CHEM 101 Fall 09 Exam 1 (a)
|
|
|
- Anastasia Watson
- 5 years ago
- Views:
Transcription
1 CHEM 101 Fall 09 Exam 1 (a) On the answer sheet (scantron) write your name, student ID number, and recitation section number. Choose the best (most correct) answer for each question and enter it on your answer sheet. 1. Please choose the letter a as your answer for this question. Potentially useful data: Avogadro s number: x Speed of light: c = 3.00 x 10 8 m/s Planck constant: h = x J s E = hc/λ = hν 2. All of the following properties of a substance can aid in its identification except: a. density. b. temperature. c. reactivity. d. melting point. e. boiling point. 3. Which of the following is a chemical property of iron? a. Iron conducts heat. b. Iron conducts electricity. c. Iron melts at 1535 C. d. Iron can be bent into shapes. e. Iron rusts on exposure to water and oxygen. 4. Which is the best definition of a pure substance? a. A material that contains two or more types of atoms. b. A material in the gas phase. c. A material whose properties cannot be changed by further physical separation. d. A material whose properties have been measured. e. A material that has been heated. 5. All atoms of a given element are chemically identical. This is an example of: a. The Law of Conservation of Mass. b. Dalton's Atomic Theory. c. The Law of Constant Composition. d. The Law of Multiple Proportions. e. The Law of Conservation of Energy. Page 1 of 5
2 6. The Millikan oil drop experiment was used to determine a. whether the atom was radioactive. b. the electron distribution in the atom. c. the atomic number of an atom. d. the charge of an electron. e. the nuclear character of the atom. 7. Calculate the number of grams in moles of nitrogen molecules (N 2 ). a g b g c g d g e g 8. How many grams of argon (Ar) contain the same number of atoms as 27 g of aluminum (Al)? a. 18 g b. 27 g c. 31 g d. 40 g e. 67 g 9. How many hydrogen atoms are in a 27.0 g sample of water (H 2 O)? a b c d e Which sample contains the greatest number of atoms? a. 50 g Ba b. 50 g Br c. 50 g Ca d. 50 g Ti e. 50 g P 11. Which element can be classified as a transition metal? a. Ar b. N c. F d. Co e. Rb Page 2 of 5
3 12. Which of the following is not an ionic compound? a. TiO 2 b. KMnO 4 c. CH 4 d. Na 2 SO 3 e. Ca(CH 3 COO) What are the products of the dissolution of NaH 2 PO 4 (s) in water? a. NaH PO 4 3- b. Na + + 2H + + P + 4O 2- c. Na + + H 2 + P + 2O 2 d. Na + + H 2 PO 4 - e. Na + + H + + P + O Determine the number of molecules in 325 mg of aspirin, C 9 H 8 O 4. a b c d e In the reaction given below, how many grams of sodium metal are consumed if 2.02 g of hydrogen gas are produced? 2 Na(s) + 2 H 2 O(l) 2 NaOH(aq) + H 2 (g) a g b g c g d g e g 16. Classify the following reaction. 2 Al(s) + 3 CuSO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 3 Cu(s) a. combination b. decomposition c. combustion d. dissolution e. displacement Page 3 of 5
4 17. The Roman numerals in the reaction given represent the coefficients in the balanced chemical equation. What are the values of the coefficients? I II III IV a b c d e I CH 3 OH + II O 2 III CO 2 + IV H 2 O 18. How many moles of ammonia will be formed from the complete reaction of 45.0 g of H 2? N H 2 2 NH 3 a mol b mol c mol d mol e mol 19. How many grams of MgI 2 are produced by the reaction of 25.0 g of Mg with 25.0 g of I 2? Mg + I 2 MgI 2 a g b g c g d g e. 195 g 20. Which substance gets reduced in the reaction below? Na 2 SO C Na 2 S + 4 CO a. CO b. C c. Na 2 S d. Na 2 SO 4 e. this is not an oxidation-reduction reaction 21. What is the oxidation number of P in PO 4 3-? a. +5 b. +3 c. -2 d. -3 e. -5 Page 4 of 5
