General Chemistry Study Guide
|
|
- Zoe Anthony
- 6 years ago
- Views:
Transcription
1 General Chemistry 1311 Study Guide Name : Louise K number: Date: Oct Instructor: Jingbo Louise Liu kfjll00@tamuk.edu 1
2 Chapter 04 & 05 (10 questions required and 5 questions for extra credit) Credited Questions 1. Which of the following compounds is insoluble in water? a. NaNO 3 b. Na 2 CO 3 c. CuS d. (NH 4 ) 2 SO 4 2. According to the solubility rules, which of the following compounds will be soluble in water? a. NaCl b. PbCO 3 c. AgCl d. CaSO 4 3. When aqueous solutions of NaOH and H 2 SO 4 are mixed, a reaction occurs. What ions, if any, are the spectator ions in this reaction? a. Na + & SO 4 b. H + & SO 4 c. H + & OH - d. NH + 4 & SO 4 4. The correct net ionic equation for the process which occurs when aqueous solutions of the electrolytes AgNO 3 and Na 2 S are mixed is: a. Ag + (aq) + Na 2 S (s) Na + (aq) + Ag 2 S(s) b. 2Ag + (aq) + S (aq) Ag 2 S(s) c. Ag + (aq) + S (aq) Ag 2 S(aq) d. AgNO 3 (aq) + Na 2 S (s) NaNO 3 (aq) + Ag 2 S(s) 5. The net ionic equation for the reaction between aqueous solutions of HCl and KOH is, a. H + (aq) + OH - (aq) H 2 O (aq) b. HCl (aq) + OH - (aq) H 2 O(l) + Cl - (aq) c. H + (aq) + OH - (aq) H 2 O (l) d. H + (aq) + OH - (aq) H 2 O (g) 6. What volume of a M solution of HCl is required to neutralize a solution 0.200M 10.0 ml of KOH solution? a. 20 ml b. 10 ml c. 100 ml d. 5 L 7. What are the products when aqueous solutions of HCl and Na 2 CO 3 react? a. NaCl and H 2 CO 3 b. Na 2 CO 3 and H 2 CO 3 c. NaCl, H 2 O and CO 2 d. HCl and CaSO 4 8. Equation: 3Cu(s) + 8HNO 3 (aq) 2NO(g) + 3Cu(NO 3 ) 2 (aq) + 4H 2 O(l) In the above reaction, the element oxidized is and is the reducing agent. a. Cu (s) and HNO 3 b. Cu (s) and Cu (s) c. Cu(NO 3 ) 2 (aq) and HNO 3 d. NO and Cu 9. What is the oxidation number of the polyatomic ion MnO - 4? a. +4 b. +5 c. +6 d In the equation shown below, which species, if any, is the oxidizing agent? Equation: Cr 2 O 7 + 2OH - 2CrO 4 + H 2 O a. Cr 2 O 7 b. CrO 4 c. OH - d. none of them is reducing agent. 2
3 11. Balance the following chemical equation: CH 3 OH (l) + O 2 (g) CO 2 (g) + H 2 O(g) a. CH 3 OH (l) + O 3 (g) CO 2 (g) + 2 H 2 O(g) b. 2 CH 3 OH (l) + 3 O 2 (g) 2 CO 2 (g) + 4 H 2 O(g) c. CH 3 OH (l) + 2 O 2 (g) CO 2 (g) + 2 H 2 O(g) d. CH 3 OH (l) + O 2 (g) CO 2 (g) + H 2 O(g) 12. What amount of bromine reacts with 4.0 mol of aluminum to produce AlBr 3? 2 Al(s) + 3 Br 2 (g) 2 AlBr 3 (s) a. 2.0 mol b. 4.0 mol c. 6.0 mol d. 12 mol 13. What mass of sodium will react with 1.23 g of chlorine gas to produce sodium chloride? 2 Na(s) + Cl 2 (g) 2 NaCl(s) a g (1.23/(35.45*2) * 2* b g c g d g 14. Which of the following statements concerning electrolytes are correct? 1) Soluble compounds are always strong electrolytes. 2) Elements, such as N 2, are weak electrolytes. 3) Strong acids, such as HCl, are strong electrolytes. a. 1 only. b. 2 only. c. 3 only. d. 2 and Which of the following compounds is a strong electrolyte? a. HNO 3 b. HNO 2 c. NH3 d. H 2 O e. HF ( strong acid, strong base, and soluble salts are usually strong electrolyte.) 16. Which of the following compounds is soluble in water? a. BaSO 4 b. Cu 2 O c. AgBr d. NaClO 3 e. Hg 2 Cl 2 ( compounds contains 1A elements (Na, K, NH 4 + ) are soluble. ) 17. In accordance with the solubility rules, which of the following is true when solutions of KCl(aq) and AgNO 3 (aq) are mixed? a. No precipitate will form. b. KAg 2+ will precipitate and Cl - and NO 3 - will be spectator ions. c. KNO 3 will precipitate and Ag + and Cl - will be spectator ions. d. ClNO 3 will precipitate and K + and Ag + will be spectator ions. e. AgCl will precipitate and K + and NO 3 - will be spectator ions. 18. What is the name of H 3 O +? a. Proton b. Hydronium c. Trihydrogen oxide cation d. Water cation 3
