1.1 Notes - Reaction Kinetics
|
|
- Cathleen Hood
- 5 years ago
- Views:
Transcription
1 Chemistry 12-Unit I-Reaction Kinetics=Notes Chemistry Notes - Reaction Kinetics Reaction Kinetics is the study of rates and the factors which affect the rates. Expressing Rates rate = ~guantity of a product formed f:l time or rate = _~guantity of a reactant consumed ~time in general: rate = ~ amount (a reactant or product) ~time Note: A time unit is always in the denominator ~ '- ~i(\.) S.l hr J cl~. of a rate equation. If you have... Il Amount can be measured Units: as: Solids (s) ~mass grams (g) Gases (g) ~ volume Litres (L) ~ pressure Atmospheres (atm) ~ mass (if open container) grams (g) Aqueous ions (aq) ~ molarity ~C\Of'"1 Molarity (M) or mol/l Any species can be measured in ~ moles/ ~ time Note: We don't measure the concentrations (~ molarity) of pure liquids (ex: H 2 0) and solids since they have constant densities (basically constant concentrations). Chemistry 12-Unit l-reaction Kinetics-Notes Page 1 of 17pages
2 Chemistry J2-Unit J-Reaction Kinetics--Notes eg.) How could we measure the rate of this reaction: Z11(s)+ 2HCI(aq) ~ H2(g) + ZnCI2(aq) r = Ll mass ofzn r = Ll [HCI] (note:[] = molarconcentration) fo. ~: -t"\ s r = Ll mass of container (as H2 (g) escapes) r = Ll volume H2 Spectator Ions - some rxs, when written in ionic form show that some ions don't change concentration. Ions that appear on both sides of the arrow in equal amounts are called SPE:cTWfo C'4 ions! ego Mg(s) + 2HC~ ~ H2(g) + MgCI@ NOTE: To writean equationin IONIC FORM, dissociateall the aqueous(aq)compounds: br--:tz C4 ~ " (1 t7> ita u + "..)~, I )..-f J DrV,s,v~~:)fo:m 2 IJ ~) -+ 2~) -7 H1.. t{j) + M(j ta.j) + 2. G~) (use ion chart) *j1>j.vpt~ Oc:Ulittbll S~ ChlU~S Of rons" Write 4 possible equations which express rate for this reaction: (i) ra-\l =p 'ri\ d ~ ~.,+ ~ ~.@ ~J,L -=- A C M,9 2-~J f:j t\ V'A.e.., Is tim-<"" ~ ~te- -;:.~ 1'1\a~~ 0+ cpt\+ai nly I to~nh' ~ b t\~ l0rn-k=- ~ \JO\u.w'\{ ()~ \-h Lv\o~ ) {J h'v\i\ e, ~S#rn rak -:.. lj f~~\!((. Of Chemistry J2-Unit l-reaction Kinetics-Notes IS -ti1ml > Page Z of 17pages rt~
3 Chemistry i2-unit I-Reaction Kinetics=Notes Calculations Involving Reaction Rates When doing calculations involving rate, amount (grams, moles, Litres etc.) use the general equation: Rate = L1amount (g, mol, L) L1time (s, min) or I A amount = Rate x A time I or L1time L1amount Rate WHEN YOU USE ONE OF THESE FORMULAS, MAKE SURE YOUR UNITS CAN CANCEL OUT PROPERL Yl AL WAYS use conversion factors to cancel units you don't want and replace them with ones you do want! CO"" t\(5\ on -t-cu...-tq( for ~\'ty1~ Eg.) The rate of a reaction is mol \ m\{\ =- (OC~. mm. \ m\ ('\. or /" C, ~ \5 CoO 5 Express the rate in moll s: It. 'N ANT : \-\ A \J EX. \Gn DW CoO So /' \ \ m\ f\ ro..it. i{\~\ :=..Q.