Exam 1 Chemistry 142, Spring 2005 March 2, 2005
|
|
- Ophelia Bell
- 6 years ago
- Views:
Transcription
1 Exam Chemistry 4, Spring 005 March, 005 Part. Answer 7 of the following 8 multiple choice questions. If you answer more than 7 cross out the one you wish not to be graded, otherwise only the first 7 will be graded. 4 points each.. The value of K eq for the following reaction is 0.5: SO (g) + NO (g) SO 3 (g) + NO(g) The value of K eq at the same temperature for the reaction below is. SO (g) + NO (g) SO 3 (g) + NO(g) A) 0.50 B) 0.06 C) 0. D) 0.5 E) 6. Acetic acid is a wea acid that dissociates into the acetate ion and a proton in aqueous solution: HC H 3 O (aq) C H 3 O - (aq) + H + (aq) At equilibrium at 5 C a 0.00 M solution of acetic acid has the following concentrations: [HC H 3 O ] = M, [C H 3 O - ] = M, and [H + ] = M. The equilibrium constant, K eq, for the ionization of acetic acid at 5 C is. A) B) 0.00 C) D) E) Consider the following reaction at equilibrium. CO (g) CO(g) + O (g) H = -54 J Le Châtelier s Principle predicts that the partial pressure of CO(g) can be maximized by carrying out the reaction. A) at high temperature and high pressure B) at high temperature and low pressure C) at low temperature and low pressure D) at low temperature and high pressure E) in the presence of solid carbon
2 4. Which energy difference in the energy profile below corresponds to the activation energy for the forward reaction? Energy x y A) x B) y C) x + y D) x y E) y x Reaction pathway 5. Which one of the following will change the value of an equilibrium constant? A) changing temperature B) adding other substances that do not react with any of the species involved in the equilibrium C) varying the initial concentrations of reactants D) varying the initial concentrations of products 6. Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: NO NO + O In a particular experiment at 300 C, [NO ] drops from to M in 00s. The rate of disappearance of NO for this period is M/s. A) 0.35 B) C) D) E).8 0-3
3 7. The reaction CH 3 -N C CH 3 -C N is a first-order reaction. At 30.3 C, = s -. If [CH 3 -N C] is initially, [CH 3 -N C] is after s. A) B) C) D) E) The effect of a catalyst on a chemical reaction is to. A) lower the activation energy B) accelerate the forward reaction only C) mae reactions more exothermic D) react with product, effectively removing it and shifting the equilibrium to the right Part. Answer 4 of the following 5 short answer questions. If you answer more than 4 cross out the one you wish not to be graded, otherwise only the first 4 will be graded. 6 points each. 9. In the following reaction label the two sets of conjugate acid-base pairs. To do this draw a line between both members of each pair and label each as an acid or a base: NH 3 + H O + NH 4 + OH - Base Acid Acid Base 0. Predict the products for the following reactions. Does the equilibrium position lie to the left or right for each? (a) O - + H O OH - Equilibrium lies to the right (O - is a strong base). Also do the "tug-of-war": O -..H OH, the oxide ion has the larger charge, so it will be the stronger base. However, OH - is the strongest base that can exist in aqueous solution. (b) HOAc + H O H 3 O + + OAc - Equilibrium lies to the left (HOAc is a wea acid) where HOAc is acetic acid (or CH 3 COOH).
4 . HF (K a = ) is a stronger acid than HCN (K a = ). Which is the stronger conjugate base, F - or CN -? CN - is the conjugate base of the weaer acid HCN (relative to HF), and is therefore a stronger conjugate base (relative to F - ).. For the reaction NO + CO NO + CO the experimental rate law is rate = [NO ] The following mechanism has been proposed: NO NO 3 + NO NO 3 + CO NO + CO a. Which step is the rate determining step? Step (see rate law) b. Is there a reactive intermediate in this reaction? If so what is it? Yes. The reactive intermediate is NO 3 (produced in step and consumed in step ) 3. The rate law for a third order reaction is [A] - = t [A] o To mae a straight line plot to verify third order behavior, a. what would you plot on the vertical axis? /[A] b. what would you plot on the horizontal axis? t c. what would the slope equal?