5 22. Which of the following reactions are oxidation reduction reactions? I) Ca + 2 H 2 O Ca(OH) 2 + H 2 II) CaO + H 2 O Ca(OH) 2 III) Ca(OH) 2 + H 3 PO 4 Ca 3 (PO 4 ) 2 + H 2 O IV) Cl KBr Br KCl a. I and II b. II and III c. I and IV d. III and IV e. I and III 23. Determine the volume of solution that contains 15.0 g of AgNO 3 if the solution is M. a ml b ml c. 235 ml d. 447 ml e. 956 ml 24. Dental lasers are based on neodymium yttrium aluminum garnet (Nd-YAG) crystal, with an emission wavelength of 1066 nm. What is the frequency of this laser? a Hz b Hz c Hz d Hz e Hz 25. Which statement below is false? a. The wavelength of light is the distance between two corresponding points in the wave pattern. b. The frequency of light is the number of waves that pass a given point in a second. c. The frequency of light increases as wavelength decreases. d. The higher the frequency of light, the greater its energy. e. The higher the frequency of light, the longer the wavelength. 26. Of the following, radiation has the longest wavelength and radiation has the greatest energy. gamma ultraviolet visible a. ultraviolet, gamma b. visible, ultraviolet c. gamma, gamma d. visible, gamma e. gamma, visible Page 5 of 5
6 CHEM101 Exam 1 Answer Section MULTIPLE CHOICE 1. ANS: A PTS: 0 2. ANS: B PTS: 1 3. ANS: E PTS: 1 4. ANS: C PTS: 1 5. ANS: B PTS: 1 6. ANS: D PTS: 1 7. ANS: D PTS: 1 8. ANS: D PTS: 1 9. ANS: D PTS: ANS: E PTS: ANS: D PTS: ANS: C PTS: ANS: D PTS: ANS: B PTS: ANS: E PTS: ANS: E PTS: ANS: C PTS: ANS: B PTS: ANS: C PTS: ANS: D PTS: ANS: A PTS: ANS: C PTS: ANS: C PTS: ANS: B PTS: ANS: E PTS: ANS: D PTS: 1 Page 6 of 5
CHEM 101 Fall 09 Final Exam (a)
CHEM 101 Fall 09 Final Exam (a) On the answer sheet (scantron) write your name, student ID number, and recitation section number. Choose the best (most correct) answer for each question and enter it on
CHEM 101 Fall 08 Exam II(a)
CHEM 101 Fall 08 Exam II(a) On the answer sheet (scantron) write you name, student ID number, and recitation section number. Choose the best (most correct) answer for each question and enter it on your
Chem 101 Practice Exam 3 Fall 2012 You will have a Solubility Table and Periodic Table
Chem 101 Practice Exam Fall 01 You will have a Solubility Table and Periodic Table 1. A 1.6-mol sample of KClO was decomposed according to the equation KClO (s) KCl(s) O (g) How many moles of O are formed
What is one of the spectator ions (with correct coefficient)? A)
Chem 101 Exam Fall 01 Section 001 1. Based on the solubility rules Mg (PO 4 ) is A) soluble B) insoluble. An aqueous solution of potassium sulfate is allowed to react with an aqueous solution of What is
Chem 205: GENERAL CHEMISTRY I MIDTERM EXAMINATION
Concordia University CHEM 205 Winter 2007 -- MIDTERM EXAM Student ID #: Chem 205: GENERAL CHEMISTRY I MIDTERM EXAMINATION PLEASE READ THIS WHILE WAITING TO START INSTRUCTIONS: This test paper includes
CHEMISTRY 101 EXAM 1 FORM 1J
CHEMISTRY 101 EXAM 1 SECTIONS 540-550 Dr. Joy Heising FORM 1J September 26, 2003 Directions: 1. This examination consists of two parts: 17 multiple choice questions (4 points each) in Part 1 and 3 free
CHEM 101 Fall 08 Exam III(a)
CHEM 101 Fall 08 Exam III(a) On the answer sheet (scantron) write you name, student ID number, and recitation section number. Choose the best (most correct) answer for each question and enter it on your
Unit 4: Reactions and Stoichiometry
Unit 4: Reactions and Stoichiometry Reactions Chemical equation Expression representing a chemical reaction Formulas of reactants on the left side Formulas of products on the right side Arrow(s) connect(s)
Chem 105 Final Exam. Here is the summary of the total 225 points plus 10 bonus points. Carefully read the questions. Good luck!
