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Stoichiometry. Balanced Equations. All stoichiometry problems start with a balanced equation. You must check for this! If it is not balanced, BALANCE IT!. Reviewing Balancing Equations. S. Fe. Fe 2 S 3. S. Fe. S. Can change coefficients but CANNOT change subscripts Example

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balanced equations
Balanced Equations
  • All stoichiometry problems start with a balanced equation.
  • You must check for this!
  • If it is not balanced, BALANCE IT!
reviewing balancing equations
Reviewing Balancing Equations

S

Fe

Fe2S3

S

Fe

S

  • Can change coefficients but CANNOT change subscripts
  • Example
    • 3S + 2 Fe  Fe2S3
reviewing balancing equations1
Reviewing Balancing Equations
  • Al + CuO Al2O3 + Cu
  • ____________________________
reviewing balancing equations2
Reviewing Balancing Equations
  • H2 + O2 H2O

_______________________

equations and the mole
Equations and the Mole
  • Remember what an equation actually means
    • Mg + S  MgS
    • One _____________reacts with one ___________ creating one formula unit of MgS
  • But
    • This also means that one mole of _________ reacts with one mole of ___________ to form one mole of _______ formula units.
    • 1 mol Mg, 1 mol S, and 1 mol MgS are stoichiometry equivalents
equations and the mole cont
Equations and the Mole (cont)
  • What about the equation
    • C3H8 + 5O2 3CO2 + 4H2O
    • Now, ____ mol C3H8, _____ mol O2, _____ mol CO2, and _______ mol H2O are stoichiometry equivalents
what does this mean
What does this mean?
  • As stoichiometry equivalents, they can be used in a conversion factor
  • __________________ Conversion Factors
    • One equivalent is placed on top and one on bottom
    • Allows us to move from one compound to another in a balanced equation
stoichiometry problems
Stoichiometry Problems

Given the equation:

MgCl2 + 2 AgNO3 Mg(NO3)2 + 2 AgCl

What is the mass of AgCl produced if 24g of MgCl2 is reacted with excess AgNO3?

What amount of MgCl2 will react with 3.85 g AgNO3?

limiting reagents
Limiting Reagents
  • So far we have been assuming that we have an excess of all the other reactants
  • This is not often true….often you have a set amount of both reactants
    • Each amount would lead you to a different amount of product
    • Must use the number that is ___________
limiting reagent problem
Limiting Reagent Problem

Given the equation:

MgCl2 + 2 AgNO3 Mg(NO3)2 + 2 AgCl

How much AgCl will be produced if 28g of MgCl2 is reacted with 51g of AgNO3?

theoretical and actual yield
Theoretical and Actual Yield
  • Yield is the amount of product that you get from a reaction
  • Theoretical yield is the amount that you should get based on using stoichiometry
  • Actual yield is the amount of product actually attained during an experiment
yield
% Yield
  • Calculated by taking
    • _____________________________________
theoretical and yield
Theoretical and % Yield

Given the equation:

MgCl2 + 2 AgNO3 Mg(NO3)2 + 2 AgCl

What is the percent yield of Mg(NO3)2 if 168.4 g of AgNO3 is reacted to produce 47.2g of Mg(NO3)2?

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