5 Part 3. Answer all of the following questions. points each. 4. At 00 C, the equilibrium constant for the reaction below is NO(g) N (g) + O (g) A closed vessel is charged with 36. atm of NO. At equilibrium, what is the partial pressure of O? NO(g) N (g) + O (g) Initial (atm) Changes -x +x +x Equilibrium (atm) 36. x x x K eq P = P N PNO x (36. x) Tae the square root of both sides Thus, the partial pressure of O x = x x = x 98.98x = x = 7.9 O =.40 0 =.40x0 3 3 at equilibrium is7.9 atm.
6 5. Determine the rate law for the reaction NO (g) + Br (g) NOBr (g) from the following initial rate study. (Write the full rate law in the form: rate =?) [NO] (mol L - ) [Br ] (mol L - ) Rate (mol L - sec - ) Rate = [NO] x [Br ] y Order with respect to [NO]: By inspection we see that as we double the concentration of NO (experiments and ) while holding [Br ] constant, the initial rate of the reaction doubles therefore, we can say that the reaction is first-order with respect to [NO]. Order with respect to [Br ]: By inspection we see that as we double the concentration of Br (experiments and 3) while holding [NO] constant, the initial rate of the reaction increases by a factor of 4 therefore we can say that the reaction is second-order with respect to [Br ]. Rate = [NO][Br ] 6. For the first-order reaction N O 5 N O 4 + O, the activation energy is 06 J/mol. How many times faster will the reaction go at 00 C than at 5 C? ln T T T ln T E R = T = 373. K, T = 98. K 06 J/mol = J/mol K 373. K 98. K a ln E a = R T T = 06 J/mol 373. K 98. K = J/mol K = K times as fast 98. K
7 7. A reaction that is second order in reactant A has [A] o = 0.00 M. The half-life is 45.6 sec. What is [A] after 3.00 min?. Find the rate constant, : For a second-order reaction the half-life, t /, is related to as follows: / = = 0.00M 45.6s t o - = 0.09 M s. [A] after 3 minutes (80 s) is related to [A] o as follows (for a second-order process): 80s 80s 80s 80s = + t - = + (0.09 M s 0.00M = 4.6 M - = M o )(80s) TOTAL EXAM OUT OF 00 EXAM % 0.95 TOTAL HW OUT OF HW % 0.05 FINAL CORRECTED EXAM
8 R = L atm mol - K - = 8.34 J mol - K - T(O C) = 73.K K w =.0x0-4 x = -b ± b - 4ac a ln [A] t [A] = - t ln [A] t = - t + ln [A] o [A] t = [A] o o e - t - = t [A] t [A] o t ½ = -ln ½ = t ½ = [A] o = A e -E a/rt ln = - E a R T + ln A ln T T = - E a R T - or ln T = E a T T R T - T
B. The rate will increase by a factor of twelve. C. The rate will increase by a factor of twenty-four. D. The rate will decrease by a factor of six.
1. If O 2 (g) disappears at a rate of 0.250 M/s at a particular moment in the reaction below, what is the rate of appearance of H 2 O(g) at the same time? C 3 H 8 (g) + 5 O 2 (g) 3 CO 2 (g) + 4 H 2 O(g)
More informationName (please print) Chemistry Last Name First Name Test #2 Zumdahl, Chapters 13 and 14 March 1, 2004
Form L Name (please print) Chemistry 1302-003 Last Name First Name Test #2 Zumdahl, Chapters 13 and 14 March 1, 2004 Instructions: 1. This exam consists of 25 questions. 2. No scratch paper is allowed.
More informationChem 106 Thursday, March 10, Chapter 17 Acids and Bases
Chem 106 Thursday, March 10, 2011 Chapter 17 Acids and Bases K a and acid strength Acid + base reactions: Four types (s +s, s + w, w + s, and w + w) Determining K from concentrations and ph ph of aqueous
More information2. For the reaction H 2 (g) + Br 2 (g) 2 HBr, use the table below to determine the average [Br 2 ] from 20.0 to 30.0 seconds.
