7. Consider the reaction coordinate diagram shown. Which statement is true? C D
|
|
- Rosemary Lawrence
- 7 years ago
- Views:
Transcription
1 SPRING 2001 FINAL 1. A solution prepared by dissolving 6.54 g of a non-volatile solute in 60.0 g of water boils at C. What is the approximate molar mass of the solute? K b of H 2 O = C/m. A g/mol B g/mol C. 151 g/mol D. 295 g/mol E. 543 g/mol 2. A molar solution of sugar is separated from pure water by a membrane at 20 C. What is the osmotic pressure? A. 12 torr B. 91 torr C. 901 torr D torr E. 6.2 torr 3. Which is true? A. dipole-dipole forces are responsible for the solubility of ions in water B. the solubility of gases in liquids increases with increasing temperature C. dispersion forces are the result of distortion of the distribution of electrons in adjacent molecules D. hydrogen bonds are those present in hydrocarbons E. none of these 4. The reaction, 4 A + C => D has the mechanism below. What is the rate law? 2 A => B slow 2B + C => D fast A. rate = k[b] 2 [C] B. rate = k[a] 2 C. rate = k[a][b][c] D. rate = k[a] 4 [C] E. rate = k[a] 2 [B] 2 [C] 5. For the reaction, H 2 (g) + I 2 (g) => 2 HI(g), the rate constant for the formation of HI(g) is 2.7 x 10-4 L/mol.sec at 600 K and 3.5 x 10-3 at 650 K. Calculate the activation energy for the reaction. A. 166 kj/mol B. 83 kj/mol C. 332 kj/mol D. 475 kj/mol E. 166 kj/mol
2 6. The initial rates of reaction for 2 NO(g) + Cl 2 (g) => 2 NOCl(g) are Exp. Initial [NO] Initial [Cl 2 ] Initial rate [M sec -1 ] M M 2.27 x M M 4.55 x M M 9.08 x M M 3.63 x 10-4 What is the rate law for this reaction? A. rate = k[no][cl 2 ] B. rate = k[no][cl 2 ] 2 C. rate = k[no] 2 D. rate = k[no] 2 [Cl 2 ] E. rate = k[no] 2 [Cl 2 ] 2 7. Consider the reaction coordinate diagram shown. Which statement is true? B C D A A. there are three intermediates B. there are two transition states C. the first step is rate-limiting D. the reaction is endothermic E. all are false
3 8. Cobalt-60 has a half-life of 5.27 years. How long will it require for 10.5 mg of a 22.8 mg sample of 60 Co to decay? A y B y C y D y E y 9. Alpha emission by polonium-204 [ 204 Po] results in the product? A. 203 Tl B. 200 Hg C. 204 Bi D. 204 Hg E. 200 Pb 10. The actual mass of a 37 Cl atom is amu. Calculate the mass deficiency in amu/atom for a 37 Cl atom. Mass of an electron = amu, a proton = amu, a neutron = amu. A B C D E A positron has a mass number of, a charge of and a mass equal to that of a (an) : A. 0, 1+, electron B. 0, 1+, proton C. 1, 2+, proton D. 4, 2+, helium nucleus E. 1, 2+, electron 12. A buffer solution is prepared that is 0.24 M NH 3 and 0.20 M NH 4 Cl. What is the ph of this buffer? K b for NH 3 is 1.8 x 10-5 A B. 9.0 C D. 1.8 x 10-5 E. 9.33
4 13. Of the salts shown below, which ones form a basic aqueous solution? I. NaCH 3 CO 2 II. NaCN III. NaF IV. NH 4 NO 3 A. I and II only B. I, II and III only C. II and III only D. IV only E. I, II, III and IV 14. Which is TRUE? A. In the Lewis theory, BF 3 is an acid B. In a solution of H 3 PO 4, the ph is greatly influenced by K a2 and K a3? C. In the Bronsted-Lowry theory, an acid is a donor of electrons D. In water, the salt of a weak acid and a weak base has a ph Of 7.0 E. all of these are false 15. The conjugate base of HPO 4 2- is A. PO 4 3- B. H 2 PO 4 - C. HPO 4 2- D. H 3 PO 4 E. PO For the gas phase reaction, SO 2 + 1/2 O 2 <=> SO 3, ΔH = -160 kj for the forward reaction. In order to increase the yield of SO 3, the reaction should be run A. at low P, low T B. at low P, high T C. at high P, low T D. at high P, high T E. at high P, but is independent of T 17. If ml of a M aqueous NH 3 solution is mixed with ml of M aqueous HCl at 25 C, the resulting solution will have a ph = A. > 7.00 B. < 7.00 C D. cannot be predicted from the information E. none of these 18. Given that K p = 1.39 at 400 C for the reaction, P 4 (g) <=> 2 P 2 (g), which answer best describes the situation when 1.40 mol of P 4 (g) and 1.25 mol of P 2 (g) are mixed in a 25.0 L closed container at 400 C?