4 19. Which statement is correct in terms of the ph definition? a. ph is the measurement of concentration of an aqueous solution. b. ph is the measurement of acidity of an aqueous solution and defined as ph = -log[h + ] c. ph is the measurement of conductivity of an aqueous solution. d. ph is the measurement of acidity of an aqueous solution and defined as ph = -log[oh - ]. Credited Questions 11. The net ionic equation of FeBr 2 and AgNO 3 is, a. Ag + (aq) + Br - (s) AgBr (s) b. Ag + (aq) + Br - (aq) AgBr (s) c. Ag + (aq) + Br - (aq) AgBr (aq) d. AgNO 3 (aq) + FeCl 2 (aq) NaNO 3 (aq) + AgBr (s) 12. The net ionic equation for the reaction between aqueous solutions of H 2 CO 3 and NaOH is, a. 2H + (aq) + CO 3 (aq) H 2 O (l) + CO 2 (g) b. 2H + (aq) + CO 3 (aq) H 2 O (aq) +CO 2 (g) c. H + (aq) + OH - (aq) H 2 O (aq) d. H + (aq) + OH - (aq) H 2 O (g) 13. What is the oxidizing agent in the redox reaction: C 2 H 6 O + Cr 2 O 7 + H + C 2 H 4 O + H 2 O + Cr 3+ a. Cr 2 O 7 b. H 2 O c. C 2 H 6 O d. H + 4
5 1. Data: 2SO 2 (g) + O 2 (g) 2SO 3 (g) ΔH = -198 kj Use the data above to calculate the standard enthalpy change for the reaction below. Reaction: 2SO 3 (g) O 2 (g) + 2SO 2 (g) ΔH =? a kj (reverse reaction) b kj c kj d kj 2. Data: (1) 2H 2 (g) + O 2 (g) 2H 2 O(g) ΔH = kj (2) 2H 2 (g) + O 2 (g) 2H 2 O(l) ΔH = kj On the basis of the above data, determine the ΔH of H 2 O (g) H 2 O(l)? a kj (switch the direction of reaction (1) and change the sign of ΔH, (483.6+(-571.6)) b kj c kj d kj 3. Data: SO 2 (g) + ½O 2 (g) SO 3 (g) ΔH = kj Given the above data, calculate the enthalpy change ΔH when 120 g of SO 2 is converted to SO 3. a kj b kj c kj d kj moles of SO 2 = 120/ (molar mass), 120/( *2) *(-99.1) 4. A combustion reaction occurs in a bomb calorimeter. The temperature of the calorimeter and the 3.5 mol of water rose from 22.5 C to 32.5 C. The heat Determine the heat released by the combustion. (c = 4.18 J / g K, q= c m T) a kj b kj c kj d kj (3.5*18.016*( ) 5. Which equation is associated to the standard enthalpy of formation? a. CO(g) + NO(g) CO 2 (g) + ½ N 2 (g) b. 2Ag(s) + Cl 2 (g) 2AgCl(s ) c. ½ Ca(s) + C(graphite) + 3/2 O 2 (g) CaCO 3 (s) d. H 2 (g) + 2C(graphite) + N 2 (g) 2HCN(g) (find the equation only has one product, the product has only one mole) 6. Data: 2Ba(s) + O 2 (g) 2BaO(s) ΔH = kj (1) BaCO 3 (s) Ba (s) + CO 2 (g) + ½O 2 (g) ΔH = kj (2) Given the data above, calculate ΔH for the reaction below: BaO(s) + CO 2 (g) BaCO 3 (s) a kj b kj c kj d kj (Switch the direction of equation (1), and then divided by 2, switch the direction of equation (2): (-)( )/2 + (-)(+822.5) =
6 1. Steam is subject the phase change mol of steam at C is cooled to ice at C. Calculate total heat released. (5 pts) H cond. = kj/mol, H fus = 6.01 kj/mol, C (liquid water ) = J/(mol / C), C ice = J/(mol / C). 100 C H 1 = moles H cond. H 2 = moles c liquid T 0 C H 3 = moles H fus -40 C H 4 = moles c ice T H 1 H 2 H 3 H 4 H *40.67 = kj H *75.40*(100)/1000 = 9.42 kj H *6.01 = 7.52 kj H * * (40) / 1000 = 1.82 kj Total heat released = kj 2. Explain what the kinetics-molecular theory is (5 pts) Postulate 1: Particle Volume 1 Because the volume of an individual gas particle is so small compared to the volume of its container, the gas particles are considered to have mass, but no volume. Postulate 2: Particle Motion 2 3 Gas particles are in constant, random, straight-line motion except when they collide with each other or with the container walls. Postulate 3: Particle Collisions Collisions are elastic therefore the total kinetic energy (Ek) of the particles is constant. 6
