Autumn Semester. Basic Chemistry for Engineering/ Fundamental Inorganic Chemistry Final Exam. 18 February Time: 60 minutes
|
|
- Brook Walton
- 5 years ago
- Views:
Transcription
1 Basic Chemistry Final Exam 1 Name: Student number: Instructions: Autumn Semester Basic Chemistry for Engineering/ Fundamental Inorganic Chemistry Final Exam 18 February 2013 Time: 60 minutes Answer any 4 questions out of 5 possible questions. You may answer more than 4 questions if you wish. Your marks will be taken from your top 4 questions. Show all relevant working. Write all answers and final working in pen. Give your answers to an appropriate number of significant figures. 9 pages including: 1 top page, 1 data page, 1 periodic table, 5 question pages, 1 page for rough working Hand in all pages at the end of the exam. Permissible materials: Calculator. English or English bilingual Dictionary.
2 Basic Chemistry Final Exam 2 Avagadro number x Equations and Data pv = nrt where p = pressure, V = volume, n= no. of moles, R = ideal gas constant T = temperature R = J K 1 mol 1 or R = L atm K 1 mol 1 H rxn = H f products H f reactants Density of water: 1.0 g ml 1 Enthalpies of formation CH 4(g) : 74.9 kj mol 1 HCCH (g) : kj mol 1 H 2 (l) : kj mol 1 H 2 2(l) : kj mol 1 H 3 P 4(l) : 1288 kj mol 1 PCl 3(l) : 320 kj mol 1 Latent heat of fusion (heat of forming a liquid from a solid) of Na 2 CCH 3 : 22.9 kj mol 1
3 Basic Chemistry Final Exam 3
4 Basic Chemistry Final Exam 4 Question 1 A) An inventor asks a bank to invest in a new kind of heater that uses water as a fuel. He claims the engine burns water to generate heat using oxygen and a secret catalyst. He says the reaction occurs according to the following equation: 2H 2 (l) + 2(g) > 2H 2 2(l) i) Use data from the data sheet to calculate the enthalpy change, per mole of H 2, for this reaction. iii) Which of the following words best describes the above reaction? Circle the answer. exothermic concentrated dilute endothermic spontaneous iii) Do you predict the entropy change for this reaction would be positive or negative? Why? iv) Should the bank invest in this heater? Why? B) A pocket hand warmer pouch contains a supersaturated solution of 170 g sodium acetate (Na 2 CCH 3 ) dissolved in 100 ml water. When the pouch is activated, 134 g of Na 2 CCH 3 crystallises out of solution. i) Using data from the data sheet, calculate the enthalpy change of this crystallisation process. [1] _ [3]
5 Basic Chemistry Final Exam 5 Question 2 A) i) What is the chemical formula of the following compounds? (Write C n H m followed by other elements, e.g. C 2 H 4 2 ) H 3 C CH 3 N NH 2 H 3 C CH 3 CH 3 ii) Identify pairs of isomers. If no isomer exists, circle 'No isomer'. [4] H H a) b) c) d) e) Isomer with: or: No isomer No isomer No isomer No isomer No isomer [4] B) Choose your answers from the molecules bearing the following functional groups: H NH 2 Cl a) b) c) d) i) Which molecule can exist as geometrical isomers? ii) Which molecule bears the most easily-detachable functional group?
6 Basic Chemistry Final Exam 6 Question 3 A) Choose the most appropriate concentration measure from the following list to complete parts i) iv). molarity, molality, percentage by weight, percentage by volume, parts per million i) Reporting the amount of flavour syrup in a sweet drink. ii) Measuring the effect of a solute on solvent vapour pressure across a range of temperatures. iii) Calculating the volume of solution needed for a chemical reaction. iv) Reporting levels of trace pollutants in the atmosphere. [4] B) Refer to the following chart of solubility: i) Demonstrate, using calculations, whether it is, or is not, possible to make a 12M aqueous solution of potassium chloride (KCl). [3] You will need one or more of the following terms for part ii): concentrated dilute dissolve saturated precipitate ii) Na 2 S 4 is dissolved in water at 30 C until no more will dissolve. At this point, the solution is. The solution is heated to boiling which makes some Na 2 S 4. iii) Will the Na 2 S 4 solution boil at exactly 100 C? Why? [1]
7 Basic Chemistry Final Exam 7 Question 4 A) i) Why is tin used to protect the iron in 'tin' cans. Explain why. [1] ii) Explain one method of protecting metal against corrosion with one advantage and one disadvantage. [3] B) A student makes three mistakes when designing a voltaic cell. Identify the mistakes and briefly explain why they are a problem. silver (Ag) electrode wires battery wire copper (Cu) electrode Cu(N 3 ) 2 Ag(N 3 ) 2 i) ii) iii) [6]
8 Basic Chemistry Final Exam 8 Question 5 A) Explain what effect the following changes will make to the rate of a reaction and why: i) heating the reaction: ii) diluting the reaction: iii) using a catalyst: [4] B) i) Chemists rarely perform chemical reactions between two solids. Instead, they prefer to dissolve the solids in solvents and run the reactions in solution. Explain why, in terms of collision theory. ii) Gunpowder burns charcoal (pure carbon) as a fine powder (~0.1 mm diameter), whilst barbeques burn large pieces of charcoal (~ mm length). Explain this difference. C) According to thermodynamics calculations, wood should spontaneously react with oxygen at room temperature. Explain why wooden furniture does not spontaneously catch fire at room temperature.