1. The rate of the reaction A X is defined as A. Δ[A]/Δtime. B. the time it takes to convert all of A to X. C. [A] initial /Δtime. D. ([X]-[A])/Δtime. 2. For the reaction H 2 (g) + Br 2 (g) 2 HBr, use
More informationEquilibrium & Reaction Rate
Equilibrium & Reaction Rate 1. One of the important reactions in coal gasification is the catalytic methanation reaction: CO(g) + H (g) H O(g) + CH 4 (g) H 06 kj a) Predict the direction in which this
More informationChapter 15 Equilibrium
Chapter 15. Chemical Equilibrium 15.1 The Concept of Equilibrium Chemical equilibrium is the point at which the concentrations of all species are constant. A dynamic equilibrium exists when the rates of
More informationRepresentative Exam Questions On The Topic of Equilibrium (Includes Acid / Base Equilibria)
Representative Exam Questions On The Topic of Equilibrium (Includes Acid / Base Equilibria) 1. If a chemical equilibrium very much favors the products over the reactants, what would we expect its equilibrium
More informationAP Chapter 13: Kinetics Name
AP Chapter 13: Kinetics 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 13: Kinetics 2 Warm-Ups (Show your work for credit) Date 1.
More information1. (4) For this reaction: NO 2. + H 3 AsO 3 D H 2 AsO 3
Exam 1 Chem 1B, Spring 2017 Fossum Name: There are 6 points of extra credit built in to this exam. Always show your work and explain your reasoning, include units, and check significant figures. Note:
More information4) What is the order of the reaction with respect to ClO2? 4) A) 2 B) 1 C) 4 D) 0 E) 3
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 1) 2NO2 2NO
More informationGeneral Chemistry II CHM 1046 E Exam 2
General Chemistry II CHM 1046 E Exam 2 Dr. Shanbhag Name: 1. The formation of ammonia from elemental nitrogen and hydrogen is an exothermic process. N 2 (g) + 3 H 2 (g) 2 NH 3 (g) H= -92.2 kj Which of
More informationAP Chem Chapter 14 Study Questions
Class: Date: AP Chem Chapter 14 Study Questions 1. A burning splint will burn more vigorously in pure oxygen than in air because a. oxygen is a reactant in combustion and concentration of oxygen is higher
More information1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases
Chemistry 12 Acid-Base Equilibrium II Name: Date: Block: 1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases Strengths of Acids and
More informationChapter 15 Equilibrium
Chapter 15. Chemical Equilibrium Sample Exercise 15.1 (p. 632) Write the equilibrium expression for K eq for these three reactions: a) 2 O 3(g) 3 O 2(g) b) 2 NO (g) + Cl 2(g) 2 NOCl (g) c) Ag + (aq) +
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 informationExam 2 Sections Covered: (the remaining Ch14 sections will be on Exam 3) Useful Information Provided on Exam 2:
Chem 101B Study Questions Name: Chapters 12,13,14 Review Tuesday 2/28/2017 Due on Exam Thursday 3/2/2017 (Exam 2 Date) This is a homework assignment. Please show your work for full credit. If you do work
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. A) B) 1588 C) 397 D) 28 E) 0.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The value of Keq for the equilibrium 1) H2 (g) + I2 (g) 2 HI (g) is 794 at 25 C. What
More informationExam 4, Ch 14 and 15 December 7, Points
Chem 130 Name Exam 4, Ch 14 and 15 December 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
More informationKinetics. 1. Consider the following reaction: 3 A 2 B How is the average rate of appearance of B related to the average rate of disappearance of A?
Kinetics 1. Consider the following reaction: 3 A 2 B How is the average rate of appearance of B related to the average rate of disappearance of A? A. [A]/ t = [B]/ t B. [A]/ t = (2/3)( [B]/ t) C. [A]/
More informationClass Results Simulator:
Class Results http://chemconnections.org/general/chem120/equil-graph.html Simulator: http://chemconnections.org/java/equilibrium/ http://chemconnections.org/general/chem120/equil-graph.html The changes
More informationCHEM Dr. Babb s Sections Lecture Problem Sheets
CHEM 116 - Dr. Babb s Sections Lecture Problem Sheets Kinetics: Integrated Form of Rate Law 61. Give the integrated form of a zeroth order reaction. Define the half-life and find the halflife for a general
More informationBrown et al, Chemistry, 2nd ed (AUS), Ch. 12:
Kinetics: Contents Brown et al, Chemistry, 2 nd ed (AUS), Ch. 12: Why kinetics? What is kinetics? Factors that Affect Reaction Rates Reaction Rates Concentration and Reaction Rate The Change of Concentration
More informationCHEM Chapter 14. Chemical Kinetics (Homework) Ky40
CHEM 1412. Chapter 14. Chemical Kinetics (Homework) Ky40 1. Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2ClO 2 (aq) + 2OH (aq) ClO
More informationAP CHEMISTRY NOTES 7-1 KINETICS AND RATE LAW AN INTRODUCTION
AP CHEMISTRY NOTES 7-1 KINETICS AND RATE LAW AN INTRODUCTION CHEMICAL KINETICS the study of rates of chemical reactions and the mechanisms by which they occur FACTORS WHICH AFFECT REACTION RATES 1. Nature
More informationChapter 15 Equilibrium
Chapter 15. Chemical Equilibrium Common Student Misconceptions Many students need to see how the numerical problems in this chapter are solved. Students confuse the arrows used for resonance ( )and equilibrium
More informationKinetics Practice Test 2017 Name: date: 1. Use the data provided the answer the question.