~qlYlil \ v: \ t01fs =- O ~7- \ Eg.) Solid copper dissolves in ni~ acid at a rate of2.43 gl min. How long will it take to dissolve 15.0 g of copper? '------v----" ro.k == ~ ~ h' Y'I\e, =. t 0..~O \1(\ -\ :.\_5_" _0--~L--:--- ~.'-t~ 81m'/(' f'0l ~ 0 Heljuen Questions #1-4 1!.2 c@ A'(\oW\<.-'( W ~j to S()\\l~ W ~f\ \- =- h O\'J--t X 6t;""{= \ S.Dj 'f. \ {'<\ \ (\, ~,L-\ ~ l' ~ \i~e...~ -\~-.-\1--m-\-(\-'\ L- Page 3
4 Chemistry I2-Unit Reaction Rate Calculations: I-Reaction Kinetics=Notes When Conversions Are Needed You also must use molar mass to go grams!:+ moles. m\)\a{ ma~s (at-bml'g ('0a6 s ) Co. (\ be- usul Q -S a." CD (\ V-[if&' \00 -ft.< c-ti>(. Eg) The rate of reaction of zinc metal is given below. Express the rate in units of grams/second: 0.26 mol Zri rmn? g ofzn s W a(\\-- c, h 0..\J.( " \<..V\~ 't-le. n-(.u:l. tt> GOn-J~(1- mc\ ~ 3 An~ 0'(\ '""~ ~()\\ulv\: m;{\~ 5 (b) SCO (\-I~Vs.iOf> tll(,~{s 3_ == o.26 rp~s '/-.tc5.~!3 ~ \~ (Q \ f"\\)\ 2(\ :==. ~5. 1.\ ~ os f<\yf \Mt\ ' w "" 100 s, \ - O,2'03Q --- O,:L~9;5 -- V \ When you have GASES at STP, you can use this conversion to convert from mol ~ L: Q2.4 LI m~'-.. eg.) ~l 02/S = ~ 1/s (at STP) W~ \.eec\ to LonV(l("-\- f'f\\')\ ~ L Solution: W o.n-\- c- n t>. \II( ~ KnoW..h :: o.o~o ~ i..? d\ LtL S s - - \1=06\. NOTE: This conversion is only used for gases at STP! f'(\ \() -= factor ~\ \m, (..... \ f'f"o \_ " ~J,l~ L :::.O.b1-L -O fai-l - s ~\)s ~~.4- L <; ~~.l\ L- \'3\ \ mo \ Try this problem: The rate of a reaction is g ofmg per second. Calculate the number of moles ofmg used up in 6;0 ~tes. <D R (So\- ~' {\~ 4h.e.rnk \ (\ mo 1:. fa-\-.::. 0 I ()~L.\ ~ mi{\ 1\Atl(\" ~Q. lcln -\)1\0. 'N\O~.s ~ 8 '\ll to'(\\h r-\- 3..."t'C\ 0 \ ( \Zo..\e. i- +\UV'I.{-=.. II0'1I)UI'lt-) \ ty\~\ ~..9=- ~L\.~.9 -(0 (j.:) '(\~.t(+- S ~ rn\('\ \ \"0 ( (\ -::::: bo S 'N OS\ \- ~ n C\\j (. '" '" now m~\ ::: tj b34 4c{ t...\ m~\ 'f.. 6n % '20 o. tl '3~q 5 fy1{.)l '{1\\ '" 7i ~L\.~6 \'fy\ \' n m \() ~o\ts 0 ~ t-a~9=- O.0'88QG rn~ 'f.. b -0 r<'(o ::. (), f)t) rno es
5 -Io ChCh"se -from D(l~ Chemistry I2-Unit I-Reaction Kinetics--Notes SP-lLI-eJ to a ()O+h-ef).,/ W-i lyiu6~ C;(b&~ -\-4t-<.- Comparing rates using balanced equations (Crossing the Mole Bridge) mo\ e. b\f\' ~, eg.) ethane 2C2H C02 + 6H20 lco\~a -\- Coef\ iu{~~: -- ~:- t:: 4- : ~ if ethane is consumed at a rate of mol Is, calculate the rate of consumption of 02 in molls mc\c. '\C\.-\io Ot- e-",qi\(., : O~ \ ~ CO,","t(\ mo\ et~a4\..q~ m\)\ 02- ~ : =t- Solution: 'ND.n1- =- no.'j )(. KV\t>\U (j:,y-n.er-s,ic'j\f\ t-ctc-\-o(si. "I~ ~m()\-e.+hthvl tnt!' 09. ::: Q. 066 mo~o.~l '" J rot)\ 02- t-mo\ 0 L - =-ro, ~ '0 mo\ OL.1 ""+ (,(\0\ 02: L:----;t~-~s~ 2.m()\ e\ hla ~ ethane 2C2H C02 + 6H20 '~'. 1-', L+' 6 rcn:\ ~ S ~m~~ if ethane is consumed at a rate of mol /s calculate rate of production ~V Solution: p\ 0."', [n,<,\l-t'c-\- m'd\ e~ha(lq ~ rf\0\ GO.L ' mo\.e.. 'fa. \i o 0 ~ e \-'n a (\G :. CO?. ;l. : L\- ~L~&:: '-- mo \ e-\-hfanl ~ 4-- mo\ tal L\- Me>\ (,02- ~ roo \ e+nla o.l. Page 5