9 Basic Chemistry Final Exam 9 Rough Working
Autumn Semester. Basic Chemistry for Engineering/ Fundamental Inorganic Chemistry Final Exam. 3 February Time: 60 minutes
Basic Chemistry Final Exam 1 Name: Student number: Instructions: Autumn Semester Basic Chemistry for Engineering/ Fundamental Inorganic Chemistry Final Exam 3 February 2014 Time: 60 minutes Answer any
More informationHonors Chemistry Unit 4 Exam Study Guide Solutions, Equilibrium & Reaction Rates
Honors Chemistry Unit 4 Exam Study Guide Solutions, Equilibrium & Reaction Rates Define the following vocabulary terms. Solute Solvent Solution Molarity Molality Colligative property Electrolyte Non-electrolyte
More informationAutumn Semester. Basic Chemistry for Engineering/ Fundamental Inorganic Chemistry Mid-term Exam. 07 December 2015.
Basic Chemistry Mid-term Eam 1 Name: Student number: Instructions: Autumn Semester Basic Chemistry for Engineering/ Fundamental Inorganic Chemistry Mid-term Eam 07 December 2015 Time: 60 minutes Answer
More informationc. K 2 CO 3 d. (NH 4 ) 2 SO 4 Answer c
Chem 130 Name Exam 2, Ch 4-6 July 7, 2016 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units and
More informationFinal Exam Review-Honors Name Period
Final Exam Review-Honors Name Period This is not a fully comprehensive review packet. This packet is especially lacking practice of explanation type questions!!! You should study all previous review sheets
More informationChem GENERAL CHEMISTRY II
GENERAL CHEMISTRY II CHEM 206 /2 51 Final Examination December 19, 2006 1900-2200 Dr. Cerrie ROGERS x x programmable calculators must be reset Chem 206 --- GENERAL CHEMISTRY II LAST NAME: STUDENT NUMBER:
More informationAP Chapter 6: Thermochemistry Name
AP Chapter 6: Thermochemistry Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 6: Thermochemistry 2 Warm-Ups (Show your work for credit)
More informationChemistry. Student Number. Mark / 64. Final Examination Preliminary Course General Instructions. Total Marks 64
Student Number Mark / 64 Chemistry Final Examination Preliminary Course 2003 General Instructions Reading time 5 minutes Working time 120 minutes Write using black or blue pen Draw diagrams using pencil
More information2 nd Semester Study Guide 2016
Chemistry 2 nd Semester Study Guide 2016 Name: Unit 6: Chemical Reactions and Balancing 1. Draw the remaining product 2. Write a balanced equation for the following reaction: The reaction between sodium
More informationFORMULA SHEET (tear off)
FORMULA SHEET (tear off) N A = 6.022 x 10 23 C = ( 5 / 9 ) ( F - 32) F = ( 9 / 5 )( C) + 32 1 amu = 1.661 x 10-27 kg C = K - 273.15 K = C + 273.15 1 atm = 760 torr = 760 mm Hg 1 atm = 1.013 bar pv = nrt
More information5 Energy from chemicals
5 Energy from chemicals Content 5.1 Enthalpy 5.2 Hydrogen fuel cell Learning Outcomes Candidates should be able to: (a) (b) (c) (d) (e) describe the meaning of enthalpy change in terms of exothermic (H
More informationChemistry 6A F2007. Dr. J.A. Mack. Freezing Point Depression: 11/16/07. t f = nk f M
Chemistry 6A F2007 Dr. J.A. Mack 11/16/07 11/14/07 Dr. Mack. CSUS 1 Freezing Point Depression: Similarly: The Freezing point of a solution is always lower than the freezing point of the pure solvent of
More informationChem 130 Name Exam 2 October 11, Points Part I: Complete all of problems 1-9
Chem 130 Name Exam October 11, 017 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units and significant
