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General Chemistry 2 Final Exam Questions and Answers: Ace Your Exam with Confidence
Are you staring down the barrel of your General Chemistry 2 final exam, feeling overwhelmed by the sheer volume of material? Don't panic! This comprehensive guide provides a structured approach to tackling common General Chemistry 2 final exam questions and answers, helping you build confidence and achieve a stellar grade. We'll cover key concepts, tackle challenging problem types, and provide valuable strategies for exam success. This isn't just a list of questions; it's a roadmap to mastering the subject matter.
Thermodynamics and Equilibrium: Mastering the Fundamentals
This section forms a significant portion of many General Chemistry 2 final exams. Expect questions testing your understanding of:
H2: Gibbs Free Energy and Spontaneity:
H3: Calculating ΔG: Practice calculating Gibbs Free Energy (ΔG) using both standard free energy changes (ΔG°) and the equation ΔG = ΔH - TΔS. Remember to consider the units and the significance of a positive or negative ΔG value in relation to spontaneity.
H3: Relationship between ΔG, K, and Equilibrium: Understand the connection between Gibbs Free Energy, the equilibrium constant (K), and the direction of equilibrium. Be prepared to calculate K from ΔG° and vice versa. Practice problems involving different temperature conditions.
H3: Non-Standard Conditions: Don't forget the equation that accounts for non-standard conditions: ΔG = ΔG° + RTlnQ. Understand how the reaction quotient (Q) affects the spontaneity of a reaction.
H2: Equilibrium Calculations and Le Chatelier's Principle:
H3: ICE Tables: Master the use of ICE (Initial, Change, Equilibrium) tables to solve equilibrium problems. This is a fundamental skill for determining equilibrium concentrations.
H3: Applying Le Chatelier's Principle: Be prepared to predict the effect of changes in concentration, pressure, volume, or temperature on the equilibrium position of a reaction. Know how to explain these shifts using Le Chatelier's Principle.
H3: Acid-Base Equilibria: This often overlaps with thermodynamics. Practice calculating pH, pOH, Ka, and Kb for weak acids and bases. Understand buffer solutions and their capacity to resist pH changes.
Kinetics and Reaction Mechanisms: Understanding Reaction Rates
Kinetics is another crucial area. Expect questions focusing on:
H2: Rate Laws and Reaction Orders:
H3: Determining Rate Laws from Experimental Data: Practice determining the rate law (including reaction orders) from experimental data. Understand the difference between zero-order, first-order, and second-order reactions.
H3: Integrated Rate Laws: Be able to use integrated rate laws to determine the concentration of reactants at a given time or the half-life of a reaction.
H3: Activation Energy and Arrhenius Equation: Understand the concept of activation energy (Ea) and be able to use the Arrhenius equation to calculate the rate constant (k) at different temperatures.
H2: Reaction Mechanisms and Catalysts:
H3: Elementary Steps and Rate-Determining Steps: Understand how a reaction mechanism is composed of elementary steps and how to identify the rate-determining step.
H3: Catalysts and their Effects: Know how catalysts increase the rate of a reaction without being consumed and understand their effect on the activation energy.
Electrochemistry: Mastering Oxidation and Reduction
Electrochemistry often presents challenging problems:
H2: Redox Reactions and Cell Potentials:
H3: Balancing Redox Reactions: Practice balancing redox reactions using the half-reaction method.
H3: Calculating Cell Potentials (Ecell): Know how to calculate the standard cell potential (E°cell) and the cell potential under non-standard conditions using the Nernst equation.
H3: Electrolysis and Faraday's Law: Understand the principles of electrolysis and how to calculate the amount of substance produced or consumed during an electrolytic process using Faraday's Law.
H2: Galvanic and Electrolytic Cells:
H3: Understanding Cell Diagrams: Be able to interpret and construct cell diagrams.
H3: Distinguishing between Galvanic and Electrolytic Cells: Understand the difference between spontaneous (galvanic) and non-spontaneous (electrolytic) cells.
Spectroscopy and Atomic Structure: Delving into the Quantum World
This area often includes:
H2: Atomic Orbitals and Quantum Numbers:
H3: Understanding the Significance of Quantum Numbers: Know the meaning and limitations of the principal (n), azimuthal (l), magnetic (ml), and spin (ms) quantum numbers.
