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**Chemical Quantities In Reactions**

Chapter 8 Chemical Quantities In Reactions

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**Homework Assigned Problems (odd numbers only)**

“Questions and Problems” 8.1 to 8.31 (begins on page 230) “Additional Questions and Problems” 8.39 to 8.51 (begins on page 247) “Challenge Questions” 8.53 and 8.55, page 248 “Combining Ideas” CI 11 and CI 13, page 250

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**Mole Relationships in Chemical Equations: Conservation of Mass**

As a chemical reaction proceeds: Reactants are consumed and new materials with new chemical properties are produced Bonds are broken, formed, or atoms are rearranged which produces new substances No material is lost or gained as original substances change to new substances

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**Mole Relationships in Chemical Equations: Conservation of Mass**

Law of Conservation of Mass Quantity of matter does not change during a chemical reaction The sum of the masses of products is equal to the sum of masses of reactants Atoms are neither created nor destroyed in chemical reactions

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**Mole Relationships in Chemical Equations: Conservation of Mass**

A balanced equation has the same number of atoms on each side of the arrow 2 2 Since every atom must be accounted for, a balanced equation obeys the law of conservation of mass Showing the use of coefficients to balance a chemical equation

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**Information Available from a Balanced Chemical Equation**

“1 mole of methane gas reacts with 2 moles of oxygen gas to produce 1 mole of carbon dioxide and 2 moles of water vapor.” Multiplying each of the molar masses by the coefficient will give the total mass of reactants and products Using the balanced word equation and converting to the formula equation

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**Information Available from a Balanced Chemical Equation**

Balanced chemical equations tell us: Relative number of atoms reacting and produced Number can be in terms of single atoms, or moles of atoms 2

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Mole-Mole Factors In a balanced equation, conversion from moles of one substance to another will be determined by the values of the coefficients To determine how many moles of methanol would be produced if moles of hydrogen gas is consumed Will require a mole to mole conversion Converting the given mole amount of hydrogen gas to the needed mole amount of methanol 2

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Mole-Mole Factors 2 Coefficients of the balanced equation can be used to make ratios (conversion factors) between the different reactants and products Mole to mole ratios

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Mole-Mole Factors Write all of the possible mole ratios for the following chemical equation 2 2

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**Using Mole-Mole Factors in Calculations**

Calculations based on balanced equations require the use of mole to mole conversions Equation must be balanced Identify the known and needed substances Make the conversion factor based on Balanced equations are mole statements

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**Stoichiometry Using mole ratios from a BALANCED chemical equation**

moles A moles B grams A grams B MM of A MM of B Stoichiometry Using mole ratios from a BALANCED chemical equation Can convert moles of one compound to moles of another compound using the correct mole ratio Mol-mol factor

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**Using Mole-Mole Factors in Calculations: Calculating Moles of a Product**

Calculate the moles of CO2 formed when 4.30 moles of C3H8 reacts with (the required) 21.5 moles of O2 Balance the equation Plan to convert the given amount of moles to the needed amount of moles Use coefficients to state the relationships and mole-mole factors Set up the problem using the mole-mole factor and canceling units 5 3 4 Show on the board how to calculate the 21.5 moles of oxygen, the required amount

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**Using Mole-Mole Factors in Calculations: Calculating Moles of a Product**

5 3 4 Mol-mol factor Given: Needed: Identify given and needed number of moles Write the plan to convert the given to the needed Mole-mole factor Mole-mole relation 1 mol C3H8 = 3 mol CO2

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**Using Mole-Mole Factors in Calculations: Calculating Moles of a Product**

Set up the problem using the mole-mole factor that cancels given moles and provides needed moles 5 3 4 Mole-mole factor

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**Mass Calculations for Reactions**

From the balanced equation It is also possible to start with a known mass of one substance Then convert to moles of another substance Start with a known amount of moles of a substance Then convert to the sought mass of another substance

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Mass Calculations Convert the moles of one substance to moles of another substance Find the mole-mole factor using the coefficients in the balanced equation Ratios ONLY apply to moles, NOT grams Convert grams to moles, then use mole ratio Can also start with the mass of A and calculate the mass of B Mol-mol factor

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**Mass Calculations You can only relate moles of two compounds**

Ratios ONLY apply to moles, NOT grams Convert grams to moles, then use mole ratio