May 3 rd, 2012 Name: CLID: Score: Chem 105 Final Exam There are 50 multiple choices that are worth 3 points each. There are 4 problems and 1 bonus problem. Try to answer the questions, which you know first,
ICP Final Exam Review - Part 2
ICP Final Exam Review - Part 2 Modified True/False Indicate whether the statement is true or false. If false, change the identified word or phrase to make the statement true. 1. A combustion reaction occurs
CHEM 60 Spring 2016 Exam 2 Ch 5-8, 100 points total.
Name Exam No. F CHEM 60 Spring 2016 Exam 2 Ch 5-8, 100 points total. Multiple Choice. (20 questions, 3 points each = 60 points total) Mark the letter on the scantron form corresponding to the one best
Chemistry Final Exam Sample Items
Chemistry Final Exam Sample Items 1. Which best describes the current atomic theory? a. Atoms consist of electrons circling in definite orbits around a positive nucleus. b. Atoms are composed of electrons
CHEMISTRY 101 EXAM 1 FORM 1N
CHEMISTRY 101 EXAM 1 SECTIONS 572-580 Dr. Joy Heising FORM 1N September 20, 2001 Directions: 1. Fill out your scantron sheet. a. Do not forget to include your SIGNATURE and ID number. b. Dept = CHEM, Course
Bonding Mrs. Pugliese. Name March 02, 2011
Bonding Mrs. Pugliese Name March 02, 2011 1. Atoms of which element have the greatest tendency to gain electrons? 1. bromine 3. fluorine 2. chlorine 4. iodine 2. Which polyatomic ion contains the greatest
General Chemistry I Final Exam 100 pts Fall 2010
General Chemistry I Final Exam 100 pts Fall 2010 Name This is a closed-book exam: the only reference materials you may use are a periodic table of the elements, a table of enthalpies of formation, and
(DO NOT WRITE ON THIS TEST)
Final Prep Chap 8&9 (DO NOT WRITE ON THIS TEST) Multiple Choice Identify the choice that best completes the statement or answers the question. 1. After the correct formula for a reactant in an equation
b. Na. d. So. 1 A basketball has more mass than a golf ball because:
Chem I Semester Review All of the following are general characteristics of a substance in the liquid state except a. definite volume. c. not easily compressed. b. able to flow. d. definite shape. In the
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
CHM1025 Exam 4 Chapters 9, 10, & 13 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which of the following statements is false? 1) A) The percent
CHE 105 EXAMINATION II October 13, 2011
CHE 105 EXAMINATION II October 13, 2011 University of Kentucky Department of Chemistry READ THESE DIRECTIONS CAREFULLY BEFORE STARTING THE EXAMINATION! It is extremely important that you fill in the answer
Final S2 (2011) - Practice Test - Ch 11, 12, 13, 14, 15, 16, 18, 19, 22, 23
Final S2 (2011) - Practice Test - Ch 11, 12, 13, 14, 15, 16, 18, 19, 22, 23 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. If 12.0 g of a gas at 2.5 atm
Chemistry CRT Study Guide First Quarter
Number AL COS # 1. #1.0 Classify sodium chloride as an element, mixture, compound, or colloid. Compound 2. #1.0 Classify air as an element, mixture, compound, or colloid. Mixture 3. #1.0 Classify a blueberry
Chemistry Final Exam Review
Chemistry Final Exam Review Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. All of the following are physical properties of matter EXCEPT.
Section EXAM III Total Points = 150. November 15, Each student is responsible for following directions. Read this page carefully.
Name Chemistry 11100 Test 66 Section EXAM III Total Points = 150 TA Thursday, 8:00 PM November 15, 2012 Directions: 1. Each student is responsible for following directions. Read this page carefully. 2.