5 A. Q p = 1.39, the reaction is at equilibrium B. Q p = 2.47, the reaction proceeds to the left C. Q p = , the reaction proceeds to the left D. Q p = , the reaction proceeds to the right E. Q p = 2.47, the reaction proceeds to the right 19. Given that K p = 6.0 x 10-4 for the reaction, 2 CO(g) <=> C(s) + CO 2 (g), what is the partial pressure of CO 2 (g) at equilibrium if initially 2.00 atm of CO is in contact with solid carbon? A atm B atm C atm D atm E atm 20. A M solution of an acid has a ph of Calculate the K a of the acid A. 2.4 x 10-2 B. 2.3 x 10-5 C. 2.6 x 10-5 D. 5.7 x 10-4 E. 2.4 x Which of the following K a values belongs to the strongest acid? A. 6.6 x 10-4 B. 4.6 x 10-4 C. 9.1 x 10-8 D. 3.0 x 10-8 E. this cannot be determined from the information given 22. When 0.60 mol of NH 3 is introduced into a 1 L container at 850 K, the equilibrium concentration of NH 3 is measured as 0.12 M. What is K c for the reaction, 2 NH 3 (g) <=> N 2 (g) + 3 H 2 (g)? A B C D E What is the ph of a M solution of C 6 H 5 NH 2 given that its K b is 1.50 x 10-6? A B C. 8.2
6 D E In which solution will a precipitate form? I mg of Na 2 CrO 4 (molar mass = 162 g/mol) is added to 225 ml of M AgNO 3. K sp of Ag 2 CrO 4 = 1.1 x II L M MgCl 2 and L of M NaF. K sp of MgF 2 is 3.7 x 10-8 A. I. yes II. no B. I. no II. no C. I. yes II. yes D. I. no II. yes E. insufficient information to say 25. The standard free energy change for a reaction is 36.2 kj at 298 K. Calculate the equilibrium constant. A x 10 6 B C x 10 6 D E. 2.2 x At what temperature would a reaction become spontaneous if ΔH = +119 kj and ΔS = +263 J/K? A. 452 K B. 382 K C K D. 363 K E K 27. If an electrochemical cell, Rb Rb + Na + Na has a potential of V, what is the standard reduction potential of the Rb half-cell is the Na + / Na half-reaction has a reduction potential of 2.71 V? A V B V C V D V E V 28. What is the equilibrium constant for the reaction, 2 Ag + (aq) + 2 I - (aq) <=> I 2 (s) + 2 Ag(s) for which E = V? A x 10 7
7 B x 10 3 C D x 10 8 E x The second law of thermodynamics states that A. the enthalpy of the universe is increasing B. ΔS of the universe is zero C. the total entropy of the universe is increasing D. if ΔG is positive, the reaction is spontaneous E. heat is energy 30. The reaction, A + B => C + D has an enthalpy of reaction of 104 kj and a change in entropy of 60.8 J/K at 30 C. What is ΔG and the spontaneity of the reaction? A kj, non-spontaneous B kj, spontaneous C kj, non-spontaneous D kj, non-spontaneous E kj, spontaneous 31. When the following redox equation is balanced in acidic solution using the smallest possible whole number coefficients, what is the coefficient of zinc? Zn(s) + ReO 4 - (aq) => Zn 2+ (aq) + Re(s) A. 2 B. 7 C. 8 D. 14 E Calculate ΔG for the reaction of ammonia with fluorine: 2 NH 3 (g) + 5 F 2 (g) => N 2 F 4 (g) + 6 HF(g) given that the ΔG f for NH 3 = kj/mol, for N 2 F 4 = 79.9 kj/mol and for HF = kj/mol A kj B kj C kj D kj E kj 33. Calculate the solubility of silver oxalate, Ag 2 C 2 O 4 in pure water given that the K sp = 1.0 x A. 1.4 x 10-4
8 B. 2.2 x 10-4 C. 5.4 x 10-5 D. 3.2 x 10-6 E. 1.0 x A voltaic cell consists of a Cu 2+ /Cu electrode (E red = 0.34 V) and an Au 3+ /Au electrode (E red = 1.50 V). Calculate [Au 3+ ] if [Cu 2+ ] = 1.20 M and E cell = 1.13 V. A M B M C M D. 0.2 M E. 5.0 M 35. Predict the product at the anode when electric current is passed through an aqueous solution of KI A. K(s) B. K + (aq) C. H 2 (g) D. O 2 (g) E. I 2 (s) 36. How long would it take to plate 1.5 g of gold by electrolyzing a solution of Au 3+ with a current of 2.5 amps? A. 290 s B. 58,000 s C. 880 s D. 2.3 x 10-8 s E. 500 s 37. Which one of the following statements about electrochemical cells is correct A. in a salt bridge, current is carried by cations moving towards the anode and anions moving towards the cathode B. in the external wire of a voltaic cell, electrons move from cathode to anode C. in a voltaic cell, the anode is labeled as negative D. in an electrolytic cell, oxidation occurs at the cathode E. all of these are correct 38. What is a result of the lanthanide contraction? A. A Ti atom is about the same size as a Zr atom B. A Zr atom is about the same size as a Hf atom C. A Ti atom is about the same size as a Hf atom
