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Chemistry Assessment: Gas Laws and Acid-Base Concepts

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sofia
104 diapositives · 1.2K Views · Aug 13, 2014

This chemistry assessment focuses on gas laws, acid-base definitions, and equilibrium reactions. Students will engage in a warm-up activity that involves identifying the role of compounds as Bronsted-Lowry bases and Arrhenius acids in various reactions. Through a collaborative White Board Jeopardy session, teams will review essential concepts such as pH calculations, properties of acids and bases, and classifying reactions. The assessment prepares students for their Acid/Base Exam, scheduled for tomorrow, and aims to solidify their understanding of key chemistry principles.

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  1. Week 32 Chemistry Assessment 9, Gas Laws

  2. Write the Learning Target Warm Up: 4 Minutes Sit in your assigned seat You should be working SILENTLY The reaction between carbonic acid and water is shown below: H2CO3 + H2O D H3O+ + HCO3- Which compound is acting as the Bronsted-Lowry Base in the forward reaction? Which compound is acting as the Arrhenius Acid in the forward reaction?

  3. Announcement/Reminders • Acid/Base Exam is TOMORROW • Exam is 24 questions long

  4. Reminder!!! Exam Tomorrow

  5. Agenda • Warm Up- 7 Minutes • Purpose of Review/ Material Covered- 3 Minutes • Expectations for White Board Jeopardy- 3 Minutes • White Board Jeopardy- 37 Minutes • Closing- 3 Minutes

  6. Purpose of Reviewing • Prepare for Assessment 9

  7. Why Prepare? 85% 21 Questions

  8. Material Covered on Assessment 9 • Properties of Acids and Bases • Arrhenius and Bronsted-Lowry Definitions • Classifying Reactions • pH scale • pH Calculations (pH, pOH, [H+], [OH-]) • Strengths of Acids and Bases (Ka, Kb)

  9. White Board Jeopardy Students will work in groups of 3 to 4 (Team number is on the desk in front of you). Students will need Dry Erase Board, Marker, Periodic Table, Eraser, and Calculator. NOTES are allowed during White Board Jeopardy

  10. White Board Jeopardy Team # How to Play??? Write your team number in the upper right hand corner During the song, you will work the problem shown in your lap INDIVIDUALLY. At the end of the Jeopardy song, you will talk with your group. When Mr. Ghosh says “Boards Up” , all students in group must have Identical responses on their Dry Erase Boards that are correct in order to receive FULL CREDIT. Boards that are not up will not be counted. You may be called on randomly to explain your answer. If I do this and you cannot explain correctly, your team will NOT receive credit.

  11. Scoring and Rules/Expectations Scoring: All questions are worth 1 point Rules/Expectations: No talking during the Jeopardy song Must be working individually during the song No arguing with Mr. Ghosh about scoring Must be explaining WHY during group work time Any violations of the rules/expectations will result in your team losing a point

  12. Prizes! The team that finishes with the most number of points will receive 5% extra credit on the Exam tomorrow.

  13. Which of the following is a property of a base? • Bases are bitter in taste • Bases have a strong color • Bases are unreactive • Bases turn litmus paper red

  14. The equation below represents an equilibrium reaction: CH3NH2+ H2O D CH3NH3+ + OH- According to the Brønsted- Lowry theory of acids and bases, which of the following is acting as the base for the forward reaction? • CH3NH2 • H2O • CH3NH3+ • OH-

  15. Which of the following is a precipitation reaction? • 4 Al (s) + 3 O2 (g)  2 Al2O3 (s) • Ca(NO3)2 (aq) + Na2SO4 (aq)  CaSO4 (aq) + 2 NaNO3 (aq) • HClO4 (aq) + KOH (aq)  KClO4 (aq) + H2O (l) • KBr (aq) + AgNO3 (aq)  KNO3 (aq) + AgBr (s)

  16. What does the pOH for a solution measure? • The relative hydrogen ion concentration • The relative hydroxide ion concentration • The molarity • The solubility

  17. A solution of Rubidium Hydroxide (RbOH) was designed to have a molarity of 0.65 mol/L. However, there was a mistake in measurement and there are actually 2.45 moles of OH- dissolved in 8.87L of solution. Calculate the pH for the solution.

  18. The Kb for a base is calculated using the following formula: Calculate the Kb if [HB] = 1.4 x 10-7 M, [OH-] = 1.80 x 10-5 M, and [B-] = 178 M. Would this be a stronger or weaker base than one with a Kb of 1.6 x 10-9?