Ch 9 Stoichiometry Practice Test
Ch 9 Stoichiometry Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A balanced chemical equation allows one to determine the a. mole ratio
Name AP Chemistry September 30, 2013
Name AP Chemistry September 30, 2013 AP Chemistry Exam Part I: 40 Questions, 40 minutes, Multiple Choice, No Calculator Allowed Bubble the correct answer on the blue side of your scantron for each of the
CP Chemistry Midterm Topic List
CP Chemistry Midterm Topic List Converting SI Units (Kilo, Hecto, Deca, Base Unit, Deci, Centi, Milli) Scientific Notation Precision versus Accuracy Properties of Matter Classification of Matter (Element/Compound/Mixture)
Name Date Class THE ARITHMETIC OF EQUATIONS
12.1 THE ARITHMETIC OF EQUATIONS Section Review Objectives Calculate the amount of reactants required or product formed in a nonchemical process Interpret balanced chemical equations in terms of interacting
Chem A Ch. 9 Practice Test
Name: Class: Date: Chem A Ch. 9 Practice Test Matching Match each item with the correct statement below. a. product d. balanced equation b. reactant e. skeleton equation c. chemical equation 1. a new substance
Honors text: Ch 10 & 12 Unit 06 Notes: Balancing Chemical Equations
Notes: Balancing Chemical Equations Effects of chemical reactions: Chemical reactions rearrange atoms in the reactants to form new products. The identities and properties of the products are completely
Worksheet 1: REPRESENTATIVE PARTICLES
Worksheet 1: REPRESENTATIVE PARTICLES Directions: For each substance below, state the representative particle. If the RP is a molecule, state the number of atoms that make up the molecule. If the RP is
CHEMISTRY Midterm #2 October 26, Pb(NO 3 ) 2 + Na 2 SO 4 PbSO 4 + 2NaNO 3
CHEMISTRY 123-02 Midterm #2 October 26, 2004 The total number of points in this exam is 100. The total exam time is 50 min. Good luck! PART I: MULTIPLE CHOICE (Each multiple choice question has a 2-point
Chemistry 231 Fall 2014 Oregon State University Final Exam December 8, 2014 Drs. Nafshun, Watson, Nyman, Barth, Burand
Chemistry 231 Fall 2014 Oregon State University Final Exam December 8, 2014 Drs. Nafshun, Watson, Nyman, Barth, Burand Instructions: You should have with you several number two pencils, an eraser, your
Name: Chemistry 400: General Chemistry Miller Exam I September 20, 2017 Approximately 150 points
Name: Chemistry 400: General Chemistry Miller Exam I September 20, 2017 Approximately 150 points Please answer each of the following questions to the best of your ability. If you wish to receive partial
Answer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide
Answer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide Electrons in Atoms Chapter 5 1. What is the frequency of green light, which has a wavelength of 4.90 x 10-7 m? 8 c 3.00x10
Student Name: Teacher: Date: District: NCGaston. Assessment: 9_12 Science Chemistry Exam 3. Description: Chemistry Mock Final Exam
Student Name: Teacher: Date: District: NCGaston Assessment: 9_12 Science Chemistry Exam 3 Description: Chemistry Mock Final Exam 2014-15 Form: 301 1. Shown below is a model of the structure of atom X.
Unit 5 Chemical Reactions Notes. Introduction: Chemical substances have physical and chemical properties
Unit 5 Chemical Reactions Notes Introduction: Chemical substances have physical and chemical properties Physical Properties 2 Types of Physical Properties Extensive Physical Properties Intensive Physical
CH 221 Sample Exam Exam II Name: Lab Section:
Exam II Name: Lab Section: Part I: Multiple Choice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. When methanol undergoes complete combustion,
CHEM 101 WINTER FINAL EXAM
CHEM 101 WINTER 08-09 FINAL EXAM On the answer sheet (Scantron) write you name, student ID number, and recitation section number. Choose the best (most correct) answer for each question and enter it on
Name Date Class. Match each term in Column B with the correct description in Column A. Write the letter of the correct term on the line.