More informationChem GENERAL CHEMISTRY II MIDTERM EXAMINATION
Concordia University CHEM 206 Winter 2009, Dr. C. Rogers, Section 52 LAST NAME: FIRST NAME: STUDENT ID: Chem 206 - GENERAL CHEMISTRY II MIDTERM EXAMINATION INSTRUCTIONS: PLEASE READ THIS PAGE WHILE WAITING
More informationFORMULA SHEET (tear off)
FORMULA SHEET (tear off) N A = 6.022 x 10 23 C = ( 5 / 9 ) ( F - 32) F = ( 9 / 5 )( C) + 32 1 amu = 1.661 x 10-27 kg C = K - 273.15 K = C + 273.15 1 atm = 760 torr = 760 mm Hg 1 atm = 1.013 bar pv = nrt
More informationCHEM5. (JAN13CHEM501) WMP/Jan13/CHEM5. General Certificate of Education Advanced Level Examination January 2013
Centre Number Surname Candidate Number For Examiner s Use Other Names Candidate Signature Examiner s Initials General Certificate of Education Advanced Level Examination January 2013 Question 1 2 Mark
More informationMCGILL UNIVERSITY FACULTY OF SCIENCE MIDTERM EXAMINATION CHEM 120 MONDAY MARCH 16, :30PM 8:30PM VERSION NUMBER: 1
MCGILL UNIVERSITY FACULTY OF SCIENCE MIDTERM EXAMINATION CHEM 120 MONDAY MARCH 16, 2009 6:30PM 8:30PM VERSION NUMBER: 1 Instructions: BEFORE YOU BEGIN: Enter your student number and name on the computer
More informationKWANTLEN UNIVERSITY COLLEGE DEPARTMENT OF CHEMISTRY
KWANTLEN UNIVERSITY COLLEGE DEPARTMENT OF CHEMISTRY NAME: CHEM. 1210 FINAL EXAMINATION December 13, 2001 Time: 3 hours INSTRUCTIONS: 1. Read all questions thoroughly and answer each question completely.
More information2nd Semester Exam Review. C. K eq = [N 2][H 2 ]
Name: ate: 1. Which pair of formulas represents the empirical formula and the molecular formula of a compound?. H 2 O, 4 H 6 O 4. HO, 6 H 12 O 6 8. Given the reaction at equilibrium: N 2 (g) + 3H 2 (g)
More informationHEATING CURVE OF UNKNOWN SUBSTANCE
SPRING 2018 FINAL EXAM REVIEW STUDY GUIDE GENERAL CHEMISTRY 55 MULTIPLE CHOICE QUESTIONS STUDENTS CAN USE A CALCULATOR & TEACHER PROVIDED PERIODIC TABLE UNIT 3: THERMOCHEMISTRY Vocabulary & Concepts 1.
More informationGas 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
More informationReview Sheet 6 Math and Chemistry
Review Sheet 6 Math and Chemistry The following are some points of interest in Math and Chemistry. Use this sheet when answering these questions. Molecular Mass- to find the molecular mass, you must add
More informationChapter 19 Chemical Thermodynamics
Chapter 19. Chemical Thermodynamics Sample Exercise 19.2 (p. 819) Elemental mercury is a silver liquid at room temperature. Its normal freezing point is -38.9 o C, and its molar enthalpy of fusion is H
More informationEquilibrium. What is equilibrium? Hebden Unit 2 (page 37 69) Dynamic Equilibrium
Equilibrium What is equilibrium? Hebden Unit (page 37 69) Dynamic Equilibrium Hebden Unit (page 37 69) Experiments show that most reactions, when carried out in a closed system, do NOT undergo complete
More informationWhat type of solution that contains all of the
What type of solution that contains all of the solute it can hold at a given temperature? Saturated Solution What type of solution that contains less solute than it is able to hold at a given temperature?
More informationChapter 12 & 13 Test Review. Bond, Ionic Bond
Chapter 12 & 13 Test Review A solid solute dissolved in a solid solvent is an Alloy What is happening in a solution at equilibrium? The Ionic rate of Bond dissolving is equal to the rate of crystallization.