6 Chemistry I2-Unit I-Reaction Kinetics--Notes When other units used - you must covert first to moles (to go over the "mole" bridge) (you may go from L -7 L of one gas to another at STP) Example: 2Al(s) + 3Br2(g) -7 2AlBr3(aq) \'\\C\e f C\-\-\ os '. ~ : B! ~ if 67.5 g of At are consumed per second - calculate the rate of consumption flji\!. "-~1.5~A\ Solution: Cc)~\l~I(s.\on --..,,-- of Br2 in g/s, "-- ~ Must go over the mole bridge! Wa,(\1-- (llk tj... 8('2-?\~'f\ -,s -m L()\\\I-O-\-. 3 A \ -4 :3."Sf 2- \ (Y\\.\s-\ ~ I:> -ho\'c\ -3 A \.~ mi)l A\ ~ ~Cl\ &; Br,. FCtG-\o'C~-7 <D \ M~\ A \ :::. J-:) o 9 '.). \no\ A \ = '3 m"\ t,(l ~ \ ('(\D \ ~(2 = \5'\ '"'39 You may have to use a few conversions and the "rate equation" to arrive at an answer. As you did in Chern. 11, make a "plan" first and make sure your units all cancel the correct way! ~OJ\-\... ""0.\1<. 'f.. \<"I\()W (-h\\q\p W l!oj')-doworksheet1.1 <D 2- CD J Be2... :. tot!;" ~.1-,~ 'j..?\'ot>~_ 'j.. \ s S ~t.\)~:1 r\i~ \ ty\\)~l - S Page 6
176 5 t h Fl oo r. 337 P o ly me r Ma te ri al s
A g la di ou s F. L. 462 E l ec tr on ic D ev el op me nt A i ng er A.W.S. 371 C. A. M. A l ex an de r 236 A d mi ni st ra ti on R. H. (M rs ) A n dr ew s P. V. 326 O p ti ca l Tr an sm is si on A p ps
More informationAPPH 4200 Physics of Fluids
APPH 42 Physics of Fluids Problem Solving and Vorticity (Ch. 5) 1.!! Quick Review 2.! Vorticity 3.! Kelvin s Theorem 4.! Examples 1 How to solve fluid problems? (Like those in textbook) Ç"Tt=l I $T1P#(
More informationChemistry 185 Exam #2 - A November 5, Lab Day and Time: Instructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More informationInstructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More information~,. :'lr. H ~ j. l' ", ...,~l. 0 '" ~ bl '!; 1'1. :<! f'~.., I,," r: t,... r':l G. t r,. 1'1 [<, ."" f'" 1n. t.1 ~- n I'>' 1:1 , I. <1 ~'..
,, 'l t (.) :;,/.I I n ri' ' r l ' rt ( n :' (I : d! n t, :?rj I),.. fl.),. f!..,,., til, ID f-i... j I. 't' r' t II!:t () (l r El,, (fl lj J4 ([) f., () :. -,,.,.I :i l:'!, :I J.A.. t,.. p, - ' I I I
More informationLast 4 Digits of USC ID:
Chemistry 05 B Practice Exam Dr. Jessica Parr First Letter of last Name PLEASE PRINT YOUR NAME IN BLOCK LETTERS Name: Last 4 Digits of USC ID: Lab TA s Name: Question Points Score Grader 8 2 4 3 9 4 0
More informationChemistry 2 Exam Roane State Academic Festival. Name (print neatly) School
Name (print neatly) School There are fifteen question on this exam. Each question is weighted equally. n the answer sheet, write your name in the space provided and your answers in the blanks provided.