9 D. the periodic table gets shortened when the lanthanides are left out E. weight loss 39. Which of the following transition metal ions typically has colorless compounds? A. Fe 2+ B. Fe 3+ C. Ti 3+ D. Ti 4+ E. V Which of the following statements is TRUE? A. reactivity in transition metal groups increases as you go down the group B. most lanthanides exist as 4+ ions C. an metal in a high oxidation states has a lower electronegativity than the metal itself D. Fe is often encountered in the 8+ oxidation state E. copper can be found in a +1 oxidation state as well as +2
CHM1 Review Exam 12. Topics REDOX
CHM1 Review Exam 12 Topics REDOX REDOX Reactions Oxidation Reduction Oxidizing agent Reducing agent Galvanic (Voltaic) Cells Anode Cathode Salt bridge Electrolyte Half-reactions Voltage o Positive voltages
More informationChemistry 122 Mines, Spring 2014
Chemistry 122 Mines, Spring 2014 Answer Key, Problem Set 9 1. 18.44(c) (Also indicate the sign on each electrode, and show the flow of ions in the salt bridge.); 2. 18.46 (do this for all cells in 18.44
More information2. Write the chemical formula(s) of the product(s) and balance the following spontaneous reactions.
1. Using the Activity Series on the Useful Information pages of the exam write the chemical formula(s) of the product(s) and balance the following reactions. Identify all products phases as either (g)as,
More information1332 CHAPTER 18 Sample Questions
1332 CHAPTER 18 Sample Questions Couple E 0 Couple E 0 Br 2 (l) + 2e 2Br (aq) +1.06 V AuCl 4 + 3e Au + 4Cl +1.00 V Ag + + e Ag +0.80 V Hg 2+ 2 + 2e 2 Hg +0.79 V Fe 3+ (aq) + e Fe 2+ (aq) +0.77 V Cu 2+
More informationRedox and Electrochemistry
Name: Thursday, May 08, 2008 Redox and Electrochemistry 1. A diagram of a chemical cell and an equation are shown below. When the switch is closed, electrons will flow from 1. the Pb(s) to the Cu(s) 2+
More informationELECTROCHEMICAL CELLS
1 ELECTROCHEMICAL CELLS Allessandra Volta (1745-1827) invented the electric cell in 1800 A single cell is also called a voltaic cell, galvanic cell or electrochemical cell. Volta joined several cells together
More informationName Electrochemical Cells Practice Exam Date:
Name Electrochemical Cells Practice Exam Date: 1. Which energy change occurs in an operating voltaic cell? 1) chemical to electrical 2) electrical to chemical 3) chemical to nuclear 4) nuclear to chemical
More informationChem 1721 Brief Notes: Chapter 19
Chem 1721 Brief Notes: Chapter 19 Chapter 19: Electrochemistry Consider the same redox reaction set up 2 different ways: Cu metal in a solution of AgNO 3 Cu Cu salt bridge electrically conducting wire
More informationCh 20 Electrochemistry: the study of the relationships between electricity and chemical reactions.
Ch 20 Electrochemistry: the study of the relationships between electricity and chemical reactions. In electrochemical reactions, electrons are transferred from one species to another. Learning goals and
More informationChapter 13: Electrochemistry. Electrochemistry. The study of the interchange of chemical and electrical energy.
Chapter 13: Electrochemistry Redox Reactions Galvanic Cells Cell Potentials Cell Potentials and Equilbrium Batteries Electrolysis Electrolysis and Stoichiometry Corrosion Prevention Electrochemistry The
More information4. Using the data from Handout 5, what is the standard enthalpy of formation of BaO (s)? What does this mean?