More informationChemical Thermodynamics
Quiz A 42.8 ml solution of ammonia (NH 3 ) is titrated with a solution of 0.9713 M hydrochloric acid. The initial reading on the buret containing the HCl was 47.13 ml and the final reading when the endpoint
More informationCHM 2046 Final Exam Review: Chapters 11 18
Chapter 11 1. Which of the following has the lowest boiling point? a. NH 3 b. CH 3 Cl c. NaCl d. CO 2 e. CH 3 CH 2 CH 2 CH 2 CH 3 2. Which of the following has the lowest vapor pressure? a. CH 3 F b. CH
More informationI. Multiple Choice Questions (Type-I) is K p
Unit 7 EQUILIBRIUM I. Multiple Choice Questions (Type-I) 1. We know that the relationship between K c and K p is K p K c (RT) n What would be the value of n for the reaction NH 4 Cl (s) NH 3 (g) + HCl
More informationName Class Date. As you read Lesson 17.1, use the cause and effect chart below. Complete the chart with the terms system and surroundings.
Name Class Date Thermochemistry 17.1 The Flow of Energy As you read Lesson 17.1, use the cause and effect chart below. Complete the chart with the terms system and surroundings. Process Cause Effect endothermic
More informationChemistry 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
More informationChem 128, Exam III April 23, 2004
I. (35 points) A. (10 points) Consider an aqueous solution of PbI 2 with solid lead(ii) iodide present. K sp =8.4x10 9. 1. Write a balanced net ionic equation for the equilibrium established between the
More informationKinetics & Equilibrium Review Packet. Standard Level. 1. Which quantities in the enthalpy level diagram are altered by the use of a catalyst?
Kinetics & Equilibrium Review Packet Standard Level 1. Which quantities in the enthalpy level diagram are altered by the use of a catalyst? Enthalpy I II III Time A. I and II only B. I and III only C.
More information1 Which of the following compounds has the lowest solubility in water? (4 pts)
version: 516 Exam 1 - Sparks This MC portion of the exam should have 19 questions. The point values are given with each question. Bubble in your answer choices on the bubblehseet provided. Your score is
More informationSolutions. Solutions. How Does a Solution Form? Solutions. Energy Changes in Solution. How Does a Solution Form
Ummm Solutions Solutions Solutions are homogeneous mixtures of two or more pure substances. In a solution, the solute is dispersed uniformly throughout the solvent. Solutions The intermolecular forces
More informationAP Chemistry Chapter 16 Assignment. Part I Multiple Choice
Page 1 of 7 AP Chemistry Chapter 16 Assignment Part I Multiple Choice 1984 47. CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O(l) H = 889.1 kj H f H 2 O(l) = 285.8 kj mol 1 H f CO 2 (g) = 393.3 kj mol 1 What is
More informationChem GENERAL CHEMISTRY II MIDTERM EXAMINATION
Concordia University CHEM 206 Winter 2009, Dr. C. Rogers, Section 01 LAST NAME: FIRST NAME: STUDENT ID: Chem 206 - GENERAL CHEMISTRY II MIDTERM EXAMINATION INSTRUCTIONS: PLEASE READ THIS PAGE WHILE WAITING
More informationICSE Board Class IX Chemistry Paper 5 Solution
ICSE Board Class IX Chemistry Paper 5 Solution SECTION I Answer 1 i. Dalton used the symbol for oxygen and the symbol for hydrogen. Symbol represents gram atom(s) of an element. i Symbolic expression for
More informationSilver nitrate solution is added to sodium dichromate solution
Chem. 110 50 Points Final Exam Part 1 Practice Write the chemical names or formulas for the following a H 2 SO 4 b NiNO 2 c Aluminum thiosulfate d Plumbic acetate e Ag 2 C 2 O 4 f P 2 O 5 g Cyanic acid
More information2 nd Semester Study Guide 2017
Chemistry 2 nd Semester Study Guide 2017 Name: KEY Unit 6: Chemical Reactions and Balancing 1. Draw the remaining product 2. Write a balanced equation for the following reaction: The reaction between sodium
More informationChemistry 121 Chapters 7& 8 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question.