12 STOICHIOMETRY Chapter Test B A. Matching Match each term in Column B with the correct description in Column A. Write the letter of the correct term on the line. 1. 2. 3. 4. 5. Column A the substance
Chemistry Section Review 7.3
Chemistry Section Review 7.3 Multiple Choice Identify the choice that best completes the statement or answers the question. Put the LETTER of the correct answer in the blank. 1. The molar mass of an element
2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with
Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12
Practice Multiple Choice
Practice Multiple Choice 1. A theory differs from a hypothesis in that a theory A. cannot be disproved C. always leads to the formation of a law B. represents an educated guess D. has been subjected to
Exam 2. Name: Class: Date:
Class: Date: Exam 2 Multiple Choice Identify the choice that best completes the statement or answers the question. Record your name on the top of this exam and on the scantron form. Record the test ID
CHEMISTRY 15 EXAM II-Version A (White)
CHEMISTRY 15 EXAM II-Version A (White) Dr. M. Richards-Babb June 8, 2001 An optical scoring machine will grade this examination. The machine is not programmed to accept the correct one of two sensed answers
NAME: SECTION #: Fill in your A00 number and name correctly on the scantron. Attempt all the questions and fill in the bubbles with your answers.
NAME: SECTION #: Chemistry 111 EXAM 2- Fall 2013 10/25/2013/12:00PM/Odago Fill in your A00 number and name correctly on the scantron. Attempt all the questions and fill in the bubbles with your answers.
Chapter 3: Stoichiometry
Chapter 3: Stoichiometry Chem 6A Michael J. Sailor, UC San Diego 1 Announcements: Thursday (Sep 29) quiz: Bring student ID or we cannot accept your quiz! No notes, no calculators Covers chapters 1 and
5. What is the name of the compound PbO? 6. What is the name of HCl(aq)?
1. Which idea of John Dalton is no longer considered part of the modern view of atoms? (A) Atoms are extremely small. (B) Atoms of the same element have identical masses. (C) Atoms combine in simple whole
Types of chemical reactions
PowerPoint to accompany Types of chemical reactions Chapters 3 & 16.1 M. Shozi CHEM110 / 2013 General Properties of Aqueous Solutions Solutions are mixtures of two or more pure substances. The solvent
The photograph in the textbook provides evidence that an exothermic chemical reaction is occurring.
Preview Lesson Starter Objectives Indications of a Chemical Reaction Characteristics of Chemical Equations Significance of a Chemical Equation Balancing Chemical Equations Section 1 Describing Chemical
Chem 101 Review. Fall 2012
Chem 101 Review Fall 2012 Elements, Atoms, Ions Elements in nature symbols Constant composition chemical formula Dalton s atomic theory Atomic structure what makes up the atom ions isotopes Periodic table
Name. Practice Test 2 Chemistry 111
Name Practice Test 2 Chemistry 111 1) In the aqueous reaction of K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) BaSO 4 (s) + 2KNO 3 (aq), which ions are the spectator ions? A) Ba 2+ 2- and SO 4 B) Ba 2+ and K + C) Ba
When reading Chapter 4: Skip p (Balancing Redox Equations/Redox Titrations)
Announcements When reading Chapter 4: Skip p. 154-157 (Balancing Redox Equations/Redox Titrations) On to Chapter 5 today (Gases) Hour Exam 2 Aug 26 Goal is to cover up to and include Chapter 6.2-6.5 Don
General Chemistry Multiple Choice Questions Chapter 8
1 Write the skeleton chemical equation for the following word equation: Hydrochloric acid plus magnesium yields magnesium chloride and hydrogen gas. a HClO 4 + Mg --> MgClO 4 + H 2 b HClO 4 + Mg --> MgClO
Name: Class: Date: SHORT ANSWER Answer the following questions in the space provided.
CHAPTER 9 REVIEW Stoichiometry SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. The coefficients in a chemical equation represent the (a) masses in grams of all reactants
Chemical Reactions. Writing chemical reactions Types of chemical reactions Reactions in aqueous solutions. (ionic equations and solubility rules)
Chemical Reactions Writing chemical reactions Types of chemical reactions Reactions in aqueous solutions (ionic equations and solubility rules) Writing Equations REACTANTS PRODUCTS gold (III) sulfide is
Moles Revisited Name Date Molar Mass How do you calculate the formula mass of a compound? Examples Potassium fluoride Strontium nitrate Aluminum nitri
Moles Revisited Name Date Molar Mass How do you calculate the formula mass of a compound? Examples Potassium fluoride Strontium nitrate Aluminum nitride Magnesium phosphate Mole Conversions One-step How
Gas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T
Name Period Teacher Practice Test: OTHS Academic Chemistry Spring Semester 2017 The exam will have 100 multiple choice questions (1 point each) Formula sheet (see below) and Periodic table will be provided
How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? How many neutrons are there in one atom of 24 Mg?