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**Mass Calculations For Reactions: Mass of Product from Mass of Reactant**

moles C3H8 moles CO2 grams C3H8 grams CO2 MM of A MM of B Stoichiometry What mass of carbon dioxide is produced when 96.1 g of propane react with sufficient oxygen? Balance the equation Plan to convert the given mass to given moles Convert the given moles to needed moles by the use of mole-mole factor Convert the needed moles to needed mass 5 3 4

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**Mass Calculations Example 1**

moles C3H8 moles CO2 grams C3H8 grams CO2 MM of A MM of B moles A moles B Stoichiometry Write the equalities 1 mol C3H8 = g C3H8 1 mol CO2 = g CO2 1 mol C3H8 = 3 mol CO2 to create mole-mole factor 5 3 4 Given: 96.1 g C3H8 Mass needed: g of CO2 Use the coefficients to write the equalities, then mole to mole factors Equality 1 to convert moles to mass Equality 2 to convert mass to moles Equality 3 mole to mole ratio from the coefficients

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**Mass Calculations Example 1**

5 3 4 X g CO2

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**Mass Calculations Example 2**

What mass of carbon monoxide and what mass of hydrogen are required to form 6.0 kg of methanol by the following reaction: 2

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**Mass Calculations Example 2**

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**Mass Calculations Example 2**

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Limiting Reactants Chemical reactions with two or more reactants will continue until one of the reactants is used up The reactant used up is called the limiting reactant (reagent) This limits the amount of product that can be made The reaction will stop once that reactant is gone

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Reactions In the lab, reactants do not always combine in exact mole ratios Often reactions are run with more of one reactant than is needed (excess) A reaction will continue until one of the reactants runs out Reactant that runs out first is the Limiting Reactant More of one reactant is an excess

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**Calculating Moles of Product from a Limiting Reactant**

To determine the limiting reactant between two reactants Balance the equation Determine the number of moles of each reactant Calculate the number of moles of product that each of the reactants (moles) would produce The reactant producing the least amount of product (moles) is the limiting reactant

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**Calculating Moles of Product from a Limiting Reactant**

Determine the number of moles of product that each reactant can make The smallest number is the MAXIMUM product you can make The reactant that gives the smallest amount of product is the limiting reactant

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**Calculating Mass of Product from a Limiting Reactant**

Balance the equation Determine the amount of product that can be made by each reactant Compare numbers Reagent that gives the smaller number is limiting and that is the maximum amount of product that can be made

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**Limiting Reactant Problem**

Lithium nitride, an ionic compound containing Li+ and N3- ions, is prepared by the reaction of lithium metal and nitrogen gas. Calculate the mass of lithium nitride formed from 56.0 g of nitrogen gas and 56.0 g of lithium metal. 2 6

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**Limiting Reactant Problem**

moles Li moles Li3N grams Li Grams Li3N MM of Li MM of Li3N Stoichiometry 6 3 Given: 56.0 g Li Given: 56.0 g N2 Needed: g of Li3N Equalities and Conversion Factors 1 mol Li = 6.941g Li 1 mol N2 = g N2 1 mol Li3N= g Li3N

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**Calculate the Limiting Reactant**

8.07 mol Li 2.69 mol Li3N Set up problem Fewer number of moles of product with Li as reactant, so it is limiting 2.00 mol N2 3.997 mol Li3N

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**Limiting Reactant Problem**

Lithium is the limiting reagent. Calculate the number of grams of lithium nitride formed in the reaction based on the limiting reactant: 2.69 mol of lithium 93.7 g Li3N

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Product Yield The calculated amount of product that should be obtained is called the theoretical yield Assumes all reactants are converted to product based on the mole-mole ratios of reactant to product Rarely do you get the maximum amount of product Side reactions Loss during transfer Accidental spills Also impure reagents and solubility problems

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**Percent Yield Theoretical Yield The calculated amount of product**

Actual Yield The actual amount of product Something less than the theoretical Percent Yield The fraction of the theoretical yield actually obtained is expressed as a percent Theoretical based on the mole ratios

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Percent Yield Example In the previous limiting reactant problem, you actually produced g of Li3N. What is the percent yield of this reaction? 96.9 % yield

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Mass Relationships in Chemical Reactions Chapter 3 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Mass Relationships in Chemical Reactions Chapter 3 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

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