Chemistry 121 Chapters 7& 8 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A sample of carbon dioxide occupies 22.4 L at STP. Which of the
More informationCHEM5. General Certificate of Education Advanced Level Examination June Unit 5 Energetics, Redox and Inorganic Chemistry
Centre Number Surname Candidate Number For Examiner s Use Other Names Candidate Signature Examiner s Initials General Certificate of Education Advanced Level Examination June 2010 Question 1 2 Mark Chemistry
More informationM09/4/CHEMI/SP2/ENG/TZ2/XX CHEMISTRY. Monday 18 May 2009 (afternoon) Candidate session number. 1 hour 15 minutes INSTRUCTIONS TO CANDIDATES
M09/4/CHEMI/SP2/ENG/TZ2/XX 22096117 CHEMISTRY standard level Paper 2 Monday 18 May 2009 (afternoon) 1 hour 15 minutes 0 0 Candidate session number INSTRUCTIONS TO CANDIDATES Write your session number in
More informationUNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certifi cate of Education Advanced Level
*3046788947* UNIVERSITY OF CAMBRIDGE INTERNATIONAL EXAMINATIONS General Certifi cate of Education Advanced Level CHEMISTRY 9701/51 Paper 5 Planning, Analysis and Evaluation October/November 2013 1 hour
More informationFRONT PAGE FORMULA SHEET - TEAR OFF
FRONT PAGE FORMULA SHEET - TEAR OFF N A = 6.022 x 10 23 C = ( 5 / 9 ) ( F - 32) F = ( 9 / 5 )( C) + 32 1 amu = 1.661 x 10-27 kg C = K - 273.15 K = C + 273.15 1 atm = 760 torr = 760 mm Hg 1 atm = 1.013
More informationSect 7.1 Chemical Systems in Balance HMWK: Read pages
SCH 4UI Unit 4 Chemical Systems and Equilibrium Chapter 7 Chemical Equilibrium Sect 7.1 Chemical Systems in Balance HMWK: Read pages 420-424 *Some reactions are reversible, ie not all reactions are as
More informationChemistry 1A, Spring 2007 Midterm Exam 3 April 9, 2007 (90 min, closed book)
Chemistry 1A, Spring 2007 Midterm Exam 3 April 9, 2007 (90 min, closed book) Name: KEY SID: TA Name: 1.) Write your name on every page of this exam. 2.) This exam has 34 multiple choice questions. Fill
More informationThe student s results are shown in the table below. Time / minutes Time / minutes
Q1.(a) Anhydrous calcium chloride is not used as a commercial de-icer because it reacts with water. The reaction with water is exothermic and causes handling problems. A student weighed out 1.00 g of anhydrous
More informationBased on the kinetic molecular theory of gases, which one of the following statements is INCORRECT?
1 Based on the kinetic molecular theory of gases, which one of the following statements is INCORRECT? A) The collisions between gas molecules are perfectly elastic. B) At absolute zero, the average kinetic
More informationCh 9 Practice Problems
Ch 9 Practice Problems 1. One mole of an ideal gas is expanded from a volume of 1.50 L to a volume of 10.18 L against a constant external pressure of 1.03 atm. Calculate the work. (1 L atm = 101.3 J) A)
More information2. Identify each of the following samples of matter as heterogeneous or homogeneous.
EOC REVIEW #1 1. List the following in order from smallest to largest. (A) 1 dm 3 (B) 1 ml (C) 1 cl (D) 1 L (E) 1 dl 2. Convert the following. Express your answer in standard scientific notation. (A) 36
More information(g) burns according to this reaction? D) CH 4 (g) + 2O 2 (g) CO 2 (g) + 2H 2 O(l)
Name: 7171-1 - Page 1 1) In a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is defined as the A) heat of reaction B) ionization
More informationCHEMISTRY. Section II (Total time 95 minutes) Part A Time 55 minutes YOU MAY USE YOUR CALCULATOR FOR PART A.