1 A 2 B 3 C The atomic number of Na is 11. How many electrons are there in a sodium ion, Na +? How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? What is the mass in grams
OPTIONAL PRACTICE PROBLEMS
OPTIONAL PRACTICE PROBLEMS 1 DIMENSIONAL ANALYSIS AND PROPERTIES OF MATTER (1) List the base (fundamental) SI units: (2) Fill in the following table: Object Weight, g Mass, g Piece of iron 50 g? Huge container
Solubility Rules See also Table 4.1 in text and Appendix G in Lab Manual
Ch 4 Chemical Reactions Ionic Theory of Solutions - Ionic substances produce freely moving ions when dissolved in water, and the ions carry electric current. (S. Arrhenius, 1884) - An electrolyte is a
4) Tetrasulfur trioxide. 5) barium fluoride. 6) nitric acid. 7) ammonia
Unit 9: The Mole- Funsheets Part A: Molar Mass Write the formula AND determine the molar mass for each of the following. Be sure to include units and round you answer to 2 decimal places. 1) calcium carbonate
Chapter 4. Reactions in Aqueous Solutions. Chemistry, Raymond Chang 10th edition, 2010 McGraw-Hill
Chemistry, Raymond Chang 10th edition, 2010 McGraw-Hill Chapter 4 Reactions in Aqueous Solutions Ahmad Aqel Ifseisi Assistant Professor of Analytical Chemistry College of Science, Department of Chemistry
Name. Academic Chemistry Stoichiometry Notes. Unit #10 Test Date: cincochem.pbworks.com
Name Academic Chemistry Stoichiometry Notes Unit #10 Test Date: cincochem.pbworks.com Resources Unit 10 Common Polyatomic Ions List 20 Name Common Polyatomic Ion Ions Name Ion acetate C 2 H 3 O 2 or CH3
Chemical Reactions. Burlingame High School Chemistry 1
Chemical Reactions 1 Chemical Equations Chemical equations are use to describe: the substances that react, the reactants the substances that are formed, the products the relative amounts of all substances
Chemistry 1A Midterm Exam 1 February 12, Potentially Useful Information. Violet Blue Green Yellow Orange Red Wavelength (nm)
Chemistry 1A Midterm Exam 1 February 12, 2013 Professor Pines 5 pages total Student Name: Student ID#: Potentially Useful Information Violet Blue Green Yellow Orange Red 400 500 600 700 Wavelength (nm)
Unit 5. Chemical reactions
Unit 5. Chemical reactions Index 1.- Physical and chemical phenomena...2 2.- What is a chemical reaction?...2 2.1. Chemical equation...2 2.2.- Balance of chemical reactions. Law of conservation of mass...3
TA Wednesday, 3:20 PM Each student is responsible for following directions. Read this page carefully.
Name Chemistry 111 Section FINAL EXAM Total Points = TA Wednesday, 3:20 PM 200 Directions: December 12, 2007 1. Each student is responsible for following directions. Read this page carefully. 2. Write
!!! DO NOT OPEN THIS EXAM BOOK UNTIL TOLD TO DO SO BY THE INSTRUCTOR!!!
CHEM 142 - Exam 1 Version B!!! DO NOT OPEN THIS EXAM BOOK UNTIL TOLD TO DO SO BY THE INSTRUCTOR!!! Instructor: Dr. Kari Pederson NO GRAPHING CALCULATORS ALLOWED Date: Friday, July 15 ONLY CALCULATORS MAY
Slide 1 / Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy. a only b only c only a and c b and c
Slide 1 / 84 1 Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy A B C D E a only b only c only a and c b and c Slide 2 / 84 2 The internal energy of a system
Introductory Chemistry I Chemistry 1111 September 17, 2009 Hour Examination I Name There is a Periodic Table and a summary of solubility rules attached to the end of this examination. You may use a non-programmed
Chemistry 1210, Section 3, Fall semester 2012 Second Hour Exam October 24, 2012 Dr. Scott Ensign ExamVersion 0001
Chemistry 1210, Section 3, Fall semester 2012 Second Hour Exam October 24, 2012 Dr. Scott Ensign ExamVersion 0001 Instructions: Be sure to mark the exam version number (0001) on your scantron Do not begin
Reactions. Chapter 3 Combustion Decomposition Combination. Chapter 4 Reactions. Exchange reactions (Metathesis) Formation of a precipitate
Reactions Chapter 3 Combustion Decomposition Combination Chapter 4 Reactions Exchange reactions (Metathesis) Formation of a precipitate Formation of a gas Formation of a week or nonelectrolyte Single Displacement
Identification Sticker
Chemistry 1A Midterm Exam 1 September 20, 2001 Page 1 of 10. (Closed Book, 90 minutes, 150 points) Version D Name: TA: SID: Section: Identification Sticker Test-taking strategy: PLEASE READ THIS FIRST!