Kinetics Practice Test 2017 Name: date: 1. Use the data provided the answer the question. The data above was obtained for a reaction in which X + Y Z. Which of the following is the rate law for the reaction?
More informationReview for Exam 2 Chem 1721/1821
Review for Exam 2 Chem 1721/1821 The following are the major concepts with which you should be well acquainted from Chapters 13, 14, 15, 16.1-16.3: Chapter 13: Chemical Kinetics Reaction Rates The rate
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. A) 1588 B) C) 28 D) 397 E) 0.
Chapter 15 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The value of Keq for the equilibrium 1) H2 (g) + I2 (g) 2 HI (g) is 794 at 25 C. What
More informationChapter 14: Chemical Kinetics
1. Which one of the following units would not be an acceptable way to express reaction rate? A) M/s B) M min 1 C) L mol 1 s 1 D) mol L 1 s 1 E) mmhg/min 3. For the reaction BrO 3 + 5Br + 6H + 3Br 2 + 3H
More informationChem 105 Tuesday March 8, Chapter 17. Acids and Bases
Chem 105 Tuesday March 8, 2011 Chapter 17. Acids and Bases 1) Define Brønsted Acid and Brønsted Base 2) Proton (H + ) transfer reactions: conjugate acid-base pairs 3) Water and other amphiprotic substances
More informationPart A: Multiple Choice (23 marks total)
Part A: Multiple Choice (23 marks total) Use the answer sheet found at the end of this examination to answer the multiple-choice questions in this section. Shade in the circle that corresponds to your
More informationChapter 14. Chemical Kinetics
Sample Exercise 14.1 (p. 578) For the reaction pictured at the bottom of the previous page, calculate the average rate at which A disappears over the time interval from 20 s to 40 s. (1.2 x 10-2 M/s) Practice
More informationCHEM 102 Winter 10 Exam 2(a)
CHEM 102 Winter 10 Exam 2(a) On the answer sheet (scantron) write your Name, Student ID Number, and Recitation Section Number. Choose the best (most correct) answer for each question AND ENTER IT ON YOUR
More informationCHEMISTRY. Chapter 14 Chemical Kinetics
CHEMISTRY The Central Science 8 th Edition Chapter 14 Kozet YAPSAKLI kinetics is the study of how rapidly chemical reactions occur. rate at which a chemical process occurs. Reaction rates depends on The
More information3 Chemical Equilibrium
Aubrey High School AP Chemistry 3 Chemical Equilibrium Name Period Date / / 3.1 Problems Chemical Analysis 1. Write the equilibrium constant expressions for the following reactions. How are they related
More informationAP Study Questions
ID: A AP 16.4-16.7 Study Questions Multiple Choice Identify the choice that best completes the statement or answers the question. 1 What is the ph of an aqueous solution at 25.0 C in which [H + ] is 0.0025
More informationChapter 14. Chemical Kinetics
Chapter 14. Chemical Kinetics Common Student Misconceptions It is possible for mathematics to get in the way of some students understanding of the chemistry of this chapter. Students often assume that
More informationReturn Exam 3 Review for final exam: kinetics, equilibrium, acid-base
Chem 106 Thurs. 5-5-2011 Return Exam 3 Review for final exam: kinetics, equilibrium, acid-base Hour Ex 3; Ave=64, Hi=94 5/5/2011 1 ACS Final exam question types Topic # Calcul n Qualitative Intermol forces
More informationChapters 10 and 11 Practice MC
Chapters 10 and 11 Practice MC Multiple Choice Identify the choice that best completes the statement or answers the question. d 1. Which of the following best describes the rates of chemical reaction?