CHEMISTRY Section II (Total time 95 minutes) Part A Time 55 minutes YOU MAY USE YOUR CALCULATOR FOR PART A. CLEARLY SHOW THE METHOD USED AND THE STEPS INVOLVED IN ARRIVING AT YOUR ANSWERS. It is to your
More informationIn previous chapters we have studied: Why does a change occur in the first place? Methane burns but not the reverse CH 4 + 2O 2 CO 2 + 2H 2 O
Chapter 19. Spontaneous Change: Entropy and Free Energy In previous chapters we have studied: How fast does the change occur How is rate affected by concentration and temperature How much product will
More informationChemistry I 2nd Semester Exam Study Guide
Chemistry I 2nd Semester Exam Study Guide Study the following topics and be able to apply these concepts to answer related questions to best prepare for the Chemistry exam. You should be able to: 1. Identify
More informationHEATING CURVE OF UNKNOWN SUBSTANCE
TEMPERATURE ( C) SPRING 218 FINAL EXAM REVIEW STUDY GUIDE GENERAL CHEMISTRY 55 MULTIPLE CHOICE QUESTIONS STUDENTS CAN USE A CALCULATOR & TEACHER PROVIDED PERIODIC TABLE UNIT 3: THERMOCHEMISTRY VOCABULARY
More informationCHEM5. General Certificate of Education Advanced Level Examination June Unit 5 Energetics, Redox and Inorganic Chemistry
Centre Number Surname Candidate Number For Examiner s Use Other Names Candidate Signature Examiner s Initials General Certificate of Education Advanced Level Examination June 2011 Question 1 2 Mark Chemistry
More informationCHEM 10123/10125, Exam 3
CHEM 10123/10125, Exam 3 April 4, 2012 (50 minutes) Name (please print) Please box your answers, and remember that significant figures, phases (for chemical equations), and units do count! 1. (18 points)
More informationMULTIPLE CHOICE PORTION:
AP Chemistry Fall Semester Practice Exam 4 MULTIPLE CHOICE PORTION: Write the letter for the correct answer to the following questions on the provided answer sheet. Each multiple choice question is worth
More informationAnswer ALL questions
Answer ALL questions 01. Most experiments involving electrolysis use inert electrodes, which do not take part in the reactions. However, in some experiments the electrodes do take part in the reactions.
More informationUNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 2 March 14, pm (60 minutes) DISPLAY YOUR STUDENT ID CARD ON THE TOP OF YOUR DESK NOW
Version A UNIVERSITY OF VICTORIA CHEMISTRY 102 Midterm Test 2 March 14, 2014 5-6 pm (60 minutes) Version A DISPLAY YOUR STUDENT ID CARD ON THE TOP OF YOUR DESK NOW Answer all multiple choice questions
More informationN10/4/CHEMI/SP2/ENG/TZ0/XX CHEMISTRY STANDARD LEVEL PAPER 2. Thursday 11 November 2010 (afternoon) Candidate session number.
N10/4/CHEMI/SP2/ENG/TZ0/XX 88106105 CHEMISTRY STANDARD LEVEL PAPER 2 Thursday 11 November 2010 (afternoon) 1 hour 15 minutes 0 0 Candidate session number INSTRUCTIONS TO CANDIDATES Write your session number
More informationPart A Answer all questions in this part.
Part A Directions (1-24): For each statement or question, record on your separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question.
More informationApply the concept of percent yield to stoichiometric problems. Methanol can be produced through the reaction of CO and H 2 in the presence of a
Apply the concept of percent yield to stoichiometric problems. Methanol can be produced through the reaction of CO and H 2 in the presence of a catalyst. CO (g) + H 2 (g) CH 3 OH (l) If 75.0 g of CO reacts
More information4. Which of the following gas molecules will have the highest average velocity at 500K? a. H 2 b. He c. CH 4 d. C 2H 6
Multiple hoice (3 pts each) 1. In which of the following processes will work be positive? Assume the pressure remains constant for all examples. a. 2(l) 2(g) at constant temperature b. 2 8 18(l) + 25 2(g)
More informationChemistry 30: Thermochemistry. Practice Problems
Name: Period: Chemistry 30: Thermochemistry Practice Problems Date: Heat and Temperature 1. Pretend you are doing a scientific study on the planet Earth. a. Name three things in the system you are studying.
More information1. Read all questions thoroughly and answer each question completely. ALL WORK MUST BE SHOWN IN ORDER TO RECEIVE ANY CREDIT.
INSTRUCTIONS: 1. Read all questions thoroughly and answer each question completely. ALL WORK MUST BE SHOWN IN ORDER TO RECEIVE ANY CREDIT. 2. You will be allowed to use only the given sheet of thermodynamic
More informationTOPIC 4: THE MOLE CONCEPTS
TOPIC 4: THE MOLE CONCEPTS INTRODUCTION The mass is gram (g) of 1 mole of substances is called its.. 1 mole of substances has.. particles of a substances The mass of 1 mole of substances is always equal
More informationTest #3 Last Name First Name November 13, atm = 760 mm Hg
Form G Chemistry 1442-001 Name (please print) Test #3 Last Name First Name November 13, 2003 Instructions: 1. This exam consists of 25 questions. 2. No scratch paper is allowed. You may do the work in
More informationName AP CHEM / / Collected AP Exam Essay Answers for Chapter 16
Name AP CHEM / / Collected AP Exam Essay Answers for Chapter 16 1980 - #7 (a) State the physical significance of entropy. Entropy (S) is a measure of randomness or disorder in a system. (b) From each of
More informationMoles of NaOH Mass of NaOH...