H3: Electron Configurations and Hund's Rule: Be able to write electron configurations and apply Hund's rule to determine the electronic structure of atoms.
H2: Spectroscopy:
H3: Understanding Different Types of Spectroscopy (UV-Vis, IR): Have a basic understanding of how different types of spectroscopy provide information about molecular structure.
Conclusion
Preparing for your General Chemistry 2 final exam requires a systematic approach. By focusing on the core concepts outlined above and practicing regularly with diverse problem sets, you can build a strong understanding of the material and significantly improve your chances of success. Remember to utilize your textbook, lecture notes, and any practice exams provided by your instructor. Good luck!
FAQs
1. What are the most commonly missed questions on General Chemistry 2 finals? Commonly missed questions often revolve around equilibrium calculations (especially ICE tables and Le Chatelier's principle), complex redox reactions, and applications of the Nernst equation.
2. Are there any specific resources you recommend beyond this blog post? Your textbook, online practice problems (like those found on websites like Khan Academy or Chegg), and past exams from your professor are invaluable resources.
3. How can I best manage my time during the exam? Allocate time proportionally to the point value of each question. Don't get stuck on a single problem; move on and return to it if time permits.
4. What if I'm struggling with a particular concept? Seek help from your professor, TA, or classmates. Utilize office hours and study groups to clarify difficult concepts.
5. Is memorization crucial for success? While some memorization is necessary (e.g., equations, definitions), a deeper understanding of the underlying principles is crucial for solving complex problems. Focus on conceptual understanding rather than rote memorization.
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Page 4 of 17. 10. According to the overall equilibrium equation above, the amount of sulfur removed may be increased by A. adding a catalyst B. removing water vapour C. increasing the volume of the system D. increasing the temperature of the system 11. As H2S (g) forms S (s), the oxidation number of sulfur A. changes from 0 to –2 and sulfur is reduced
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1 Organic Chemistry II - Jasperse FINAL EXAM PRACTICE …
2 CrO 4, PBr 3, PPh 3, BuLi, Mg, etc.) a. b. 12. Put in the starting materials for the following. (Note: May be only one chemical in several of these cases). (2 points each) a. 3 b. c. d. O O 1. NaOH, H2O 2. HCl + O HO H2N 1. LiAlH4 2. HO+ OH OH Note: Starting Material includes a ring, and has the formula C7H12O2 NaOCHO 3 CH3OH heat O H+ OO
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Final Exam Please answer the following questions clearly and concisely. In general, use pictures and less than 10 words in your answers. Write your answers in the space provided. Write your initials on each page you want graded. There are 17 total pages to this exam. The last 2 pages were intentionally left blank and may be used for scratch paper.
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submitting answers after the deadline. Please carefully note all due dates and times (found in Blackboard). There are no make-ups and no late submissions. Quizzes: There will be seven quizzes during the semester (approximately every other week) and a final quiz worth two quizzes (during our Final Exam slot on Wednesday, December 8, 11am-1pm).
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Final Exam Practical 10% Final Exam Written 20% If you score below 40% on the practical exam or the written exam, your final grade will be below a C grade (you will not be able to take Organic Chemistry I). View Grades You will be able to access your grade for the pre-lab quiz in the gradebook on NYU Classes right after completion.
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Final Exam Practice 1 Part 4 1) The decomposition of hydrogen iodide follows the equation 2HI (g) !H 2 (g) + I 2 (g) and it is second order with a rate constant of 1.6 X 10 -3 L/mol sec at 700 o C. If the initial concentration of HI in the container is 3.4 X 10 -2 M, how many seconds will it take for
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The final exam is Saturday May 15th from 12:30-2:30 pm. FINAL FORGIVENESS: The following policy applies only to students who complete all twelve in-class quizzes. In the event a student earns a higher percentage on their final exam than one of the twelve in-class quiz percentages, the final exam percentage will be substituted for that quiz grade.
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Exam I is on Tuesday 7/27, and Exam II Tuesday 8/10. Each examination will be given during the lecture time (1:40–3:10 pm). Each 90-min examination will account for 100 points. A three-hour final exam covering the entire course material will be given on Wednesday 8/18 from 1:40 – 4:40 pm. The final exam is worth 200 points.