Attention: Please study problem set 1, 2, 5 and 6 as well. This review does not contain these chapters.
Chemistry 101 Review for Final Attention: Please study problem set 1, 2, 5 and 6 as well. This review does not contain these chapters. 1. Use the following ions to write the chemical formula for each ionic
Which of the following answers is correct and has the correct number of significant figures?
Avogadro s Number, N A = 6.022 10 23 1. [7 points] Carry out the following mathematical operation: 6.06 10 3 + 1.1 10 2 Which of the following answers is correct and has the correct number of significant
The Mole. Relative Atomic Mass Ar
STOICHIOMETRY The Mole Relative Atomic Mass Ar Relative Molecular Mass Mr Defined as mass of one atom of the element when compared with 1/12 of an atom of carbon-12 Some Ar values are not whole numbers
Chem 115 Sample Examination #3
_ Chem 115 Sample Examination #3 Student Number: This exam consists of seven (7) pages, including this cover page. Be sure your copy is complete before beginning your work. If this test packet is defective,
GENERAL PRINCIPLES OF CHEMISTRY CHEM 110/CHEM 195 TEST 1
GENERAL PRINCIPLES OF CHEMISTRY CHEM 110/CHEM 195 TEST 1 Date: THURSDAY, 14 March 2013 Total marks: 25 Time: 17h45 18h30 IMPORTANT: Complete this part immediately. Name: Student No: Tutorial Day: Tutorial
5) Which statement correctly describes the relationship of wavelength and frequency in a wave?
Exam 2 Name: Multiple Choice (2 pts each) 1) Which of the following bonds is the most polar? a) C O b) N O c) O O d) Si O 2) The maximum electron capacity of an f sublevel is a) 7 c) 14 b) 6 d) 10 3) Which
Usual Atomic Charges of Main Group Elements
Usual Atomic Charges of Main Group Elements +1 +2 +3 +4 +5 +6 +7-5 -4-3 -2-1 Examples SO 3 sulfur trioxide CO 2 carbon dioxide Al 2 O 3 aluminum trioxide IF 7 iodine heptafluoride Fig. 2-6, p.63 Chemical
(50 pts.) 26. (24 pts.) 27. (8 pts.) 28. (18 pts.) TOTAL (100 points)
Moorpark College Chemistry 11 Spring 2011 Instructor: Professor Torres Examination #2: Section Two March 12, 2011 Name: (print) Name: (sign) Directions: Make sure your examination contains ELEVEN total
Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON
Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON Name /80 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments by changing the
Class XI Chapter 1 Some Basic Concepts of Chemistry Chemistry
Question 1.1: Calculate the molecular mass of the following: (i) H 2 O (ii) CO 2 (iii) CH 4 (i) H 2 O: The molecular mass of water, H 2 O = (2 Atomic mass of hydrogen) + (1 Atomic mass of oxygen) = [2(1.0084)
Chem 121 Final Exam. (2) 1) A cube measures 3.21 cm on one side. Calculate its volume in liters (cm 3 = ml) and put the answer in the box.