More informationUnit 4 ~ Learning Guide Name:
Unit 4 ~ Learning Guide Name: Instructions: Using a pencil, complete the following notes as you work through the related lessons. Show ALL work as is eplained in the lessons. You are required to have this
More informationLab Day and Time: Instructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More informationSolutions and Ions. Pure Substances
Class #4 Solutions and Ions CHEM 107 L.S. Brown Texas A&M University Pure Substances Pure substance: described completely by a single chemical formula Fixed composition 1 Mixtures Combination of 2 or more
More informationAdvanced Placement. Chemistry. Integrated Rates
Advanced Placement Chemistry Integrated Rates 204 47.90 9.22 78.49 (26) 50.94 92.9 80.95 (262) 52.00 93.94 83.85 (263) 54.938 (98) 86.2 (262) 55.85 0. 90.2 (265) 58.93 02.9 92.2 (266) H Li Na K Rb Cs Fr
More informationPDF created with pdffactory trial version A) mol Answer: moles FeS 2 8 mol SO 2 /4 mol FeS 2 = mol SO 2.
Part A. [2 points each] For each question, circle the letter of the one correct answer and enter the answer on the TEST SCORING SHEET in pencil only. The TEST SCORING ANSWER SHEET will be considered final.
More informationP a g e 5 1 of R e p o r t P B 4 / 0 9
P a g e 5 1 of R e p o r t P B 4 / 0 9 J A R T a l s o c o n c l u d e d t h a t a l t h o u g h t h e i n t e n t o f N e l s o n s r e h a b i l i t a t i o n p l a n i s t o e n h a n c e c o n n e
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 informationLab Day and Time: Instructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More informationCHEM 107 (Spring-2004) Exam 2 (100 pts)
CHEM 107 (Spring-2004) Exam 2 (100 pts) Name: ------------------------------------------------------------------------, SSN -------------------------------- LAST NAME, First (Circle the alphabet segment
More information(C) Pavel Sedach and Prep101 1
(C) Pavel Sedach and Prep101 1 (C) Pavel Sedach and Prep101 1 (C) Pavel Sedach and Prep101 2 (C) Pavel Sedach and Prep101 2 (C) Pavel Sedach and Prep101 3 (C) Pavel Sedach and Prep101 3 (C) Pavel Sedach
More informationPOLYTECHNIC OF NAMIBIA
POLYTECHNIC OF NAMIBIA DEPARTMENT OF HEALTH SCIENCES BACHELOR OF ENVIRONMENTAL HEALTH SCIENCES HEALTH SCIENCE CHEMISTRY (HSC 511S) NQF level 5 SECOND OPPORTUNITY EXAMINATION November 2014 TIME: MARKS:
More informationINSTRUCTIONS: Exam III. November 10, 1999 Lab Section
CHEM 1215 Exam III John III. Gelder November 10, 1999 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 7 different pages. The last page includes a periodic table and
More informationFuture Self-Guides. E,.?, :0-..-.,0 Q., 5...q ',D5', 4,] 1-}., d-'.4.., _. ZoltAn Dbrnyei Introduction. u u rt 5,4) ,-,4, a. a aci,, u 4.
te SelfGi ZltAn Dbnyei Intdtin ; ) Q) 4 t? ) t _ 4 73 y S _ E _ p p 4 t t 4) 1_ ::_ J 1 `i () L VI O I4 " " 1 D 4 L e Q) 1 k) QJ 7 j ZS _Le t 1 ej!2 i1 L 77 7 G (4) 4 6 t (1 ;7 bb F) t f; n (i M Q) 7S
More information8. Relax and do well.
CHEM 1215 Exam III John III. Gelder November 11, 1998 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 7 different pages. The last page includes a periodic table and
More informationChapter 3: Stoichiometry
Chapter 3: Stoichiometry Chem 6A Michael J. Sailor, UC San Diego 1 Announcements: Thursday (Sep 29) quiz: Bring student ID or we cannot accept your quiz! No notes, no calculators Covers chapters 1 and
More information8. Relax and do well.