More information1. The reaction between solid barium hydroxide and solid ammonium chloride can be represented by the equation below.
1. The reaction between solid barium hydroxide and solid ammonium chloride can be represented by the equation below. Ba(OH) 2 (s) + 2NH 4 Cl(s) BaCl 2 (s) + 2NH 3 (g) + 2H 2 O(l) ΔH ο = +51.1 kj mol 1
More informationK P VERSUS K C PROPERTIES OF THE EQUILIBRIUM CONSTANT
K P VERSUS K C 1. What are the units of K p and K c for each of the following? a) 2H 2 S(g) 2H 2 (g) + S 2 (g) b) 4NH 3 (g) + 3O 2 (g) 2N 2 (g) + 6H 2 O(g) 2. What are the units of K p and K c for each
More informationAP Chemistry Big Idea Review
Name: AP Chemistry Big Idea Review Background The AP Chemistry curriculum is based on 6 Big Ideas and many Learning Objectives associated with each Big Idea. This review will cover all of the Big Ideas
More informationC h a p t e r 13. Chemical Equilibrium
C h a p t e r 13 Chemical Equilibrium Chemical equilibrium is achieved when: the rates of the forward and reverse reactions are equal and the concentrations of the reactants and products remain constant
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) The effect of a catalyst on a chemical reaction is to. A) increase the entropy change
More informationCHEM 36 General Chemistry EXAM #2 March 13, 2002
CHEM 36 General Chemistry EXAM #2 March 13, 2002 Name: Key INSTRUCTIONS: Read through the entire exam before you begin. Answer all of the questions. For questions involving calculations, show all of your
More informationconcentrations (molarity) rate constant, (k), depends on size, speed, kind of molecule, temperature, etc.
#73 Notes Unit 9: Kinetics and Equilibrium Ch. Kinetics and Equilibriums I. Reaction Rates NO 2(g) + CO (g) NO (g) + CO 2(g) Rate is defined in terms of the rate of disappearance of one of the reactants,
More informationAcids and Bases. A strong base is a substance that completely ionizes in aqueous solutions to give a cation and a hydroxide ion.
Acid-Base Theories Arrhenius Acids and Bases (1884) Acids and Bases An acid is a substance that, when dissolved in water, increases the concentration of hydrogen ions. A base is a substance that, when
More informationChemical Equilibrium
Chemical Equilibrium Concept of Equilibrium Equilibrium Constant Equilibrium expressions Applications of equilibrium constants Le Chatelier s Principle The Concept of Equilibrium The decomposition of N
More informationCalculations Involving the Equilibrium Constant K eq )
Calculations Involving the Equilibrium Constant K eq ) 1. Given the equilibrium equation below: A 2(g) + B 2(g) 2AB (g) If, at equilibrium, the concentrations are as follows: [A 2 ] = 3.45 M, [B 2 ] =
More informationCHEM Dr. Babb s Sections Exam #3 Review Sheet
CHEM 116 Dr. Babb s Sections Exam #3 Review Sheet Acid/Base Theories and Conjugate AcidBase Pairs 111. Define the following terms: Arrhenius acid, Arrhenius base, Lewis acid, Lewis base, BronstedLowry
More informationSemester 2 Midterm Review (Bluffer s Guide) *Adapted from Paul Groves [South Pasadena HS]
Semester 2 Midterm Review (Bluffer s Guide) *Adapted from Paul Groves [South Pasadena HS] Unit 5: Kinetics How to talk about Reaction Rate rate = Δ[chemical]/Δtime - Common Units: M/s, mol L - s rate of
More information2. What is the equilibrium constant for the overall reaction?
