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Stoichiometry

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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  1. Stoichiometry

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

  3. Reviewing Balancing Equations S Fe Fe2S3 S Fe S • Can change coefficients but CANNOT change subscripts • Example • 3S + 2 Fe  Fe2S3

  4. Reviewing Balancing Equations • Al + CuO Al2O3 + Cu • ____________________________

  5. Reviewing Balancing Equations • H2 + O2 H2O _______________________

  6. 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

  7. 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

  8. 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

  9. 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?

  10. 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 ___________

  11. 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?

  12. 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

  13. % Yield • Calculated by taking • _____________________________________

  14. 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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