HOMEWORK 3A 1. In each of the following pairs, tell which has the higher entropy. (a) One mole of liquid water or one mole of water vapor (b) One mole of dry ice or one mole of carbon dioxide at 1 atm
More informationElectrochemistry Worksheet
Electrochemistry Worksheet 1. Assign oxidation numbers to each atom in the following: a. P 4 O 6 b. BiO 3 c. N 2 H 4 d. Mg(BrO 4 ) 2 e. MnSO 4 f. Mn(SO 4 ) 2 2. For each of the reactions below identify
More informationElectrochemistry Voltaic Cells
Electrochemistry Voltaic Cells Many chemical reactions can be classified as oxidation-reduction or redox reactions. In these reactions one species loses electrons or is oxidized while another species gains
More informationElectrochemistry - ANSWERS
Electrochemistry - ANSWERS 1. Using a table of standard electrode potentials, predict if the following reactions will occur spontaneously as written. a) Al 3+ + Ni Ni 2+ + Al Al 3+ + 3e - Al E = -1.68
More informationSummer 2003 CHEMISTRY 115 EXAM 3(A)
Summer 2003 CHEMISTRY 115 EXAM 3(A) 1. In which of the following solutions would you expect AgCl to have the lowest solubility? A. 0.02 M BaCl 2 B. pure water C. 0.02 M NaCl D. 0.02 M KCl 2. Calculate
More informationName AP CHEM / / Collected Essays Chapter 17 Answers
Name AP CHEM / / Collected Essays Chapter 17 Answers 1980 - #2 M(s) + Cu 2+ (aq) M 2+ (aq) + Cu(s) For the reaction above, E = 0.740 volt at 25 C. (a) Determine the standard electrode potential for the
More informationGalvanic Cells. SCH4U7 Ms. Lorenowicz. Tuesday, December 6, 2011
Galvanic Cells SCH4U7 Ms. Lorenowicz 1 Electrochemistry Concepts 1.Redox reactions involve the transfer of electrons from one reactant to another 2.Electric current is a flow of electrons in a circuit
More informationGalvanic cell and Nernst equation
Galvanic cell and Nernst equation Galvanic cell Some times called Voltaic cell Spontaneous reaction redox reaction is used to provide a voltage and an electron flow through some electrical circuit When
More informationChem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses
Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses B. Calculations of moles C. Calculations of number of atoms from moles/molar masses 1. Avagadro
More informationK + Cl - Metal M. Zinc 1.0 M M(NO
Redox and Electrochemistry This section should be fresh in your minds because we just did this section in the text. Closely related to electrochemistry is redox chemistry. Count on at least one question
More information5.111 Principles of Chemical Science
MIT OpenCourseWare http://ocw.mit.edu 5.111 Principles of Chemical Science Fall 2008 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms. Page 1 of 10 pages
More informationCHAPTER 21 ELECTROCHEMISTRY
Chapter 21: Electrochemistry Page 1 CHAPTER 21 ELECTROCHEMISTRY 21-1. Consider an electrochemical cell formed from a Cu(s) electrode submerged in an aqueous Cu(NO 3 ) 2 solution and a Cd(s) electrode submerged
More informationB) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal
1. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 2. Which list of elements consists of a metal, a metalloid, and
More informationstoichiometry = the numerical relationships between chemical amounts in a reaction.
1 REACTIONS AND YIELD ANSWERS stoichiometry = the numerical relationships between chemical amounts in a reaction. 2C 8 H 18 (l) + 25O 2 16CO 2 (g) + 18H 2 O(g) From the equation, 16 moles of CO 2 (a greenhouse
More informationChemistry 51 Chapter 8 TYPES OF SOLUTIONS. A solution is a homogeneous mixture of two substances: a solute and a solvent.
TYPES OF SOLUTIONS A solution is a homogeneous mixture of two substances: a solute and a solvent. Solute: substance being dissolved; present in lesser amount. Solvent: substance doing the dissolving; present
More informationDiscovering Electrochemical Cells
Discovering Electrochemical Cells Part I Electrolytic Cells Many important industrial processes PGCC CHM 102 Cell Construction e e power conductive medium What chemical species would be present in a vessel
More informationStandard Free Energies of Formation at 298 K. Average Bond Dissociation Energies at 298 K
1 Thermodynamics There always seems to be at least one free response question that involves thermodynamics. These types of question also show up in the multiple choice questions. G, S, and H. Know what
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Chemistry 1C-Dr. Larson Chapter 20 Review Questions MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) is reduced in the following reaction: Cr2O7
More informationName period Unit 9: acid/base equilibrium
Name period Unit 9: acid/base equilibrium 1. What is the difference between the Arrhenius and the BronstedLowry definition of an acid? Arrhenious acids give H + in water BronstedLowry acids are proton
More informationFigure 1. A voltaic cell Cu,Cu 2+ Ag +, Ag. gas is, by convention, assigned a reduction potential of 0.00 V.