7 3. Explain what the significance of different variable is in the ideal gas law. Meaning Commonly used unit P Partial pressure of gases atm (standard atmosphere) V Volume of the gas container L (liter) n Moles of gases mol T Absolute temperature K (Kelvin) R Ideal gas constant or universal constant atm L/(mol K) 4. Define three rules of thermo-chemistry. (5 pts) H and amount of substances H of forward and reverse reaction Hess Law Rules of thermo-chemistry The enthalpy change is directly proportional to the amount (moles) of the substances of interest. The enthalpy change for the forward reaction has the same digit but opposite sign compared with its reverse direction. The total enthalpy change for the overall reaction is the sum of the enthalpy changes for the individual reactions. 5. A 1.57 g sample of an unknown vapor occupies ml at C and mmhg. The empirical formula of the compound is CH 2. What is the molecular formula of the compound? The vapor behaves as an ideal gas. (5 pts) PV = nrt Molar mass = mass / moles mmhg To atm /760 = ml To liter /1000 = C To Kelvin = moles PV 1.033*0.5/( *331.63) = RT molar mass Mass 1.57/ = moles Molar mass of g/mol *2 = Empirical formula Molecular Formula (CH 2 )x X = / = C 6 H 12 is your molecular formula 7
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
More informationCHEMISTRY 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
More informationChem 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
More informationTYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
More informationPage 1. Exam 2 Review Summer A 2002 MULTIPLE CHOICE. 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l)
Page 1 MULTIPLE CHOICE 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l) The coefficient of HCl(aq) in the balanced reaction is. a) 1 b) 2 c) 3 d) 4 e) 0 2. Given the information
More informationb) Na 2 S(aq) + ZnCl 2 (aq) ZnS(s) + 2 NaCl(s)
Chem 111 2010 Name: Vining Exam #2, Version 23 1. Which of the following compounds are soluble in water: K 2 CO 3, CaCO 3, NiCO 3, and Fe 2 (CO 3 ) 3? a) K 2 CO 3 only b) K 2 CO 3 and CaCO 3 c) CaCO 3
More informationX212F Which of the following is a weak base in aqueous solution? A) H 2 CO 3 B) B(OH) 3 C) N 2 H 4 D) LiOH E) Ba(OH) 2
PX212SP14 Practice Exam II / Spring 2014 1. Which of the following statements are characteristic of acids? 1. They are proton donors. 2. They react with bases to produce a salt and water. 3. They taste
More informationUnit 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)
More informationSolubility 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
More informationChapter 4. Types of Chemical Reactions and Solution Stoichiometry
Chapter 4 Types of Chemical Reactions and Solution Stoichiometry Chapter 4 Table of Contents 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition
More informationChapter 4 Types of Chemical Reaction and Solution Stoichiometry
Chapter 4 Types of Chemical Reaction and Solution Stoichiometry Water, the Common Solvent One of the most important substances on Earth. Can dissolve many different substances. A polar molecule because
More informationChapter 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
More informationCHEM134- Fall 2018 Dr. Al-Qaisi Chapter 4b: Chemical Quantities and Aqueous Rxns So far we ve used grams (mass), In lab: What about using volume in lab? Solution Concentration and Solution Stoichiometry
More informationAqueous Reactions. The products are just the cation-anion pairs reversed, or the outies (A and Y joined) and the innies (B and X joined).
Aqueous Reactions Defining Aqueous Reactions Aqueous reactions are reactions that take place in water. To understand them, it is important to understand how compounds behave in water. Some compounds are
More informationExam 2, Ch 4-6 October 12, Points
Chem 130 Name Exam 2, Ch 4-6 October 12, 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
More informationMidterm Examination 2
CH 221 General Chemistry Spring 2012 Name: Midterm Examination 2 Useful Information is located on the last two pages of the Exam. Multiple Choice Questions A carton of Morton's Iodized Salt, NaCl with
More informationChemistry Stoichiometry and Heat Exam (ver.1) Mr. Thaler. Please do not write on this exam. Mark your answers on the scantron only.
