1 / 25

The Mole

Chapters 10 & 11. The Mole. What is a mole?. http://www.topnews.in/health/scientists-identify-protein-marks-difference-between-mole-and-melanoma-2990. What is a mole?. http://scienceblogs.com/neurophilosophy/2009/08/the_star_nosed_moles_amazing_appendages.php.

tan
Télécharger la présentation

The Mole

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. Chapters 10 & 11 The Mole

  2. What is a mole? http://www.topnews.in/health/scientists-identify-protein-marks-difference-between-mole-and-melanoma-2990

  3. What is a mole? http://scienceblogs.com/neurophilosophy/2009/08/the_star_nosed_moles_amazing_appendages.php http://animals.nationalgeographic.com/animals/mammals/naked-mole-rat/

  4. A unit of measurement for molecules # of particles of any chemical substance 1 mole = 6.02x1023 particles This is known as Avagodro’s # 1mole of Carbon = 6.02x1023atomsof Carbon 1mole of water = 6.02x1023molecules of H2O 1mole of glucose = 6.02x1023moleculesof C6H12O6 1mol of popcorn kernels = 6.02x1023 kernels (enough to bury the entire US under 9 feet of popcorn kernels!) What is a mole in CHEMISTRY? http://www.holidayforeveryday.com/?p=451

  5. Practical Application of the Mole Molar Mass = mass of 1 mole of a substance in grams = average atomic mass given in periodic table

  6. Practical Application of the Mole Formula Mass = sum of the atomic masses of each element represented in formula

  7. Learning Check Prozac, C17H18F3NO, is a widely used antidepressant that inhibits the uptake of serotonin by the brain. Find its molar mass.

  8. Calculations with Molar Mass Mole Conversions molar mass Grams Moles If you know one, you can calculate the other!

  9. Calculations with Molar Mass Mole Conversions Practice Example #1 Aluminum is often used for the structure of light-weight bicycle frames. How many grams of Al are in 3.00 moles of Al? = 81g of Al

  10. Learning Check The artificial sweetener aspartame (Nutra-Sweet) formula C14H18N2O5 is used to sweeten diet foods, coffee and soft drinks. How many moles of aspartame are present in 225 g of aspartame? = 0.76 mol aspartame

  11. Calculations with Molar Mass Multistep Mole Conversions molar mass Avogadro’s # Grams Moles Particles Everything goes through moles!

  12. Multistep Practice Problem #1 How many atoms of Cu are present in 35.4 g of Cu? = 3.4 X 1023 atoms Cu

  13. How many atoms of K are present in 78.4 g of K? Multistep Practice Problem #2 = 1.21 x 1024 atoms K

  14. What is the mass (in grams) of 1.20 X 1024 molecules of glucose (C6H12O6)? Multistep Practice Problem #3 = 358 g glucose

  15. How many atoms of O are present in 78.1 g of oxygen gas? Multistep Practice Problem #4 = 2.94 x 1024 atoms of O

  16. Calculations with Molar Volume Translation… Molar Volume One mole of any gas at STP = 22.4L Gases at STP (Standard Temperature & Pressure) with the same number of particles will occupy the same volume

  17. Calculations with Molar Volume Molar Volume Practice Problem A student fills a 1.0L flask with carbon dioxide (CO2) at standard temperature and pressure. How many molecules of gas are in the flask? = 2.69 x 1022 molecules CO2

  18. Empirical & Molecular Formulas Percent Composition • The mass of each element in a compound compared to the total mass

  19. Calculating Empirical Formulas What is the empirical formula of a compound containing 25.9% N and 74.1% O?

  20. Calculating Molecular Formulas

  21. Stoichiometry: Mole-Mole A balanced formula indicates the number of moles of each compound. Ex: 2HCl + Zn  ZnCl2 + H2 2 moles HCl+1 mole Zinc yield 1 mole Zinc Chloride +1 mole hydrogen gas Based on this formula, how many moles of HCl are needed to react with 2.3 moles of Zn?

  22. Stoichiometry: Mass-Mass In a thermite reaction, powdered aluminum reacts with iron (III) oxide to produce aluminum oxide and molten iron. What mass of aluminum oxide is produced when 2.3g of aluminum reacts with iron (III) oxide? Balanced Equation Stoichiometry 2 2 Al + Fe2O3 Al2O3 + Fe = 4.3g Al2O3

  23. Stoichiometry: Mass-Volume Sodium Bicarbonate (NaHCO3) can be used to extinguish a fire. When heated, it decomposes into sodium carbonate, carbon dioxide and water. If a sample contains 4.0g NaHCO3, what volume of CO2 gas is produced? Balanced Equation Stoichiometry 2 NaHCO3  Na2CO3 + H2O + CO2 = .53L CO2

  24. Limiting Reactants • The limiting reactant in any equation • would produce a smaller amount of product • is completely used up first • determines the amount of product made • Which reactant in an equation is the limiting reactant?

  25. Percent Yield Expected yield is determined from a stoichiometry problem. Actual yield is the amount of product measured or recovered.

More Related