Voltaic Cells Introduction In this lab you will first prepare a set of simple standard half-cells and then measure the voltage between the half-cells with a voltmeter. From this data you will be able to
More informationChemistry B11 Chapter 4 Chemical reactions
Chemistry B11 Chapter 4 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl
More informationCHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH
1. Is H 3 O + polar or non-polar? (1 point) a) Polar b) Non-polar CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH 2. The bond strength is considerably greater in HF than in the other three hydrogen halides
More informationChapter 18 Homework Answers
Chapter 18 Homework Answers 18.22. 18.24. 18.26. a. Since G RT lnk, as long as the temperature remains constant, the value of G also remains constant. b. In this case, G G + RT lnq. Since the reaction
More informationExperiment 9 Electrochemistry I Galvanic Cell
9-1 Experiment 9 Electrochemistry I Galvanic Cell Introduction: Chemical reactions involving the transfer of electrons from one reactant to another are called oxidation-reduction reactions or redox reactions.
More information10. Calculate the mass percent nitrogen in (NH 4 ) 2 CO 3 (molar mass = 96.09 g/mol). a. 29.1 % c. 17.9 % e. 14.6 % b. 35.9 % d. 0.292 % f. 96.
Chem 171-2-3: Final Exam Review Multiple Choice Problems 1. What is the molar mass of barium perchlorate, Ba(ClO 4 ) 2? a. 189.90 g/mol c. 272.24 g/mol e. 336.20 g/mol b. 240.24 g/mol d. 304.24 g/mol f.
More informationPotassium ion charge would be +1, so oxidation number is +1. Chloride ion charge would be 1, so each chlorine has an ox # of -1
Chapter 18-1 1. Assign oxidation numbers to each atom in: Ni Nickel ion charge would be +2, so oxidation number is +2 Chloride ion charge would be 1, so each chlorine has an ox # of -1 Mg 2 Ti 4 Magnesium
More informationReview: Balancing Redox Reactions. Review: Balancing Redox Reactions
Review: Balancing Redox Reactions Determine which species is oxidized and which species is reduced Oxidation corresponds to an increase in the oxidation number of an element Reduction corresponds to a
More informationATOMS. Multiple Choice Questions
Chapter 3 ATOMS AND MOLECULES Multiple Choice Questions 1. Which of the following correctly represents 360 g of water? (i) 2 moles of H 2 0 (ii) 20 moles of water (iii) 6.022 10 23 molecules of water (iv)
More informationChapter 11. Electrochemistry Oxidation and Reduction Reactions. Oxidation-Reduction Reactions. Oxidation-Reduction Reactions
Oxidation-Reduction Reactions Chapter 11 Electrochemistry Oxidation and Reduction Reactions An oxidation and reduction reaction occurs in both aqueous solutions and in reactions where substances are burned
More informationChemistry 151 Final Exam
Chemistry 151 Final Exam Name: SSN: Exam Rules & Guidelines Show your work. No credit will be given for an answer unless your work is shown. Indicate your answer with a box or a circle. All paperwork must
More informationPreliminary Concepts. Preliminary Concepts. Class 8.3 Oxidation/Reduction Reactions and Electrochemistry I. Friday, October 15 Chem 462 T.
Class 8.3 Oxidation/Reduction Reactions and Electrochemistry I Friday, October 15 Chem 462 T. Hughbanks Preliminary Concepts Electrochemistry: the electrical generation of, or electrical exploitation of
More informationCh 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent
1 Ch 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent % (v/v) = volume of solute x 100 volume of solution filled
More informationChemistry 106 Fall 2007 Exam 3 1. Which one of the following salts will form a neutral solution on dissolving in water?
