1 / 13

Stoichiometry

This guide explores stoichiometry through detailed examples of chemical reactions, including water formation and combustion of ethanol. It emphasizes the importance of conservation of atoms and mass in balanced chemical equations. By analyzing reactions like H2O formation from H2 and O2, and the combustion of ethanol (C2H5OH) with oxygen, it illustrates mole relationships and calculations of products. Additionally, we address practical calculations for moles, grams, and liters based on the given reactions, providing a solid foundation for understanding stoichiometric relationships in chemistry.

oberon
Télécharger la présentation

Stoichiometry

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Stoichiometry • The Chemical Equation: • H-O-H + H-O-H --> O=O + H-H + H-H • 2 molecules --> 1 molecule + 2 molecules • note that atoms are conserved • 2 atoms of oxygen are seen in the reactants and in the products • 4 atoms of hydrogen are seen in the reactants and the products • MOLECULES ARE NOT CONSERVED

  2. Stoichiometry • H- O-H + H-O-H --> O=O + H-H + H-H • Now by multiplying the equation by 6.02 x 1023 we now have • 2 moles H-O-H --> 1 mole O=O + 2 moles of H-H • note that MOLES ARE NOT CONSERVED BUT ATOMS ARE STILL CONSERVED.

  3. Stoichiometry • H- O-H + H-O-H --> O=O + H-H + H-H • If atoms are conserved then mass is also conserved • 36 grams of water(2 moles) = 32 grams of oxygen(1 mole) + 4 grams of hydrogen(2 moles).

  4. Stoichiometry • 2 H-O-H --> O=O + 2 H-H • A balanced equation is necessary to enable us to preduct the quantities of reactants needed to produce required amounts of specified products • It is not practical to go into the lab to deduce formulas and an equation for every reaction

  5. Stoichiometry • Thus is it important to write correct formulas and balance equations correctly • The coefficients in a balance equation, therefore, stand for the relative number of moles of substances involved in the 2reaction.

  6. Stoichiometry • Using the reaction of oxygen with ethanol • C2H5OH + 3 O2 --> 2 CO2 + 3 H2O • Determine the following: • The mole relationships between • C2H5OH and O2, CO2 and H2 • O2 and CO2 and H2O • CO2 and H2O

  7. Stoichiometry • moles of CO2 if 1.5 moles of ethanol burns • grams of CO2 if 1.5 moles of ethanol burns • Grams of CO2 if 23 grams of ethanol burns\ • Liters of CO2 if 23 grams of ethanol burns • Using the reaction of oxygen with ethanol • C2H5OH + 3 O2 --> 2 CO2 + 3 H2O

  8. Stoichiometry • Now it is your turn, for the following reaction • 3 Ag + 4 HNO33 AgNO3 + NO + 2 H2O • Determine the moles of NO produced when 1.5 moles of Ag react completely?

  9. Now it is your turn, for the following reaction • 3 Ag + 4 HNO33 AgNO3 + NO + 2 H2O • Determine the moles of NO produced when 1.5 moles of Ag react completely? • 1.5 moles Ag x 1 mol NO/3 mol Ag = .5 mol NO

  10. Stoichiometry • 3 Ag + 4 HNO33 AgNO3 + NO +2 H2O • How many grams of H2O are produced when 1.5 moles of Ag are reacted completely?

  11. 3 Ag + 4 HNO33 AgNO3 + NO +2 H2O • How many grams of H2O are produced when 1.5 moles of Ag are reacted completely? • 1.5 mol Ag x 2 mol H2O/3 mol Ag = 1 mol H2O 1 mol H2O x 18 gr H2O / 1 mol H2O = 18 gr H2O

  12. Stoichiometry • 3 Ag + 4 HNO33 AgNO3 + NO +2 H2O • How many grams of AgNO3 are produced when 183 grams of HNO3 are reacted completely?

  13. 3 Ag + 4 HNO33 AgNO3 + NO +2 H2O • How many grams of AgNO3 are produced when 183 grams of HNO3 are reacted completely? • 183 gr HNO3 x 1 mol HNO3/ 63 gr HNO3 = 3 mol • 3 mol HNO3 x 3 mol AgNO3/4 mol HNO3 = 2.25 mol AgNO3 • 2.25 mol AgNO3 x 170 gr AgNO3/ mol AgNO3 = 382.5 gr AgNO3

More Related