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Understanding Gas Production and Stoichiometry in Chemical Reactions

Explore the relationships between substances in chemical reactions through stoichiometry. Investigate how to determine the amount of gas produced in reactions by applying principles of mass and mole calculations. Engage in hands-on activities utilizing beans, pennies, and M&Ms to solidify understanding. Analyze real-world scenarios like the production of gases from specific reactant quantities and learn how to approach both straightforward and multi-step stoichiometric problems. Gain insight into measuring gases, converting moles, and understanding chemical transformations.

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Understanding Gas Production and Stoichiometry in Chemical Reactions

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  1. Chapter 4 Section 3 How much gas is produced?

  2. Date:HW: CTG p. 285 # 3-8 Do Now: WDYS, WDYT p. 274 Agenda: WDYS, WDYT Investigate: part A

  3. Stoichiometry (def) • The study of the relationships or ratios between two or more substances undergoing a physical or chemical change

  4. Investigate, Part A • Grab a bag of pennies from the teacher—do no open the bag of pennies! • You will also get a penny—don’t lose this. • The scales are around the room. Answerquestions 1 a-c

  5. Do Now I give you a bag of M&M’s. Knowing what you know in class, you weigh the bag with the M&M’s and it comes out to be about 350g. You then weigh one M&M and it comes out to be 0.75g. You then eat the M&M’s and you find that the bag itself weights about 1.3g. • How many M&M’s were there?

  6. Investigate Part A • For number 2a, find the rule

  7. Investigate Part A • For number 3, read through the paragraphs and answer letter a • Once completed, complete number 4 • Read through number 5.

  8. 4/16/12 Warm Up I have a bag of peanuts that weighs 70000g. If I weigh one peanut and it is 0.6g, how many peanuts do I have? (The bag weighs 25g)

  9. Recap of Investigation

  10. What are some examples… • Write out a domino for the following conversions: • 1 day = 24 hours • 1 hour = 60 minutes • 1 g of water = 1mL of water (remember to include units!)

  11. The mole… • The mass of one atom is too small to measure • So we use one mole of atoms to make a calculation • 1 atom of H = 1 amu • 1 mole of H = 1 g

  12. Investigation • Answer 7 a-d knowing what we just went through. • When finished, make DOMINOES for each of them.

  13. Investigate Part A • When you have a molecule, you must find all the individual components…. H2O • 2 atoms of Hydrogen • 1 atom of Oxygen

  14. Investigate, Part A • Complete number 8 on p. 276 (you have 5 minutes)

  15. Investigate, Part A • When you have a molecule, you must add up all the individual components to find the mass: H2O = 18 amus • 2 atoms of Hydrogen (1 amu each, so 2 amus) • 1 atom of Oxygen (16 amu each, so 16 amu)

  16. Investigate, Part A • Complete number 9 on p. 276

  17. 4/17/12 Warm Up For the next few problems, use CaCO3 • How much of each individual atom is present in the molecule? • How much does one mole of this compound weigh?

  18. Investigation, Part A • Do number 10 a-c on p. 276. • Use the example of water to help you!

  19. Investigate, Part A 11 a:

  20. Investigate, Part A Complete 11 b-d (looks similar to what you see) Only use the dominoes from the previous problem!

  21. Investigate, Part B • Read aloud number 1 2AgNO3 + CaCl2 2AgCl + Ca(NO3)2

  22. Investigate, Part B • Read aloud number 1 2AgNO3 + CaCl2 2AgCl + Ca(NO3)2 If I have 5 moles CaCl2 How many moles of AgCl do I have? If I have 5 moles AgNO3 How many moles Ca(NO3)2 do I have?

  23. Investigate, Part B • You have 5 minutes to answer 1 a-d • Remember, make dominoes like the one on the last slide!

  24. 3/18/12 Warm Up If I have 3 moles of NaNO3, how many grams are present? If I have 38g of NaNO3, how many moles are present?

  25. Use the following equation to solve the problem: Ba(NO3)2 + 2AgCl  BaCl2 + 2AgNO3 If I have 3 moles of Ba(NO3)2, How many moles of AgNO3 are produced?

  26. 4/23/12 Warm Up For the next few problems, use the equation below: 2KClO3 2KCl + 3O2 If I react 4 moles of KClO3, how many moles of KCl will I get as a product? How many moles of O2 will I then get?

  27. Investigate, Part C • Read aloud number 1 on p. 277 • You can use dominoes to calculate the amount of gas!

  28. Examples • 1a: How many liters will 4 moles of hydrogen gas occupy? • 1b: If an oxygen balloon fills 11.2L, how many moles of O2 are in it? • Complete 1c on your own!

  29. Investigate, Part C • Read aloud and complete number 3 together.

  30. 1) Simple One-Step Problems: If I have 7 g of H2O, how many moles do I have?

  31. 1) Simple One-Step Problems: If I have 7 moles of CaCO3, how many grams do I have?

  32. 1) Simple One-Step Problems: If I have 7 moles of H2O (g), how many Liters do I have?

  33. 2) (more) Complex Multistep Problems In the following reaction: 2H2 + O22 H2O 1) If I start out with 8 g of H2, how many moles of H2O do I end up with? 2) How many g of H2O

  34. 2) (more) Complex Multistep Problems In the following reaction: 2 Na (s) + Cl2(g) 2 NaCl (s) 1) If I start out with 8 g of Na, how many moles of Cl2 do I end up with? 2) How many g of NaCl?

  35. Summary • Essential Questions, p. 283 --How do you know? --Why do you believe --Why should you care

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