1. Which one of the following salts will form a neutral solution on dissolving in water? A. NaCN B. NH 4 NO 3 C. NaCl D. KNO 2 E. FeCl 3 2. Which one of the following is a buffer solution? A. 0.10 M KCN
More informationChapter 17. The best buffer choice for ph 7 is NaH 2 PO 4 /Na 2 HPO 4. 19)
Chapter 17 2) a) HCl and CH 3 COOH are both acids. A buffer must have an acid/base conjugate pair. b) NaH 2 PO 4 and Na 2 HPO 4 are an acid/base conjugate pair. They will make an excellent buffer. c) H
More informationChapter 20. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Chapter 20 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The gain of electrons by an element is called. A) oxidation B) reduction C) sublimation
More informationAPPENDIX B: EXERCISES
BUILDING CHEMISTRY LABORATORY SESSIONS APPENDIX B: EXERCISES Molecular mass, the mole, and mass percent Relative atomic and molecular mass Relative atomic mass (A r ) is a constant that expresses the ratio
More informationCELL POTENTIAL, E. Terms Used for Galvanic Cells. Uses of E o Values CELL POTENTIAL, E. Galvanic Cell. Organize halfreactions
Electrons move from anode to cathode in the wire. Anions & cations move thru the salt bridge. Terms Used for Galvanic Cells Galvanic Cell We can calculate the potential of a Galvanic cell using one of
More informationInstructions Answer all questions in the spaces provided. Do all rough work in this book. Cross through any work you do not want to be marked.
GCSE CHEMISTRY Higher Tier Chemistry 1H H Specimen 2018 Time allowed: 1 hour 45 minutes Materials For this paper you must have: a ruler a calculator the periodic table (enclosed). Instructions Answer all
More information4.1 Aqueous Solutions. Chapter 4. Reactions in Aqueous Solution. Electrolytes. Strong Electrolytes. Weak Electrolytes
Chapter 4 Reactions in Aqueous Solution 4.1 Aqueous Solutions Solution homogeneous mixture of 2 or more substances Solute the substance present in a smaller amount (usually solid in Chap. 4) Solvent the
More informationAP Chemistry 2008 Free-Response Questions
AP Chemistry 008 Free-Response Questions The College Board: Connecting Students to College Success The College Board is a not-for-profit membership association whose mission is to connect students to college
More informationChemistry: Chemical Equations
Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,
More informationAqueous Ions and Reactions
Aqueous Ions and Reactions (ions, acids, and bases) Demo NaCl(aq) + AgNO 3 (aq) AgCl (s) Two clear and colorless solutions turn to a cloudy white when mixed Demo Special Light bulb in water can test for
More informationo Electrons are written in half reactions but not in net ionic equations. Why? Well, let s see.
REDOX REACTION EQUATIONS AND APPLICATIONS Overview of Redox Reactions: o Change in Oxidation State: Loses Electrons = Oxidized (Oxidation number increases) Gains Electrons = Reduced (Oxidation Number Reduced)
More informationINTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION. 37 74 20 40 60 80 m/e
CHM111(M)/Page 1 of 5 INTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION SECTION A Answer ALL EIGHT questions. (52 marks) 1. The following is the mass spectrum
More informationQuestion Bank Electrolysis
Question Bank Electrolysis 1. (a) What do you understand by the terms (i) electrolytes (ii) non-electrolytes? (b) Arrange electrolytes and non-electrolytes from the following substances (i) sugar solution
More informationCST Practice Test. Multiple Choice Questions
CST Practice Test Young NAME CST Practice Test Multiple Choice Questions 1) At 1 atm and 298 K, which of the K a values listed below represents the strongest acid? 5) Which electron-dot symbol represents
More informationCHEMICAL REACTIONS. Chemistry 51 Chapter 6
CHEMICAL REACTIONS A chemical reaction is a rearrangement of atoms in which some of the original bonds are broken and new bonds are formed to give different chemical structures. In a chemical reaction,
More informationAP Chemistry 2009 Scoring Guidelines
AP Chemistry 2009 Scoring Guidelines The College Board The College Board is a not-for-profit membership association whose mission is to connect students to college success and opportunity. Founded in 1900,
More informationAP Chemistry CHAPTER 20- Electrochemistry 20.1 Oxidation States
AP Chemistry CHAPTER 20- Electrochemistry 20.1 Oxidation States Chemical reactions in which the oxidation state of a substance changes are called oxidation-reduction reactions (redox reactions). Oxidation
More informationFinal Exam CHM 3410, Dr. Mebel, Fall 2005
Final Exam CHM 3410, Dr. Mebel, Fall 2005 1. At -31.2 C, pure propane and n-butane have vapor pressures of 1200 and 200 Torr, respectively. (a) Calculate the mole fraction of propane in the liquid mixture
More informationBuilding Electrochemical Cells
Cautions Heavy metals, such as lead, and solutions of heavy metals may be toxic and an irritant. Purpose To determine the cell potential (E cell ) for various voltaic cells and compare the data with the
More informationThermodynamics Worksheet I also highly recommend Worksheets 13 and 14 in the Lab Manual
Thermodynamics Worksheet I also highly recommend Worksheets 13 and 14 in the Lab Manual 1. Predict the sign of entropy change in the following processes a) The process of carbonating water to make a soda
More informationThe Mole. 6.022 x 10 23
The Mole 6.022 x 10 23 Background: atomic masses Look at the atomic masses on the periodic table. What do these represent? E.g. the atomic mass of Carbon is 12.01 (atomic # is 6) We know there are 6 protons
More informationI N V E S T I C E D O R O Z V O J E V Z D Ě L Á V Á N Í CHEMICAL REACTIONS
Chemical reaction = process during which original substances change to new substances, reactants turn to... The bonds of reactants... and new bonds are... The classification of reactions: 1. Classification
More information6 Reactions in Aqueous Solutions
6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface
More informationAqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.
Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration
More informationChapter 3 Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative
More informationAP Chemistry 2009 Free-Response Questions Form B
AP Chemistry 009 Free-Response Questions Form B The College Board The College Board is a not-for-profit membership association whose mission is to connect students to college success and opportunity. Founded
More informationBonding Practice Problems
NAME 1. When compared to H 2 S, H 2 O has a higher 8. Given the Lewis electron-dot diagram: boiling point because H 2 O contains stronger metallic bonds covalent bonds ionic bonds hydrogen bonds 2. Which
More information1 What is the angular momentum quantum number (l) value for the 3p sublevel? A 1
1 What is the angular momentum quantum number (l) value for the 3p sublevel? 1 2 3 4 ORRET: For the 3p sublevel, the principal quantum number (n) is 3 and the angular momentum quantum number (l) is 1.
More informationCorrelation of Nelson Chemistry Alberta 20 30 to the Alberta Chemistry 20 30 Curriculum
Correlation of Nelson Chemistry Alberta 20 30 to the Alberta Chemistry 20 30 Curriculum Unit 5 Organic Chemistry General Outcomes Students will: 1. explore organic compounds as a common form of matter
More informationChapter 8: Chemical Equations and Reactions
Chapter 8: Chemical Equations and Reactions I. Describing Chemical Reactions A. A chemical reaction is the process by which one or more substances are changed into one or more different substances. A chemical
More informationGeneral Chemistry II Chapter 20
1 General Chemistry II Chapter 0 Ionic Equilibria: Principle There are many compounds that appear to be insoluble in aqueous solution (nonelectrolytes). That is, when we add a certain compound to water
More informationElectrochemical Half Cells and Reactions
Suggested reading: Chang text pages 81 89 Cautions Heavy metals, such as lead, and solutions of heavy metals may be toxic and an irritant. Purpose To determine the cell potential (E cell ) for various
More informationCHAPTERS 15 FAKE TEST QUESTIONS. 1. According to the Brønsted Lowry definition, which species can function both as an acid and as a base?
You might need to know the following K values: CHAPTERS 15 FAKE TEST QUESTIONS CH 3 COOH K a = 1.8 x 10 5 Benzoic Acid K a = 6.5 x 10 5 HNO 2 K a = 4.5 x 10 4 NH 3 K b = 1.8 x 10 5 HF K a = 7.2 x 10 4
More informationSCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001
SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample
More informationChemical Equations and Chemical Reactions. Chapter 8.1
Chemical Equations and Chemical Reactions Chapter 8.1 Objectives List observations that suggest that a chemical reaction has taken place List the requirements for a correctly written chemical equation.
More informationPART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points)
CHEMISTRY 123-07 Midterm #1 Answer key October 14, 2010 Statistics: Average: 74 p (74%); Highest: 97 p (95%); Lowest: 33 p (33%) Number of students performing at or above average: 67 (57%) Number of students
More informationUnit 19 Practice. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.