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submitting answers after the deadline. Please carefully note all due dates and times (found in Blackboard). There are no make-ups and no late submissions. Individual Quizzes: There will be four quizzes during the semester (approximately every three weeks) and a final quiz worth two quizzes (during our Final Exam slot on Thursday, May 5, 8-10am).
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Any questions for which more than one response has been blackened will not be counted. Your score is based solely on the number of questions you answer correctly. It is to your advantage to answer every question. 1. How many oxygen atoms are in 225 g O 2? (A) 4.23 1024 (B) 6.84 24 (C) 8.47 1024 (D) 1.69 25 2.
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2 and 0.50 moles of HNO 2 in 1.0 L of water. If 0.10 mol of HCl is added to this buffer solution, the pH of the solution will get slightly . The pH does not change more drastically because the NaOH reacts with the present in the buffer solution. a) higher, NaNO 2 b) higher, HNO 2 c) lower, NaNO 2 d) lower, HNO 2 13.
Practice Exam Questions - University of Minnesota Duluth
General Microbiology Biol 4501 1 PRACTICE EXAMINATION QUESTIONS MULTIPLE CHOICE QUESTIONS Note: More than one answer can be correct. Circle all correct answers. 1. What groups listed below have true cell walls? A. algae B. mycoplasmas C. Gram-positive bacteria D. fungi E. protozoans 2. Identify which statements are correct. A.
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2) When 2-bromo -2-methybutane is treated with a base, a mixture of 2-methyl-2-butene and 2-methyl-1-butene is produced When potassium hydroxide is the base, 2 methyl-1-butene accounts for 45% of the mixture, but when potassium tert-butoxide is the base, 2 methyl-1-butene accounts for 70% of the mixture.
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INTRODUCTORY ANALYTICAL CHEMISTRY - University of …
11 Sep EXAM 16 Sep – 9 Oct Chemical Equilibrium Ch 6-11 14 Oct EXAM 16 Oct-30 Oct Electrochemistry and Spectrophotometry Ch14-17, Ch 18-21 4 Nov EXAM 6 Nov – 18 Nov Chromatography Ch 23-26 20 Nov EXAM 2-4 Dec Mass Spectrometry Ch 22 11 Dec FINAL EXAM 6:00 PM, RM 154 CHVN
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2Cl 2? (A) 3.36 ´ 1023 (B) 6.72 23 (C) 1.34 ´ 1024 (D) 4.28 ´ 1024 4. A 2024 US penny (which is a mixture of zinc and copper) is dissolved in dilute nitric acid, forming aqueous Cu2+ and Zn2+ ions. The resulting solution is treated with an excess of iodide ion, causing the Cu2+ to react to form CuI(s) and I 3 –(aq). Subsequent titration ...
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MULTIPLE CHOICE: This exam contains 80 multiple choice questions. Read each question and their corresponding answers completely and carefully. Choose the best answer and mark the corresponding letter choice on your answer sheet. Directions: Use the diagrams below to answer questions 1 – 2 _____1. The diagram shows a plant cell and an animal cell.
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7. “Visualization: Chemistry constructs meaning interchangeably at the particulate and macroscopic levels.” Common hour exam dates Exam I : October 06, Thursday : Time 9.20-10.40 pm Exam II: November 03, Thursday :Time 9.20-10.40 pm Exam III : December 06 Tuesday : Time 9.20-10.40 pm Final Exam: TBA
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5. ALKYNE. 2-butyne, CH 3 CCCH 3-draw Lewis structure first 6. WATER. H 2 O 7. ALCOHOL. Ethanol, CH 3 CH 2 OH 8. ETHER. Diethyl ether, CH 3 CH 2 OCH 2 CH 3 1 2 Test 1 P S# 3: 3-D Structure-Drawing P ractice Set
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Eastern Kentucky University Department of Chemistry …
Final Exam. The final exam will be held on . Tuesday, December 13, 2016, from 3:30 – 5:30 pm. This exam is a joint final exam for all CHE 112 students. It is a comprehensive, standardized ACS exam and no make-up will be available. Any student who does not take the final exam will automatically receive a grade of F for the course.
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