Q1.A student calculated that a value for the enthalpy change of neutralisation is 51.2 kj mol 1. The design of a possible hand-warmer using hydrochloric acid and sodium hydroxide was discussed. It was
More informationReaction Rate and Equilibrium Chapter 19 Assignment & Problem Set
Reaction Rate and Equilibrium Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Reaction Rate and Equilibrium 2 Study Guide: Things You Must Know
More informationChapter 13. This ratio is the concentration of the solution.
Concentration Calculation Concentration In a solution, the solute is distributed evenly throughout the solvent. This means that any part of a solution has the same ratio of solute to solvent as any other
More informationSCH4U: EXAM REVIEW. 2. Which of the following has a standard enthalpy of formation of 0 kj mol -1 at 25ºC and 1.00 atm?
SCH4U_08-09 SCH4U: EXAM REVIEW 1. The heat of a reaction is equal to: a. enthalpy (products) + enthalpy (reactants) b. enthalpy (reactants) enthalpy (products) c. enthalpy (products) enthalpy (reactants)
More informationChem 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
More information300 May 8, Put all calculations on the examination pages. Do not make any extra marks on the computer answer sheet!!
Name Chemistry 153-080 (3150:153-080) FINAL EXAM 120 MINUTES Tuesday, 6:00PM Instructions: 300 May 8, 2003 1. Each student is responsible for following instructions. Read this page carefully. 2. Print
More informationCHEMISTRY HIGHER LEVEL
*P15* PRE-LEAVING CERTIFICATE EXAMINATION, 2008 CHEMISTRY HIGHER LEVEL TIME: 3 HOURS 400 MARKS Answer eight questions in all These must include at least two questions from Section A All questions carry
More informationCHERRY HILL TUITION AQA CHEMISTRY A2 PAPER Section A. Answer all questions in the spaces provided.
2 Section A Answer all questions in the spaces provided. 1 This question is about bond dissociation enthalpies and their use in the calculation of enthalpy changes. 1 (a) Define bond dissociation enthalpy
More informationChemistry Grade : 11 Term-3/Final Exam Revision Sheet
Chemistry Grade : 11 Term-3/Final Exam Revision Sheet Exam Date: Tuesday 12/6/2018 CCS:Chem.6a,6b,6c,6d,6e,6f,7a,7b,7d,7c,7e,7f,1g Chapter(12):Solutions Sections:1,2,3 Textbook pages 378 to 408 Chapter(16):Reaction
More informationSolutions and Their Properties
Chapter 11 Solutions and Their Properties Solutions: Definitions A solution is a homogeneous mixture. A solution is composed of a solute dissolved in a solvent. When two compounds make a solution, the
More informationChemistry 110 Practice Exam 3 (Ch 5,6,7[Energy]) closed-book cannot Cell phones are not allowed during the exam
Chemistry 110 Practice Exam 3 (Ch 5,6,7[Energy]) Note: 1. Sit according to the seat number assigned (ask the TA or the instructor). 2. Use a softhead pencil, fill in you name, z-number, department name
More informationGummy Bear Demonstration:
Name: Unit 8: Chemical Kinetics Date: Regents Chemistry Aim: _ Do Now: a) Using your glossary, define chemical kinetics: b) Sort the phrases on the SmartBoard into the two columns below. Endothermic Rxns
More information9.1 Introduction to Oxidation and Reduction
9.1 Introduction to Oxidation and Reduction 9.1.1 - Define oxidation and reduction in terms of electron loss and gain Oxidation The loss of electrons from a substance. This may happen through the gain
More informationHomework 11 - Second Law & Free Energy
HW11 - Second Law & Free Energy Started: Nov 1 at 9:0am Quiz Instructions Homework 11 - Second Law & Free Energy Question 1 In order for an endothermic reaction to be spontaneous, endothermic reactions
More informationSOLUTIONS. Homogeneous mixture uniformly mixed on the molecular level. Solvent & Solute. we will focus on aqueous solutions
SOLUTIONS Homogeneous mixture uniformly mixed on the molecular level Solvent & Solute we will focus on aqueous solutions SOLUTE-SOLVENT SOLVENT INTERACTIONS Why do solutions form? Processes occur spontaneously
More informationSpring Final Exam Review
