCl3 is mixed with 123 g of H2O PCl3 + 3 H2O H3PO3 + 3 HCl

Sample Problem #6 Determine the limiting reactant if 14.0g N2 are mixed with 9.0g H2. What is the theoretical yield in grams of the product? N2 + 3H2 2NH3

ApplicationCheapest ingredient = excess

reactant.Most expensive = limiting reactant.

Cost effective!

Examples:Cider vinegar

ER = oxygen; LR = ethanolBanana Flavoring

ER = acetic acid; LR = isopentyl alcohol

Percent YieldActual yield is always less than the theoretical

yield.LR is not always 100% used up.Can be due to human errors, not reacting to completion, reverse reactions and/or unwanted side reactions occurring, and loss during purification.

Efficiency is another name for percent yield.Percent Yield:

(actual yield/theoretical yield) x 100 = % yield

If your percent yield is greater than 100%, there could be unreacted or unwanted materials in your product.

Sample Problem #7 Using your answers from Sample Problem #6, calculate the percent yield if 16.1 g NH3 are formed in an experiment. N2 + 3 H2 2 NH3

Sample Problem #8How many grams of CH3COOC5H11 should form if 4808 g are theoretically possible and the percent yield for the reaction is 80.5%?