1. Identify from the unbalanced equations below the one that does not represent a redox reaction. a. H 2O 2(aq) + MnO 4 - (aq) O 2(g) + Mn 2+ (aq) b. H 2(g) + N 2(g) NH 3(g) c. NaCl (aq) + AgNO 3(aq) NaNO
More informationChapter 4; Reactions in Aqueous Solutions. Chapter 4; Reactions in Aqueous Solutions. V. Molarity VI. Acid-Base Titrations VII. Dilution of Solutions
Chapter 4; Reactions in Aqueous Solutions I. Electrolytes vs. NonElectrolytes II. Precipitation Reaction a) Solubility Rules III. Reactions of Acids a) Neutralization b) Acid and Carbonate c) Acid and
More informationOH (ammonium hydroxide) are in 3.47 moles of NH 4. OH? 1 grams. 2 Na(s) + Cl 2. (g) 2 NaCl(s) (32.00 g/mol) according to the reaction C 3
Question #: 1 Posting ID: 423347 Course: CHE 105 2015 SU Instructor: Sarah Edwards How many grams of NH 4 OH (ammonium hydroxide) are in 3.47 moles of NH 4 OH? 1 grams Question #: 2 When 2.61 grams of
More informationAP Chemistry Semester 1 Practice Problems
AP Chemistry Semester 1 Practice Problems 1. Adipic Acid contains 49.32% C, 43.84% O, and 6.85% H by mass. What is the empirical formula? a) C 3 H 5 O 2 b) C 3 H 3 O 4 c) C 2 HO 3 d) C 2 H 5 O 4 e) C 3
More informationCH 221 Chapter Four Part II Concept Guide
CH 221 Chapter Four Part II Concept Guide 1. Solubility Why are some compounds soluble and others insoluble? In solid potassium permanganate, KMnO 4, the potassium ions, which have a charge of +1, are
More informationChapter 7 Chemical Reactions
Chapter 7 Chemical Reactions Evidence of Chemical Change Release or Absorption of Heat Color Change Emission of Light Formation of a Gas Formation of Solid Precipitate Tro's "Introductory 2 How Do We Represent
More informationCh 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
More informationChapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary
Chapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary 4.1 Water, the Common Solvent A. Structure of water 1. Oxygen s electronegativity is high (3.5) and hydrogen s is low (2.1)
More information7. A solution has the following concentrations: [Cl - ] = 1.5 x 10-1 M [Br - ] = 5.0 x 10-4 M
Solubility, Ksp Worksheet 1 1. How many milliliters of 0.20 M AlCl 3 solution would be necessary to precipitate all of the Ag + from 45ml of a 0.20 M AgNO 3 solution? AlCl 3(aq) + 3AgNO 3(aq) Al(NO 3)
More informationCHEM 101A EXAM 1 SOLUTIONS TO VERSION 1
CHEM 101A EXAM 1 SOLUTIONS TO VERSION 1 Multiple-choice questions (3 points each): Write the letter of the best answer on the line beside the question. Give only one answer for each question. B 1) If 0.1
More informationSlide 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
More informationAP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry
I. IUPAC Naming AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry For Ionic Compounds: Formula to Name: 1. Identify the cation (positive ion) by name, then identify the
More informationCH 223 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. Which of the following equations is the solubility
More informationName 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
More informationFall 2011 CHEM Test 4, Form A
Fall 2011 CHEM 1110.40413 Test 4, Form A Part I. Multiple Choice: Clearly circle the best answer. (60 pts) Name: 1. The common constituent in all acid solutions is A) H 2 SO 4 B) H 2 C) H + D) OH 2. Which
More information1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A % C % B % D %
1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A. 9.372 % C. 28.12 % B. 21.38 % D. 42.73 % 2. How many grams of phosphorus are in 35.70 g of P 2 O 5? A. 6.359 g C. 15.58 g B. 23.37 g D. 31.16
More informationChapter 6. Types of Chemical Reactions and Solution Stoichiometry
Chapter 6 Types of Chemical Reactions and Solution Stoichiometry Chapter 6 Table of Contents (6.1) (6.2) (6.3) (6.4) (6.5) (6.6) (6.7) (6.8) Water, the common solvent The nature of aqueous solutions: Strong
More informationSolution Chemistry. Chapter 4
Solution Chemistry Chapter 4 Covalent Molecule Dissolving in Water Ionic Compound Dissolving in Water Electrolytes and Nonelectrolytes Electrolytes/Nonelectrolytes Type Dissociation Electrical Conductivity
More informationChemistry 150/151 Review Worksheet
Chemistry 150/151 Review Worksheet This worksheet serves to review concepts and calculations from first semester General Chemistry (CHM 150/151). Brief descriptions of concepts are included here. If you
More information1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3?
