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Chemical Quantities

Chemical Quantities. Chapter 12. What do all these things have in common with the mole?. Warm-up #1. 1 dozen. 1 pair. 1 six pack. Answer: They all represent quantities. Measuring Matter. Particles Names. Atoms, formula units (ionic compounds), molecules (covalent compounds).

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Chemical Quantities

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  1. Chemical Quantities Chapter 12

  2. What do all these things have in common with the mole? Warm-up #1 1 dozen 1 pair 1 six pack Answer: They all represent quantities

  3. Measuring Matter Particles Names Atoms, formula units (ionic compounds), molecules (covalent compounds) • What is a mole? • The mole (mol) is the SI base unit used to measure the amount of a substance. • 1 mol = 6.02x1023 representative particles • 6.02x1023 is called Avogadro’s number • Representative particles are the units used in these conversions

  4. Everything Leads to the Mole 1mole = 22.4 L at STP 1mole = molar mass 1mole = 6.02 x 1023 particles

  5. Mole to Particle Conversions 1mole = 6.02 x 1023 particles How many molecules of water are there in 2.4 moles of water? How many moles of copper contain 3.5 x 1018 copper atoms?

  6. Warm-up #2 • What is the mass of this bicycle given the mass of it’s individual parts? 1wheel = 0.5 kg, 1frame = 5 kg, 1seat = 0.2 kg, 1 set of handlebars = 1kg

  7. Mass and the Mole The mass of one mole of a substance is unique to that substance and is based on the sum of the atomic masses of the elements in that substance. 1 mole of copper = 63.6g 1 mole of lead = 207.2g 1 mole of water = 18.0g Mass of H2O = mass of two hydrogen atoms + mass of one oxygen atom

  8. Calculating Molar Mass Elements The molar mass of elements is equal to their atomic mass from the periodic table. Example: 1 mole of Fe atoms = 55.847g Compounds The molar mass of compounds is equal to the sum of the atomic masses of the individual elements in that compound. Example: 1 mole of Fe2(SO4)3= (2 x 55.847) + (3 x 32.066) + (12 x 15.999) = 401.662

  9. Mole-Mass Conversions • Unlike mole-particle conversions where the conversion factor is always 1mole = 6.02 x 1023 particles, each mole-mass conversion factor is unique to the substance involved. Convert 2.3 moles of sodium (Na) to grams of Na Convert 10.0 g of CO2 to moles of CO2

  10. Warm-up #3 What contains more representative particles, a mole of Fe2(SO4)3 or a mole of H2O?

  11. Volume and the Mole According to Avogadro, the mass of one mole of a gas at STP is always 22.4L regardless of the gas’ identity. STP = Standard Temperature and Pressure (0oC and 1 atm)

  12. Mole-Volume Conversions How many moles of CO are contained in 1.8L of CO gas? How many Liters of SO3 are represented by 0.5 moles of SO3 gas?

  13. Multi-Step Conversions 1mole = 22.4 L at STP 1mole = molar mass 1mole = 6.02 x 1023 particles What is the mass of 1.0 x 1019 atoms of Aluminum?

  14. Warm-up #4 • Examine the reaction above. Using the parts below, how many of the product could be made? + 4

  15. What is Stoichiometry? Stoichiometry is the study of quantitative relationships between amounts of reactants used and products formed by a chemical reaction.

  16. Practical Applications of Stoichiometry In a spacecraft, the carbon dioxide exhaled by astronauts can be removed by its reaction with lithium hydroxide, LiOH, according to the following chemical equation. CO2(g) + 2LiOH(s) Li2CO3(s) + H2O(l) How many moles of lithium hydroxide are required to react with 20 mol of CO2, the average amount exhaled by a person each day?

  17. Strategy – Relate everything to the mole The mole is the common thread that links reactants to products. 1CO2(g) + 2LiOH(s) 1Li2CO3(s) + 1H2O(l) Mole Ratios

  18. Mole Super Highway

  19. Stoichiometry Practice Problems 2H2(g) + O2(g) 2H2O(l) How many moles of water can be formed from 3 moles of oxygen? How many grams of water can be formed from 8.0 grams of hydrogen gas at?

  20. Warm-up #5 Ingredients 2 1/4 cups all-purpose flour 1 teaspoon baking soda 1 teaspoon salt 1 cup (2 sticks) butter, softened 3/4 cup granulated sugar 3/4 cup packed brown sugar 1 teaspoon vanilla extract 2 large eggs 2 cups (12-oz. pkg.) 1 cup chopped nuts Yield: 24 cookies How many cookies can be made if I only have 1 stick of butter and 1 cup of sugar (and the exact quantity of the other ingredients in the recipe)?

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