Ch 15 and 16 Practice Problems - KEY The following problems are intended to provide you with additional practice in preparing for the exam. Questions come from the textbook, previous quizzes, previous
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) Which one of the following is the weakest acid? 1) A) HF (Ka = 6.8 10-4) B) HNO2 (Ka
More informationChemistry 122 (Tyvoll) EXAMINATION II KEY November 4, 2005
Chemistry 122 (Tyvoll) EXAMINATION II KEY November 4, 2005 Part I. Multiple Choice (3 points each -- Total points = 45) 1. The activation energy for a chemical reaction is 1. the energy produced when bonds
More informationEquilibrium and Reaction Rate
Equilibrium and Reaction Rate Multiple Choice Questions - Answers 1. Activation energy could be considered as the minimum energy required to do which of these? A. change the orientation of the reactant
More information11/15/11. Chapter 16. HA(aq) + H 2 O(l) H 3 O + (aq) + A (aq) acid base conjugate conjugate
Chapter 16 Table of Contents Chapter 16 16.1 16.2 16.3 16.4 16.5 16.6 Buffered Solutions Copyright Cengage Learning. All rights reserved 2 Models of Arrhenius: Acids produce H + ions in solution, bases
More informationCh 15 and 16 Practice Problems
Ch 15 and 16 Practice Problems The following problems are intended to provide you with additional practice in preparing for the exam. Questions come from the textbook, previous quizzes, previous exams,
More informationTime (s) [N 2 O 5 ] (mol/l)
Exercises #1: 1. The following data show the concentration of N 2 O 5 as a function of time in the following reaction: 2 N 2 O 5 (g) 4 NO 2 (g) + O 2 (g) Time (s) 0 50 100 200 300 400 [N 2 O 5 ] (mol/l)
More informationHouston Community College System General Chemistry 1412 Departmental Final Exam
Houston Community College System General Chemistry 1412 Departmental Final Exam Aspirin, C 9 H 8 O 4 - Acetylsalicylic Acid was originally derived from Salicin the active ingredient in Willow bark. drug
More information1 A. That the reaction is endothermic when proceeding in the left to right direction as written.
1 Q. If Δ r H is positive, what can you say about the reaction? 1 A. That the reaction is endothermic when proceeding in the left to right direction as written. 2 Q If Δ r H is negative, what can you say
More informationFormulas and Constants (you may remove this page)
Formulas and Constants (you may remove this page) NA = 6.0x0 3 mol - h = 6.66x0-34 J s c =.99x0 m s - e =.60x0-9 C me = 9.09x0-3 kg Å = x0-0 m = 00 pm atm = 760 torr R = 0.006 L atm K - mol - =.34 J K
More informationChapter 16. Acids and Bases. Copyright Cengage Learning. All rights reserved 1
Chapter 16 Acids and Bases Copyright Cengage Learning. All rights reserved 1 Section 16.1 Acids and Bases Models of Acids and Bases Arrhenius: Acids produce H + ions in solution, bases produce OH ions.
More informationLecture Presentation. Chapter 14. Chemical Kinetics. John D. Bookstaver St. Charles Community College Cottleville, MO Pearson Education, Inc.
Lecture Presentation Chapter 14 John D. Bookstaver St. Charles Community College Cottleville, MO In kinetics we study the rate at which a chemical process occurs. Besides information about the speed at
More informationChapter 12. Kinetics. Factors That Affect Reaction Rates. Factors That Affect Reaction Rates. Chemical. Kinetics
PowerPoint to accompany Kinetics Chapter 12 Chemical Kinetics Studies the rate at which a chemical process occurs. Besides information about the speed at which reactions occur, kinetics also sheds light
More informationChapter 14 Chemical Kinetics
Chapter 14 Chemical Kinetics Factors that Affect Reaction rates Reaction Rates Concentration and Rate The Change of Concentration with Time Temperature and Rate Reactions Mechanisms Catalysis Chemical
More information14.1 Factors That Affect Reaction Rates
14.1 Factors That Affect Reaction Rates 1) 2) 3) 4) 14.2 Reaction Rates How does increasing the partial pressures of the reactive components of a gaseous mixture affect the rate at which the compounds
More informationAcid-Base Chemistry & Organic Compounds. Chapter 2