  19. Why is NaOH considered an Arrhenius base? • It has a pH less than 7 • It releases OH- ions in solution • It is able to accept protons • It reacts with hydrogen ions

  20. A chemical reaction is shown below: Ca+ 2H+Ca2+ + H2 Why is this chemical reaction classified as an oxidation-reduction reaction?

  21. A chemistry student added two clear liquids together. The products of the reaction were water and an aqueous salt. What kind of reaction occurred?

  22. Solution A has a pH of 4, and Solution B has a pH of 9. Which solution has a higher concentration of hydrogen ions? • Solution A • Solution B • They have the same concentration of hydrogen ions • The concentration of hydrogen ions cannot be determined

  23. Calculate the pH for a solution with a hydrogen ion concentration of 1.98 x 10-9 M.

  24. Two different basic solutions are compared. Both Solution #1 and Solution #2 ionize slightly in water. Which of the following is true of the two solutions? • Solution #1 and Solution #2 are strong bases • Solution #1 is a strong base, Solution #2 is a weak base • Solution #1 is a weak base, Solution #2 is a strong base • Solution #1 and Solution #2 are weak bases

  25. The Kb values for four different bases are shown below: • 2.7 x 10-7 • 5.4 x 10-3 • 6.9 x 10-5 • 3.1 x 10-8 Order the bases from strongest to weakest

  26. Closing Good Luck Studying

  27. Write the Learning Target Warm Up: 4 Minutes Stay in your own seat You should be working SILENTLY • Write three things that you could do once you get your test to ensure that you’re successful. • When you’re done, look through your notes and worksheets to prepare for the assessment.

  28. Agenda • Warm Up: 5 Minutes • Goals/ Expectations for Assessment: 3 Minutes • Assessment: 42 Minutes • Closing: 3 Minutes

  29. Why Prepare? What is Mastery? 21 Questions 85%

  30. Expectations for Assessment Clear your desk of everything except a.... • Number 2 Pencil • Scantron • Calculator Backpacks and binders on the floor

  31. Testing Tips • Read the problem and answer choices CAREFULLY • If you don’t know the answer, make sure you at least take a guess • Guessing on questions you don’t know can only help you! • Bubble your answers completely (scantron and test booklet) Periodic Table is in the test packet

  32. Testing Rules • Students will remain SILENTfor the duration of the test. Even if you are done, YOU CANNOT TALK or MAKE OTHER NOISES • Keep your eyes on YOUR OWN PAPER • Raise your hand if you have a question Failure to follow the testing rules will result in your test being taken. You will then receive a ZERO and a dean referral.

  33. Good Luck!

  34. Closing • How was your assessment? • What could you have done differently?

  35. Write the Learning Target Warm Up: 4 Minutes Stay in your own seat You should be working SILENTLY Suppose that you have two balloons. Balloon #1 contains air under high pressure, while Balloon #2 contains air under low pressure. Which balloon would you expect to take up more space?

  36. Agenda • Warm Up: 7 Minutes • Boyles Law Video: 15 Minutes • Guided Practice: 13 Minutes • Independent Practice: 15 Minutes • Closing: 3 Minutes

  37. Let’s look at Boyle’s Law

  38. What did you see?

  39. Warmup-Round 2 Suppose that you have two balloons. Balloon #1 contains air under high pressure, while Balloon #2 contains air under low pressure. Which balloon would you expect to take up more space?

  40. Boyles Law Video • Go to shschem.weebly.com (our class website) Bookmark this if you haven’t done so already!!! • Hover over my page: Mr. Ghosh  Video Lessons • Watch video for April 23 • Take notes on your handout

  41. What is a Law? • A law is a statement that describesactions or a set of actions that occurs consistently.

  42. What is Volume? • Space occupied by any sample of matter.

  43. Pressure • What is pressure? A Force Exerted by a Gas over a Given Area • What causes pressure? Collisions of the Gas Particles with the Walls of the Container That’s Pressure! Walls of the Container Gas Particle

  44. Units for Pressure atmospheres = atm millimeters of mercury = mmHg kilopascals = kPa pounds per square inch = psi torricelli = torr 1 atm = 760mmHg = 101.3kPa = 14.7psi= 760 torr Standard Pressures

  45. Boyle’s Law

  46. Boyle’s Law

  47. Boyle’s Law

  48. Boyle’s Law

  49. Boyle’s Law

  50. Example #1 1000 mL of a gas at a pressure of 101.3 kPa is compressed to 473 mL. What is the new pressure of the gas? [Round to the tenths place]