Chem 121 Final Exam Page 1 of 13 (2) 1) A cube measures 3.21 cm on one side. Calculate its volume in liters (cm 3 = ml) and put the answer in the box. (2) 2) The charge on a phosphorus atom is neutral
CH1410 Practice Exam #2 (Katz)
CH1410 Practice Exam #2 (Katz) Section 1 - Multiple Choice - Write the letter of the BEST CHOICE in the space provided. 1. How are wavelength and frequency of light related? A) Wavelength is one-half of
Lab Chemistry - Final Exam Review 1. Express in scientific notation. A) D) B) E) C)
Lab Chemistry - Final Exam Review 1. Express 30554000 in scientific notation. A) 3 10 7 D) 30554 10 3 B) 3.0554 10 7 E) 305540 10 7 C) 306 10 7 2. What is the result of the following multiplication expressed
Chem 42 Final Review Sheet Mr. J. Fassler Spring 2018
Chem 42 Final Review Sheet Mr. J. Fassler Spring 2018 These problems are given to help you review concepts you may have forgotten. Old tests, quizzes and review sheets are also important in studying. Chapter
Chemistry Released Questions
Name: Date: 1. What was Niels Bohr s prediction about the location of the electrons in an atom? 3. An atom with which atomic diagram has chemical properties most similar to calcium? A. Electrons pair with
Unit 5: Chemical Equations and Reactions & Stoichiometry
pg. 10 Unit 5: Chemical Equations and Reactions & Stoichiometry Chapter 8: Chemical Equations and Reactions 8.1: Describing Chemical Reactions Selected Chemistry Assignment Answers (Section Review on pg.
Chapter 1 IB Chemistry Warm Ups Stoichiometry. Mrs. Hilliard
Chapter 1 IB Chemistry Warm Ups Stoichiometry Mrs. Hilliard Vocabulary 1. Atomic theory 2. Kelvin 3. Mole 4. Relative abundance 5. Molar Mass 6. Empirical formula 7. Molecular formula 8. Stoichiometry
Reactions in Aqueous Solution
1 Reactions in Aqueous Solution Chapter 4 For test 3: Sections 3.7 and 4.1 to 4.5 Copyright The McGrawHill Companies, Inc. Permission required for reproduction or display. 2 A solution is a homogenous
3) What is the correct value for Avogadro's number? 3) A) x 1033 B) x 1023 C) x D) x 1022
CHM1025 Exam 3 Chapters 6, 7, & 8 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) How many hydrogen atoms are in 35.0 grams of hydrogen gas? 1)
Chapter 3: Stoichiometry
Chapter 3: Stoichiometry Key Skills: Balance chemical equations Predict the products of simple combination, decomposition, and combustion reactions. Calculate formula weights Convert grams to moles and
1.) The answer to question 1 is A. Bubble in A on your Scantron form.
Part 1: Multiple Choice. (5 pts each, 145 pts total) Instructions: Bubble in the correct answer on your Scantron form AND circle the answer on your exam. Each question has one correct answer. 1.) The answer
Chapter 4 Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Homework Chapter 4 11, 15, 21, 23, 27, 29, 35, 41, 45, 47, 51, 55, 57, 61, 63, 73, 75, 81, 85 1 2 Chapter Objectives Solution To understand the nature of ionic substances
Unit 1 - Foundations of Chemistry
Unit 1 - Foundations of Chemistry Chapter 2 - Chemical Reactions Unit 1 - Foundations of Chemistry 1 / 42 2.1 - Chemical Equations Physical and Chemical Changes Physical change: A substance changes its
Chem. 1A Midterm 2 Version A
Chem. 1A Midterm 2 Version A Name Student Number All work must be shown on the exam for partial credit. Points will be taken off for incorrect or no units and for the incorrect number of significant figures.
Chem 127, Final Exam December 13, 2002
I. (55 points) This part of the final corresponds to Exam I. It covers the material in Chapters 1, 2 and 3. A. (20 points) The following questions are NOT related to each other. 1. Express 1 part per million
Name: Class: Date: ID: A. (g), what is the ratio of moles of oxygen used to moles of CO 2 produced? a. 1:1 b. 2:1 c. 1:2 d. 2:2
Name: Class: _ Date: _ Chpt 12 review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. What is conserved in the reaction shown below? H 2 + Cl 2 2HCl a.
Stoichiometry is the relationship between the amount of reactants used and/or the amount of products produced in a chemical reaction.
Unit 7 STOICHIOMETRY 1. Introduction to Stoichiometry 2. Mole Mole Stoichiometry 3. Mass Mole Stoichiometry 4. Mass Mass Stoichiometry 5. Mass Volume & Volume Volume Stoichiometry 6. Excess & Limiting