Directions: Complete all of the following questions. Turn this in on the day of your final and you can earn up to 10 bonus points on your final. You must number and answer every questions on a separate
More informationName:. Correct Questions = Wrong Questions =.. Unattempt Questions = Marks =
Name:. Correct Questions = Wrong Questions =.. Unattempt Questions = Marks = 1. When this equation is balanced using the smallest possible integers, what is the sum of the coefficients? (NH 4 ) 3 O 4 (aq)
More informationChemistry 11: General Chemistry 1 Final Examination. Winter 2006
Chemistry 11: General Chemistry 1 Final Examination Winter 2006 Answers are given at the end of the exam. Name 1 Part 1 1. A 0.600 g pure sample of elemental iron (Fe) is dissolved in H 2 SO 4 (aq) to
More informationSolution. Types of Solutions. Concentration and Solution Stoichiometry
Concentration and Solution Stoichiometry Solution homogenous mixture of 2 or more pure substances only one perceptible phase species do not react chemically Types of Solutions solid liquid gas Solutions
More informationBonus Final Exam 3. 1 Calculate the heat of reaction,δh 0 rxn, for the following reaction as written at 298 K: g 2H 2 CH 4. g CF 4.
Bonus Final Exam 3 1 Calculate the heat of reaction,δh rxn, for the following reaction as written at 298 K: CH 4 2F 2 CF 4 2H 2 substance CH 4 CF 4 ΔH f kj/mol 75 68 (A) ΔH rxn 23 kj (B) ΔH rxn 914 kj
More informationName Page 1. N a m e F o rm u l a Soluble in Wa t e r? BaSO 4. Li 2 CO 3. Cu(OH) 2
Name Page 1 AQUEOUS SOLUTIONS 1. (10 points) Names, formulas, and solubility of compounds. N a m e F o rm u l a Soluble in Wa t e r? Ammonium chloride NH 4 Cl Yes BaS Barium phosphate Manganese(IV) oxide
More informationChemistry. ANSWERS and MARKING SCHEME. Final Examination Preliminary Course General Instructions. Total Marks 64
ANSWERS and MARKING SCHEME Chemistry Final Examination Preliminary Course 2003 General Instructions Reading time 5 minutes Working time 120 minutes Write using black or blue pen Draw diagrams using pencil
More informationE-JUST Entrance Exams 2017
E-JUST Entrance Exams 2017 Undergraduate Admission Faculty of Engineering Chemistry Time allowed: 1 hr. Choose the correct answer: 1. How many valence electrons does an oxygen atom have? A. 2 B. 4 C. 8
More informationAccelerated Chemistry Semester 2 Review Sheet
Accelerated Chemistry Semester 2 Review Sheet The semester test will be given in two parts. The first part is a performance assessment and will be given the day before the semester test. This will include
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A solution containing a large concentration of dissolved ions can be classified as a(n).
More informationStoichiometry. Percent composition Part / whole x 100 = %
Stoichiometry Conversion factors 1 mole = 6.02 x 10 23 atoms (element) 1 mole = 6.02 x 10 23 molecules (covalent compounds) 1 mole = 6.02 x 10 23 formula units (ionic compounds) 1 mole (any gas @ STP)
More informationIB Chemistry Solutions Gasses and Energy
Solutions A solution is a homogeneous mixture it looks like one substance. An aqueous solution will be a clear mixture with only one visible phase. Be careful with the definitions of clear and colourless.
More informationENTHALPY, ENTROPY AND FREE ENERGY CHANGES
ENTHALPY, ENTROPY AND FREE ENERGY CHANGES Refer to the following figures for Exercises 1-6. The lines on the vertical axis represent the allowed energies. Assume constant spacing between levels to determine
More informationCHEM J-14 June 2014
CHEM1101 2014-J-14 June 2014 An electrochemical cell consists of an Fe 2+ /Fe half cell with unknown [Fe 2+ ] and a Sn 2+ /Sn half-cell with [Sn 2+ ] = 1.10 M. The electromotive force (electrical potential)
More informationCHEMpossible. 101 Exam 2 Review
CHEMpossible 1. Circle each statement that applies to thermal energy and heat: a. Thermal energy is the average kinetic energy of its molecules due to their motion b. High thermal energy is reflected in
More information