Acid-Base Chemistry & Organic Compounds Chapter 2 Brønsted Lowry Acids & Bases! Brønsted-Lowry Acid: Proton (H + ) Donor! Brønsted-Lowry Base: Proton (H + ) Acceptor! General reaction: HA + B: A - + BH
More information(for tutoring, homework help, or help with online classes)
www.tutor-homework.com (for tutoring, homework help, or help with online classes) 1. chem10b 16.1-27 The ph of a 0.10 M solution of a weak base is 9.82. What is the K b for this base? A. 8.8 10-8 B. 2.1
More informationCHEM 1412 Practice Exam 1 - Chapters Zumdahl
CHEM 1412 Practice Exam 1 - Chapters 11 13 Zumdahl Some equations and constants: T = Km P = XP = MRT ln[a]t = kt + ln[a]o 1 / [A]t = kt + 1 / [A]o t1/2 = ln(2) / k t1/2 = 1 / k{a]o Kp = Kc(RT) n ln(k1/k2)
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 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 information1002_1st Exam_
1002_1st Exam_1010321 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Consider the following reaction: POCl3(g) POCl(g) + Cl2(g) Kc = 0.450 A sample
More informationName AP CHEM / / Chapter 12 Outline Chemical Kinetics
Name AP CHEM / / Chapter 12 Outline Chemical Kinetics The area of chemistry that deals with the rate at which reactions occur is called chemical kinetics. One of the goals of chemical kinetics is to understand
More informationDr. D. DeCoste T.A (80 pts.) 21 (30 pts.) 22 (25 pts.) 23 (25 pts.) Total (160 pts)
CHEMISTRY 202 Hour Exam III December 6, 2018 Dr. D. DeCoste Name KEY Signature T.A. This exam contains 23 questions on 13 numbered pages. Check now to make sure you have a complete exam. You have two hours
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 informationChapter 14. Chemical Kinetics
14.1 Factors that Affect Reaction Rates Chemical kinetics = the study of how fast chemical reactions occur. Factors which affect rates of reactions: Physical state of the reactants. Concentration of the
More informationChemical Equilibrium Practice Problems #2
Chemical Equilibrium Practice Problems #2 2-20-2015 1. A CPHS student does an equilibrium experiment with the general chemical equation and derives the 2 graphs below: A = B: a. When at equilibrium is
More informationChemistry 142 (Practice) MIDTERM EXAM II November. Fill in your name, section, and student number on Side 1 of the Answer Sheet.
Chemistry 4 (Practice) MIDTERM EXAM II 009 November (a) Before starting, please check to see that your exam has 5 pages, which includes the periodic table. (b) (c) Fill in your name, section, and student
More informationb. There is no net change in the composition (as long as temperature is constant).
CHAPTER THIRTEEN Questions 9. a. The rates of the forward and reverse reactions are equal at equilibrium. b. There is no net change in the composition (as long as temperature is constant). 10. False. Equilibrium
More informationCalculating Reaction Rates 1:
Calculating Reaction Rates 1: 1. A 5.0g sample of magnesium reacts complete with a hydrochloric acid solution after 150 s. Express the average rate of consumption of magnesium, in units of g/min. 2. How
More informationChapter #021. What is the poh of a M KOH solution? Student Response a. 2.1 b. 4.8 c. 9.2 d e. None of these choices is correct.
For answers, send email to: admin@tutor-homework.com. Include file name: Chemistry_Worksheet_0052 Price: $3 (c) 2012 www.tutor-homework.com: Tutoring, homework help, help with online classes. 1. 016 Chapter
More informationCHM 1046 FINAL REVIEW
CHM 1046 FINAL REVIEW Prepared & Presented By: Marian Ayoub PART II Chapter Description 14 Chemical Equilibrium 15 Acids and Bases 16 Acid-Base Equilibrium 17 Solubility and Complex-Ion Equilibrium 19
More informationLeader: Deborah Course: CHEM 178 Instructor: Bonaccorsi/Vela Date: 2/6/18 + H 2 CHF 3. a. Express the rate law in terms of m, n, and k.
EXAM I REVIEW KEY Leader: Deborah Course: CHEM 178 Instructor: Bonaccorsi/Vela Date: 2/6/18 1. Given the following reaction: CF 4 + H 2 CHF 3 + HF a. Express the rate law in terms of m, n, and k. Rate
More informationIllinois JETS Academic Challenge Chemistry Test (District) Useful Information. PV = nrt R = L atm mol -1 K -1.
