Stoichiometry
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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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Stoichiometry

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Stoichiometry

Stoichiometry


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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