1) Convert the following 1) 125 g to Kg 6) 26.9 dm 3 to cm 3 11) 1.8µL to cm 3 16) 4.8 lb to Kg 21) 23 F to K 2) 21.3 Km to cm 7) 18.2 ml to cm 3 12) 2.45 L to µm 3 17) 1.2 m to inches 22) 180 ºC to K
More informationReview Questions (Exam II)
Announcements Exam tonight, 7-8:15pm (locations posted on website) Conflict Exam, 5:15-6:30pm (114 Transportation Bldg) No lab this week! Start new material on Thursday (read chapter 10!) Review Questions
More informationChapter 4 Suggested end-of-chapter problems with solutions
Chapter 4 Suggested end-of-chapter problems with solutions a. 5.6 g NaHCO 1 mol NaHCO 84.01 g NaHCO = 6.69 10 mol NaHCO M = 6.69 10 mol 50.0 m 1000 m = 0.677 M NaHCO b. 0.1846 g K Cr O 7 1 mol K 94.0 g
More information(E) half as fast as methane.
Name AP Chem / / AP Chem Practice Exam #2 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 following.
More information1) REACTIONs: a) Al4C3(s) + H2O (l)=> Al(OH)3 (s) + CH4 (g) Solution : Al4C3(s) + 12 H2O (l)=> 4Al(OH)3 (s) + 3CH4 (g)
1) REACTIONs: a) Al4C3(s) + H2O (l)=> Al(OH)3 (s) + CH4 (g) Balance the reaction. Describe the chemical process represented by this reaction. Write the name of each single reactant and product. First,
More informationPractice questions for Chapter 4
Practice questions for Chapter 4 1. An unknown substance dissolves readily in water but not in benzene (a nonpolar solvent). Molecules of what type are present in the substance? A) neither polar nor nonpolar
More informationEXAM 3 CHEM 1310 WS09 Key Version #2
EXAM 3 CHEM 1310 WS09 Key Version #2 1. (p. 116) Select the correct name and chemical formula for the precipitate that forms when the following reactants are mixed. CuCl 2 (aq) + Na 2 CO 3 (aq) A. copper(ii)
More informationHW 7 KEY!! Chap. 7, #'s 11, 12, odd, 31, 33, 35, 39, 40, 53, 59, 67, 70, all, 77, 82, 84, 88, 89 (plus a couple of unassigned ones)
HW 7 KEY!! Chap. 7, #'s 11, 12, 15-21 odd, 31, 33, 35, 39, 40, 53, 59, 67, 70, 72-75 all, 77, 82, 84, 88, 89 (plus a couple of unassigned ones) 11) NOTE: I used the solubility rules that I have provided
More informationCH 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,
More informationThe solvent is the dissolving agent -- i.e., the most abundant component of the solution
SOLUTIONS Definitions A solution is a system in which one or more substances are homogeneously mixed or dissolved in another substance homogeneous mixture -- uniform appearance -- similar properties throughout
More informationCHEMpossible. Final Exam Review
CHEMpossible Final Exam Review 1. Given the following pair of reactions and their equilibrium constants: 2NO 2 (g) 2NO (g) + O 2 (g) K c = 15.5 2NO (g) + Cl 2 (g) 2 NOCl (g) K c = 3.20 10-3 Calculate a
More informationSolutions. Heterogenous Mixture (Not a Solution) Ice Water (w/ Ice Cubes) Smog Oil and Water
Solutions Unit 6 1 Solutions Homogenous Mixture (Solution) two or more substances mixed together to have a uniform composition, its components are not distinguishable from one another Heterogenous Mixture
More informationCHE105 SU17 Exam 2. Question #: 1. Question #: 2
CHE105 SU17 Exam 2 Your Name: Your ID: Question #: 1 The percent yield of a reaction is 68.9%. What is the actual yield for this reaction, if the theoretical yield is 26.0 grams? Actual yield = 1 g Report
More informationChapter 4: Stoichiometry of Chemical Reactions. 4.1 Writing and Balancing Chemical Equations
Chapter 4: Stoichiometry of Chemical Reactions 4.1 Writing and Balancing Chemical Equations A chemical equation represents or symbolizes a chemical reaction. o Substances are represents by their chemical
More informationCh 100: Fundamentals for Chemistry
Ch 100: Fundamentals for Chemistry Chapter 8: Chemical Equations Lecture Notes Chemical Equations (Intro) 1. Chemical equations are used to symbolically describe chemical reactions 2. In a chemical equation