CHEM 1225 Exam III John III. Gelder April 8, 1999 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 7 different pages. The last two pages includes a periodic table and
More information(tnaiaun uaejna) o il?smitfl?^ni7wwuiinuvitgviisyiititvi2a-a a imaviitjivi5a^ qw^ww^i fiaa!i-j?s'u'uil?g'ijimqwuwiijami.wti. a nmj 1,965,333.
0 fltu77jjiimviu«7mi^ gi^"ijhm?'ijjw?flfi^ V m 1 /14 il?mitfl?^i7wwuiinuvitgviiyiititvi2- imviitvi^ qw^ww^i fi!i-j?'u'uil?g'iqwuwiijmi.wti twwrlf^ imii2^
More information30 Zn(s) 45 Rh. Pd(s) Ag(s) Cd(s) In(s) Sn(s) white. 77 Ir. Pt(s) Au. Hg(l) Tl. 109 Mt. 111 Uuu. 112 Uub. 110 Uun. 65 Tb. 62 Sm. 64 Gd. 63 Eu.
Enthalpy changes: experimentally it is much easier to measure heat flow at const pressure - this is enthalpy q p = )H : also nearly all chemical reactions are done at constant pressure. Enthalpy (heat)
More informationi;\-'i frz q > R>? >tr E*+ [S I z> N g> F 'x sa :r> >,9 T F >= = = I Y E H H>tr iir- g-i I * s I!,i --' - = a trx - H tnz rqx o >.F g< s Ire tr () -s
5 C /? >9 T > ; '. ; J ' ' J. \ ;\' \.> ). L; c\ u ( (J ) \ 1 ) : C ) (... >\ > 9 e!) T C). '1!\ /_ \ '\ ' > 9 C > 9.' \( T Z > 9 > 5 P + 9 9 ) :> : + (. \ z : ) z cf C : u 9 ( :!z! Z c (! $ f 1 :.1 f.
More informationINSTRUCTIONS: CHEM Exam I. September 13, 1994 Lab Section
CHEM 1314.05 Exam I John I. Gelder September 13, 1994 Name TA's Name Lab Section Please sign your name below to give permission to post, by the last 4 digits of your student I.D. number, your course scores
More information02/05/09 Last 4 Digits of USC ID: Dr. Jessica Parr
Chemistry 05 B First Letter of PLEASE PRINT YOUR NAME IN BLOCK LETTERS Exam last Name Name: 02/05/09 Last 4 Digits of USC ID: Dr. Jessica Parr Lab TA s Name: Question Points Score Grader 2 2 9 3 9 4 2
More informationA L A BA M A L A W R E V IE W
A L A BA M A L A W R E V IE W Volume 52 Fall 2000 Number 1 B E F O R E D I S A B I L I T Y C I V I L R I G HT S : C I V I L W A R P E N S I O N S A N D TH E P O L I T I C S O F D I S A B I L I T Y I N
More information8. Relax and do well.
CHEM 15 Exam II John II. Gelder March 4, 1999 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 7 different pages. The last two pages includes a periodic table, a solubility
More informationChemistry Standard level Paper 1
Chemistry Standard level Paper 1 Thursday 12 May 2016 (morning) 45 minutes Instructions to candidates Do not open this examination paper until instructed to do so. Answer all the questions. For each question,
More informationTRU Chemistry Contest Chemistry 12 May 21, 2003 Time: 90 minutes
TRU Chemistry Contest Chemistry 12 May 21, 2003 Time: 90 minutes Last Name First name School Teacher Please follow the instructions below. We will send your teacher a report on your performance. Top performers
More informationCHEM 171 EXAMINATION 1. October 9, Dr. Kimberly M. Broekemeier. NAME: Key
CHEM 171 EXAMINATION 1 October 9, 008 Dr. Kimberly M. Broekemeier NAME: Key I A II A III B IV B V B VI B VII B VIII I B II B III A IV A V A VI A VII A inert gase s 1 H 1.008 Li.941 11 Na.98 19 K 9.10 7
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 5. Chemistry for Changing Times, Chemical Accounting. Lecture Outlines. John Singer, Jackson Community College. Thirteenth Edition
Chemistry for Changing Times, Thirteenth Edition Lecture Outlines Chemical Accounting John Singer, Jackson Community College Chemical Sentences: Equations Chemical equations represent the sentences in
More informationB. Characteristics of Gases assume volume and shape of container very compressible mix evenly and completely lower density than liquids and solids
Chapter 5: Gases Laws for gases are simpler than for liquids and solids. The behavior of gases is predictable. 5.1 Substances that exist as gases Air - 78 % N2; 21 % O2; 1 % other (including CO2 which
More informationCHEM 167 FINAL EXAM MONDAY, MAY 2 9:45 11:45 A.M GILMAN HALL
PROF. JOHN VERKADE SPRING 2005 THIS EXAM CONSISTS OF 12 QUESTIONS ON 9 PAGES CHEM 167 HOUR EXAM IV APRIL 20, 2005 SEAT NO. NAME RECIT. INSTR. RECIT. SECT. GRADING PAGE Page 2 Page 3 Page 4 Page 5 Page
More informationSpring 2012 CHEM Test 4, Form A. Part 1. Multiple Choice: Clearly indicate the best answer on the scantron form.