Useful Information PV = nrt R = 0.08206 L atm mol -1 K -1 Q = m x T x s 1 atm = 760 torr Avogadro's number = 6.022 x 10 23 K = C + 273 ph = -log [H + ] 1 1 E = (-R H ) - n 2 n 2 f i R H = 2.18 x 10-18
More informationChapter 14. Chemical Kinetics
Chapter 14. Chemical Kinetics 14.1 Factors that Affect Reaction Rates The speed at which a chemical reaction occurs is the reaction rate. Chemical kinetics is the study of how fast chemical reactions occur.
More informationAcids and Bases Written Response
Acids and Bases Written Response January 1999 4. Consider the salt sodium oxalate, Na2C2O4. a) Write the dissociation equation for sodium oxalate. (1 mark) b) A 1.0M solution of sodium oxalate turns pink
More information2. What mass of an aqueous 22.9% sodium chloride solution contains 99.5 g of water?
CHEM 1412 MIDTERM EXAM (100 pts total) ANSWER KEY Student s Name PART A (20 multiple choice questions, 3 pts each): 1. The solubility of a gas in a liquid can always be increased by: a) decreasing the
More informationCHM 2046 Test 2 Review: Chapter 12, Chapter 13, & Chapter 14
Chapter 12: 1. In an 80.0 L home aquarium, the total pressure is 1 atm and the mole fraction of nitrogen is 0.78. Henry s law constant for N 2 in water at 25 is 6.1 x 10 4. What mass of nitrogen is dissolved
More informationAP CHEMISTRY NOTES 8-1 CHEMICAL EQUILIBRIUM: AN INTRODUCTION
AP CHEMISTRY NOTES 8-1 CHEMICAL EQUILIBRIUM: AN INTRODUCTION Chemical Equilibrium a dynamic state in which the rate of the forward reaction and the rate of the reverse reaction in a system are equal (the
More informationThe table shows three possible reversible reactions that he could use. The enthalpy changes are also shown. O(g) CO 2. (g) + 4H 2.
1 A manufacturer investigates some reactions that produce hydrogen. The table shows three possible reversible reactions that he could use. The enthalpy changes are also shown. Reaction Equation H in kj/mol
More informationthe following equilibrium constants. Label the thermodynamic and kinetic regions.
REACTION RATES 1. Distinguish between kinetic and thermodynamic regions of a reaction. 2. How does an increase in pressure affect the rate of a gas-phase reaction? What effect on the rate would doubling
More informationHow would we know if equilibrium has been reached? Or if it will be reach?
1 How would we know if equilibrium has been reached? Or if it will be reach? The reaction quotient, Q, or trial KC, enables us to determine this information. The reaction quotient is determined by using
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 informationKinetics - Chapter 14. reactions are reactions that will happen - but we can t tell how fast. - the steps by which a reaction takes place.
The study of. Kinetics - Chapter 14 reactions are reactions that will happen - but we can t tell how fast. - the steps by which a reaction takes place. Factors that Affect Rx Rates 1. The more readily
More informationChapter Test A. Chapter: Chemical Equilibrium
Assessment Chapter Test A Chapter: Chemical Equilibrium In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. A 15.0 ml volume
More informationPractice Exam 1: Answer Key
CHM 2046 Practice Exam 1: Answer Key Important: Bubble in A, B or C as the test form code at the top right of your answer sheet. Useful information is provided at the end. VERSION A 1. The reaction A(aq)
More informationName. Chem 116 Sample Examination #2
page 1 of 8 Name Last 5 digits of Student Number: XXX X Chem 116 Sample Examination #2 This exam consists of eight (8) pages, including this cover page. Be sure your copy is complete before beginning your
More informationCHEMISTRY - CLUTCH CH.13 - CHEMICAL KINETICS.
!! www.clutchprep.com CONCEPT: RATES OF CHEMICAL REACTIONS is the study of reaction rates, and tells us the change in concentrations of reactants or products over a period of time. Although a chemical
More information1) Define the following terms: a) catalyst; b) half-life; c) reaction intermediate
Problems - Chapter 19 (without solutions) 1) Define the following terms: a) catalyst; b) half-life; c) reaction intermediate 2) (19.10) Write the reaction rate expressions for the following reactions in
More informationChemical Equilibrium
Chemical Equilibrium Equilibrium Constants For a generic chemical reaction, the equilibrium constant is defined as: aa + bb cc + dd (1) The equilibrium constant, K eq, for a chemical reaction indicates
More information