More informationChapter 8 Chemical Reactions
Chemistry/ PEP Name: Date: Chapter 8 Chemical Reactions Chapter 8: 1 7, 9 18, 20, 21, 24 26, 29 31, 46, 55, 69 Practice Problems 1. Write a skeleton equation for each chemical reaction. Include the appropriate
More informationReactions in Aqueous Solutions
Reactions in Aqueous Solutions 1 Chapter 4 General Properties of Aqueous Solutions (4.1) Precipitation Reactions (4.2) Acid-Base Reactions (4.3) Oxidation-Reduction Reactions (4.4) Concentration of Solutions
More informationChapter 4. Properties of Aqueous Solutions. Electrolytes in Aqueous Solutions. Strong, weak, or nonelectrolyte. Electrolytic Properties
Chapter 4 Reactions in Aqueous Solution Observing and Predicting Reactions How do we know whether a reaction occurs? What observations indicate a reaction has occurred? In your groups, make a list of changes
More informationMolecule smallest particle of a substance having its chemical properties Atoms connected via covalent bonds Examples:
Ionic equations, calculations involving concentrations, stoichiometry MUDr. Jan Pláteník, PhD Molecule smallest particle of a substance having its chemical properties Atoms connected via covalent bonds
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 informationSolutions & Solubility: Net Ionic Equations (9.1 in MHR Chemistry 11)
Solutions & Solubility: Net Ionic Equations (9.1 in MHR Chemistry 11) 1 Solubility vs. Temperature 2 Solubility Table Anions SOLUBILITY Table 8.3 page 363 in MHR Cl Br I S OH SO CO 3 PO 3 SO 3 C 2 H 3
More informationCHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY
Advanced Chemistry Name Hour Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY Day Plans
More informationUNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12)
I. Multiple Choice UNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12) 1) Which one of the following would form an ionic solution when dissolved in water? A. I 2 C. Ca(NO 3 ) 2 B. CH 3 OH D.
More informationChem 110 General Principles of Chemistry
Chem 110 General Principles of Chemistry Chapter 3 (Page 88) Aqueous Reactions and Solution Stoichiometry In this chapter you will study chemical reactions that take place between substances that are dissolved
More informationKwantlen Polytechnic University Chemistry 1105 S10 Spring Term Test No. 3 Thursday, April 4, 2013
Kwantlen Polytechnic University Chemistry 1105 S10 Spring Term Test No. 3 Thursday, April 4, 2013 Name: Student Number Instructions: Ensure that this exam contains all eight pages including this page.
More information11/3/09. Aqueous Solubility of Compounds. Aqueous Solubility of Ionic Compounds. Aqueous Solubility of Ionic Compounds
Aqueous Solubility of Compounds Not all compounds dissolve in water. Solubility varies from compound to compound. Chapter 5: Chemical Reactions Soluble ionic compounds dissociate. Ions are solvated Most
More informationOctober 19, 1999 Page 1. Chapter 4 Practice Worksheet Dr. Palmer Graves, Instructor MULTIPLE CHOICE
October 19, 1999 Page 1 MULTIPLE CHOICE Section 4.1 Some Ways that Chemical Reactions Occur 1. The reaction of HNO (aq) + KOH(aq) KNO (aq) + H O(l) is best classified as a(n) a) acid-base neutralization
More informationCHEMICAL REACTIONS. Introduction. Chemical Equations
CHEMICAL REACTIONS Chemistry I Chapter 7 1 Chemical Equations Their Job: Depict the kind of reactants and products and their relative amounts in a reaction. 4 Al (s) + 3 O 2 (g) ---> 2 Al 2 O 3 (s) The
More informationA reaction in which a solid forms is called a precipitation reaction. Solid = precipitate
Chapter 7 Reactions in Aqueous Solutions 1 Section 7.1 Predicting Whether a Reaction Will Occur Four Driving Forces Favor Chemical Change 1. Formation of a solid 2. Formation of water 3. Transfer of electrons
More information3. Which of the following compounds is soluble? The solubility rules are listed on page 8.