Spring 2012 CHEM 1110.20784 Test 4, Form A Part 1. Multiple Choice: Clearly indicate the best answer on the scantron form. (60 pts) 1. A sample of a trapped ideal gas has its volume doubled while its temperature
More informationLab Day and Time: Instructions. 1. Do not open the exam until you are told to start.
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More informationOCR A GCSE Chemistry. Topic 3: Chemical reactions. Introducing chemical reactions. Notes.
OCR A GCSE Chemistry Topic 3: Chemical reactions Introducing chemical reactions Notes C3.1a use chemical symbols to write the formulae of elements and simple covalent and ionic compounds For simple ionic
More informationExhibit 2-9/30/15 Invoice Filing Page 1841 of Page 3660 Docket No
xhibit 2-9/3/15 Invie Filing Pge 1841 f Pge 366 Dket. 44498 F u v 7? u ' 1 L ffi s xs L. s 91 S'.e q ; t w W yn S. s t = p '1 F? 5! 4 ` p V -', {} f6 3 j v > ; gl. li -. " F LL tfi = g us J 3 y 4 @" V)
More informationStoichiometry. Mole Concept. Balancing Chemical Equations
Stoichiometry The story so far The structure of an atom protons, neutrons & electrons Electron structure & the Periodic Table Shapes of electron orbitals (Quantum Numbers) Essential and toxic elements
More informationOH BOY! Story. N a r r a t iv e a n d o bj e c t s th ea t e r Fo r a l l a g e s, fr o m th e a ge of 9
OH BOY! O h Boy!, was or igin a lly cr eat ed in F r en ch an d was a m a jor s u cc ess on t h e Fr en ch st a ge f or young au di enc es. It h a s b een s een by ap pr ox i ma t ely 175,000 sp ect at
More informationLab Day and Time: Instructions. 1. Do not open the exam until you are told to start. Page # Points possible Points awarded
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More information8. Relax and do well.
CHEM 1314.03 Exam II John II. Gelder October 23, 1997 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 9 different pages. The last four pages include a periodic table,
More information8. Relax and do well.
CHEM 1515 Exam II John II. Gelder October 14, 1993 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 8 different pages. The last two pages include a periodic table, a
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 informationChemistry B11 Chapter 5 Chemical reactions
Chapter 5 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 A + BC AC +
More informationBROOKLYN COLLEGE Department of Chemistry. Chemistry 1 Second Lecture Exam Nov. 27, Name Page 1 of 5
BROOKLYN COLLEGE Department of Chemistry Chemistry 1 Second Lecture Exam Nov. 27, 2002 Name Page 1 of 5 Circle the name of your lab instructor Kobrak, Zhou, Girotto, Hussey, Du Before you begin the exam,
More informationActivity Introduction to Stoichiometry
Activity 151-9 Introduction to toichiometry Directions: This Guided Learning Activity (GLA) focuses on completing stoichiometric calculations. Part A discusses the relationships that allow us to convert
More informationPart 2. Multiple choice (use answer card). 90 pts. total. 3 pts. each.