Name: Class: Date: Unit 19 Practice Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The first law of thermodynamics can be given as. A) E = q + w B) =
More informationChemistry 2014 Scoring Guidelines
AP Chemistry 2014 Scoring Guidelines 2014 The College Board. College Board, Advanced Placement Program, AP, AP Central, and the acorn logo are registered trademarks of the College Board. Visit the College
More informationPeriodic Table Questions
Periodic Table Questions 1. The elements characterized as nonmetals are located in the periodic table at the (1) far left; (2) bottom; (3) center; (4) top right. 2. An element that is a liquid at STP is
More informationChapter 14 - Acids and Bases
Chapter 14 - Acids and Bases 14.1 The Nature of Acids and Bases A. Arrhenius Model 1. Acids produce hydrogen ions in aqueous solutions 2. Bases produce hydroxide ions in aqueous solutions B. Bronsted-Lowry
More informationCandidate Style Answer
Candidate Style Answer Chemistry A Unit F321 Atoms, Bonds and Groups High banded response This Support Material booklet is designed to accompany the OCR GCE Chemistry A Specimen Paper F321 for teaching
More informationUnit 10A Stoichiometry Notes
Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations
More informationAcids and Bases: A Brief Review
Acids and : A Brief Review Acids: taste sour and cause dyes to change color. : taste bitter and feel soapy. Arrhenius: acids increase [H ] bases increase [OH ] in solution. Arrhenius: acid base salt water.
More informationChapter 4 Chemical Reactions
Chapter 4 Chemical Reactions I) Ions in Aqueous Solution many reactions take place in water form ions in solution aq solution = solute + solvent solute: substance being dissolved and present in lesser
More informationAP Chemistry 2012 Free-Response Questions
AP Chemistry 01 Free-Response Questions About the College Board The College Board is a mission-driven not-for-profit organization that connects students to college success and opportunity. Founded in 1900,
More informationChem 1A Exam 2 Review Problems
Chem 1A Exam 2 Review Problems 1. At 0.967 atm, the height of mercury in a barometer is 0.735 m. If the mercury were replaced with water, what height of water (in meters) would be supported at this pressure?
More informationChemical Reactions 2 The Chemical Equation
Chemical Reactions 2 The Chemical Equation INFORMATION Chemical equations are symbolic devices used to represent actual chemical reactions. The left side of the equation, called the reactants, is separated
More informationChapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases
Chapter 17 Acids and Bases How are acids different from bases? Acid Physical properties Base Physical properties Tastes sour Tastes bitter Feels slippery or slimy Chemical properties Chemical properties
More informationMoles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe:
Like a recipe: Balancing Eqns Reactants Products 2H 2 (g) + O 2 (g) 2H 2 O(l) coefficients subscripts Balancing Eqns Balancing Symbols (s) (l) (aq) (g) or Yields or Produces solid liquid (pure liquid)
More informationFormulae, stoichiometry and the mole concept
3 Formulae, stoichiometry and the mole concept Content 3.1 Symbols, Formulae and Chemical equations 3.2 Concept of Relative Mass 3.3 Mole Concept and Stoichiometry Learning Outcomes Candidates should be
More informationFOR TEACHERS ONLY. The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING/CHEMISTRY
FOR TEACHERS ONLY PS CH The University of the State of New York REGENTS HIGH SCHOOL EXAMINATION PHYSICAL SETTING/CHEMISTRY Wednesday, January 29, 2003 9:15 a.m. to 12:15 p.m., only SCORING KEY AND RATING
More informationThe first law: transformation of energy into heat and work. Chemical reactions can be used to provide heat and for doing work.
The first law: transformation of energy into heat and work Chemical reactions can be used to provide heat and for doing work. Compare fuel value of different compounds. What drives these reactions to proceed
More informationThermodynamics and Equilibrium
Chapter 19 Thermodynamics and Equilibrium Concept Check 19.1 You have a sample of 1.0 mg of solid iodine at room temperature. Later, you notice that the iodine has sublimed (passed into the vapor state).
More informationCambridge International Examinations Cambridge International General Certificate of Secondary Education
Cambridge International Examinations Cambridge International General Certificate of Secondary Education *0123456789* CHEMISTRY 0620/03 Paper 3 Theory (Core) For Examination from 2016 SPECIMEN PAPER 1 hour
More informationAP Chemistry 2005 Scoring Guidelines Form B
AP Chemistry 2005 Scoring Guidelines Form B The College Board: Connecting Students to College Success The College Board is a not-for-profit membership association whose mission is to connect students to
More informationChapter 13. Properties of Solutions
Sample Exercise 13.1 (p. 534) By the process illustrated below, water vapor reacts with excess solid sodium sulfate to form the hydrated form of the salt. The chemical reaction is Na 2 SO 4(s) + 10 H 2
More information87 16 70 20 58 24 44 32 35 40 29 48 (a) graph Y versus X (b) graph Y versus 1/X
HOMEWORK 5A Barometer; Boyle s Law 1. The pressure of the first two gases below is determined with a manometer that is filled with mercury (density = 13.6 g/ml). The pressure of the last two gases below
More information