1. Classify the following reaction. Sb 2 O 3 + 3 Fe 2 Sb + 3 FeO a) Combination reaction b) Decomposition reaction c) Neutralization reaction d) Single-replacement reaction e) Double-replacement reaction
More informationChapter 9. Vocabulary Ch Kick Off Activity. Objectives. Interpreting Formulas. Interpreting Formulas
Chapter 9 Chemical Vocabulary Ch. 9.1 Chemical reaction Reactant Product Word Equation Skeleton Equation Chemical equation Coefficient 1 2 Objectives Write chemical equations to describe chemical reactions
More informationSolubility & Net Ionic review
Solubility & Net Ionic review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which of the following statements is/are correct? 1. All ionic compounds
More informationChemistry 112, Spring 2006 Prof. Metz Final Exam Name Each question is worth 4 points, unless otherwise noted
Chemistry 112, Spring 2006 Prof. Metz Final Exam Name Each question is worth 4 points, unless otherwise noted 1. The predominant intermolecular attractive force in solid sodium is: (A) metallic (B) ionic
More informationElectrolytes do conduct electricity, in proportion to the concentrations of their ions in solution.
Chapter 4 (Hill/Petrucci/McCreary/Perry Chemical Reactions in Aqueous Solutions This chapter deals with reactions that occur in aqueous solution these solutions all use water as the solvent. We will look
More informationHomework #3 Chapter 4 Types of Chemical Reactions and Solution Stoichiometry
Homework #3 Chapter 4 Types of Chemical Reactions and Solution Stoichiometry 13. Determine the concentrations of the solutions Solution A 4 particles 1.0 L Solution B 6 paticles 4.0 L Solution C 4 particles
More informationM = Molarity = mol solute L solution. PV = nrt % yield = actual yield x 100 theoretical yield. PM=dRT where d=density, M=molar mass
Solubility Rules: 1. Most nitrate salts are soluble. 2. Most salts of alkali metals and ammonium cations are soluble. 3. Most chloride, bromide and iodide salts are soluble. Exceptions: salts containing
More informationGAS FORMULAE THE GENERAL GAS EQUATION. 1 dm = 1000 ml = 1 L. 1cm = 1 ml
GAS FORMULAE THE GENERAL GAS EQUATION PV = nrt Note Useful Conversions P = Pressure ( kpa ) 760 mmhg = 1 atmosphere V = Volume ( L ) = 101,35Pa = 101.35 kpa n = Amount (in mol) of gas ( mol) 1 1 R = Gas
More information1. Rank the following elements in order of increasing atomic radius: P, Al, Cl, F, S
Useful constants and other information: R = 0.0821 LCatm/KCmole R = 8.314 J/KCmole h = 6.626 x 10-34 JCs 1 atm = 760 torr Specific heat of H 2 O(l) = 4.184 J/gC C 1 cal = 4.184 J c = 3 x 10 8 m/s PART
More informationChapter 4. Chemical Quantities and Aqueous Reactions
Lecture Presentation Chapter 4 Chemical Quantities and Aqueous Reactions Reaction Stoichiometry: How Much Carbon Dioxide? The balanced chemical equations for fossilfuel combustion reactions provide the
More informationPage III-4b-1 / Chapter Four Part II Lecture Notes. Chemistry 221 Professor Michael Russell MAR. Ba(NO3)2(aq)? soluble. BaCl2(aq)?
Page III-4b-1 / Chapter Four Part II Lecture Notes Solution Stoichiometry and Chemical Reactions Chapter 3 & Chapter 4, or Chapter 4 Part II Chemistry 221 Professor Michael Russell Terminology In solution
More informationChapter 9 Practice Worksheet: Reactions in Aqueous Solutions
Chapter 9 Practice Worksheet: Reactions in Aqueous Solutions 1. The compound H 2 S is classified as a weak electrolyte. Describe/draw how it reacts when placed in water. Completely dissociates in water.
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 informationSectional Solutions Key
Sectional Solutions Key 1. For the equilibrium: 2SO 2 (g) + O 2 (g) 2SO 3 (g) + 188 kj, the number of moles of sulfur trioxide will increase if: a. the temperature of the system is increased (at constant
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 informationPart One: Ions in Aqueous Solution
A. Electrolytes and Non-electrolytes. CHAPTER FOUR: CHEMICAL REACTIONS Part One: Ions in Aqueous Solution 1. Pure water does not conduct electric current appreciably. It is the ions dissolved in the water
More informationChapter 4. Reactions In Aqueous Solution
Chapter 4 Reactions In Aqueous Solution I) General Properties of Aqueous Solutions Homogeneous mixture on a molecular level - prop. same throughout - separable by physical means - variable composition
More informationChapter 4: Types of Chemical Reactions and Solution Stoichiometry
Chapter 4: Types of Chemical Reactions and Solution Stoichiometry Collision A bag of mostly water - Star Trek - Rareness No mobility Solution is the solution. Water, the Common Solvent A bag of mostly
More information22. What is the maximum concentration of carbonate ions that will precipitate BaCO 3 but not MgCO 3 from a solution that is 2.
PX312-1718 1. What is the solubility product expression for Th(IO 3 ) 4? A) K sp = [Th 4+ ][4IO 3 ] 4 B) K sp = [Th 4+ ][IO 3 ] C) K sp = [Th][IO 3 ] 4 D) K sp = [Th 4+ ][IO 3 ] 4 E) K sp = [Th 4+ ][IO
More informationChapter 4 - Types of Chemical Reactions and Solution Chemistry
Chapter 4 - Types of Chemical Reactions and Solution Chemistry 4.1 Water, the Common Solvent - the water molecule is bent with and H-O-H angles of approx. 105 º - O-H bonds are covalent - O is slightly
More informationWYSE Academic Challenge 2004 Sectional Chemistry Solution Set
WYSE Academic Challenge 2004 Sectional Chemistry Solution Set 1. Answer: d. Assume 100.0 g of the compound. Thus, we have 40.00 g of carbon, or 40.00/12.01 = 3.33 mol C. We have 6.71 g of hydrogen, or
More informationChapter 4 Chemical Formulas, Reactions, Redox and Solutions
Terms to Know: Solubility Solute Solvent Solution Chapter 4 the amount of substance that dissolves in a given volume of solvent at a given temperature. a substance dissolved in a liquid to form a solution
More informationChemistry Spring 2018 Final Exam Review
Name Date Period Chemistry Spring 2018 Final Exam Review TURN THIS COMPLETED REVIEW IN TO YOUR TEACHER BY DAY OF YOUR FINAL FOR A 5 point FINAL EXAM BONUS Unit #7 Moles 1. What is a mole? 2. What is molar
More information(A) Composition (B) Decomposition (C) Single replacement (D) Double replacement: Acid-base (E) Combustion
AP Chemistry - Problem Drill 08: Chemical Reactions No. 1 of 10 1. What type is the following reaction: H 2 CO 3 (aq) + Ca(OH) 2 (aq) CaCO 3 (aq) + 2 H 2 O (l)? (A) Composition (B) Decomposition (C) Single
More informationGeneral Chemistry Review
General Chemistry Review Helping you remember what you learned, oh, so long ago. Topics (Until we run out of time) The mole Stoichiometry Limiting Reactants Solution Chemistry Molarity Dilution Stoichiometry
More information11-1 Notes. Chemical Reactions
11-1 Notes Chemical Reactions Chemical Reactions In a chemical reaction 1 or more substances (the reactants) change into 1 or more new substances (the products). Reactants are always written on the left
More informationCHEMISTRY 102A Spring 2012 Hour Exam II. 1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with:
. My answers for this Chemistry 0 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E. A sample of LSD (D-lysergic acid diethylamide, C 4 H 30
More informationChemical Equilibrium
Chemical Equilibrium THE NATURE OF CHEMICAL EQUILIBRIUM Reversible Reactions In theory, every reaction can continue in two directions, forward and reverse Reversible reaction! chemical reaction in which
More informationCHAPTER Describing Chemical Reactions Reactants Products. New substances produced The arrow means yields TYPES OF EQUATIONS.
CHAPTER 11 Chemical Reactions 11.1 Describing Chemical Reactions Reactants Products New substances produced The arrow means yields Where do Chemical Reactions occur? Everywhere!!! In living organisms In
More informationWhat 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
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
More information7/16/2012. Chapter Four: Like Dissolve Like. The Water Molecule. Ionic Compounds in Water. General Properties of Aqueous Solutions
General Properties of Aqueous Solutions Chapter Four: TYPES OF CHEMICAL REACTIONS AND SOLUTION STOICHIOMETRY A solution is a homogeneous mixture of two or more substances. A solution is made when one substance
More informationAssignment 04 (A) a) ii and iii b) i, ii, and iii c) i, iv, and v d) iii e) ii (These are molecular compounds.)
Assignment 04 (A) 1- Which of the following are nonelectrolytes in water? (i) HF (ii) ethanol, C 2 H 5 OH (iii) C 12 H 22 O 11 (iv) KClO 3 (v) Cu(NO 3 ) 2 a) ii and iii b) i, ii, and iii c) i, iv, and
More information2. Write a balanced chemical equation which corresponds to the following equilibrium constant expression.
Practice Problems for Chem 1B Exam 1 Chapter 14: Chemical Equilibrium 1. Which of the following statements is/are CORRECT? 1. For a chemical system, if the reaction quotient (Q) is greater than K, products
More informationChapter 8. Chemical Equations. Flames and sparks result when aluminum foil is dropped Into liquid bromine.
Chapter 8 Chemical Equations Flames and sparks result when aluminum foil is dropped Into liquid bromine. Introduction to General, Organic, and Biochemistry 10e John Wiley & Sons, Inc Morris Hein, Scott
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 information