1 Exam I CHEM 1303.001 Name (print legibly) Seat no. On my honor, I have neither given nor received unauthorized aid on this exam. Signed Date Part 1. Nomenclature. 10 pts. total. 2 pts. each. Fill in
More informationChemistry 11 Course Review
Introduction to Chemistry 1. 0.0006 mm =? µm Chemistry 11 Course Review 6. A 0.0460 L piece of copper has a mass of 410.32 g. Calculate the density of copper in g/ml. 2. 0.054 ml =? nl 3. 3.5 µg/l =? mg/ml
More informationFaculty of Natural and Agricultural Sciences Chemistry Department. Semester Test 1. Analytical Chemistry CMY 283. Time: 120 min Marks: 100 Pages: 6
Faculty of Natural and Agricultural Sciences Chemistry Department Semester Test 1 Analytical Chemistry CMY 283 Date: 5 September 2016 Lecturers : Prof P Forbes, Dr Laurens, Mr SA Nsibande Time: 120 min
More informationChemistry 11: General Chemistry 1 Final Examination. Winter 2006
Chemistry 11: General Chemistry 1 Final Examination Winter 2006 Answers are given at the end of the exam. Name 1 Part 1 1. A 0.600 g pure sample of elemental iron (Fe) is dissolved in H 2 SO 4 (aq) to
More informationChem October 31, Dr. Susan E. Bates
Chem 1711 Exam 2 ID#: 2013171 October 31, 2013 Dr. Susan E. Bates Name 9:00 OR 10:00 PV = nrt 1 atm = 760 mmhg = 101.3 kpa u = (3RT/M m ) 1/2 R = 0.08206 L atm K 1 mol 1 OR 8.314 J K 1 mol 1 22.4 L/mol
More informationCHE 105 EXAMINATION II October 13, 2011
CHE 105 EXAMINATION II October 13, 2011 University of Kentucky Department of Chemistry READ THESE DIRECTIONS CAREFULLY BEFORE STARTING THE EXAMINATION! It is extremely important that you fill in the answer
More informationFaculty of Natural and Agricultural Sciences Chemistry Department. Semester Test 1 MEMO. Analytical Chemistry CMY 283
Faculty of Natural and Agricultural Sciences Chemistry Department Semester Test 1 MEMO Analytical Chemistry CMY 283 Date: 5 September 2016 Lecturers : Prof P Forbes, Dr Laurens, Mr SA Nsibande Time: 90
More informationHow do you measure matter?
How do you measure matter? You may count how many you have. Determine a substances mass and weight. Determine a substances volume. But how can you relate these three types of measurements to one another?
More informationChapter 3. Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions In this chapter, Chemical structure and formulas in studying the mass relationships of atoms and molecules. To explain the composition of compounds and
More informationName (Print) Section # or TA. 1. You may use a crib sheet which you prepared in your own handwriting. This may be
Name (Print) Section # or TA 1. You may use a crib sheet which you prepared in your own handwriting. This may be one 8-1/2 by 11 inch sheet of paper with handwriting only on one side. 2. You may use a
More informationCHEMISTRY 101 SPRING 2010 FINAL FORM B DR. KEENEY-KENNICUTT PART 1
NAME (Please print ) CHEMISTRY 101 SPRING 2010 FINAL FORM B DR. KEENEY-KENNICUTT Directions: (1) Put your name on PART 1 and your name and signature on PART 2 of the exam where indicated. (2) Sign the
More informationIf anything confuses you or is not clear, raise your hand and ask!
CHM 1045 Dr. Light s Section December 10, 2002 FINAL EXAM Name (please print) Recitation Section Meeting Time This exam consists of six pages. Make sure you have one of each. Print your name at the top
More information8. Relax and do well.
CHEM 1314.03 Exam I John I. Gelder September 25, 1997 Name TA's Name Lab Section Please sign your name below to give permission to post, by the last 4 digits of your student I.D. number, your course scores
More informationK. 27 Co. 28 Ni. 29 Cu Rb. 46 Pd. 45 Rh. 47 Ag Cs Ir. 78 Pt.
1 IA 1 ydrogen 1.01 Atomic number Element symbol Element name Atomic mass VIIIA 1 1.01 IIA IIIA IVA VA VIA VIIA 2 e 4.00 Metalloids 3 Li 6.94 4 Be 9.01 5 B 10.81 6 C 12.01 7 N 14.01 8 O 16.00 9 F 19.00
More information7. Relax and do well.
CHEM 1215 Exam II John II. Gelder October 13, 1999 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 5 different pages. The last page includes a periodic table and a solubility
More informationH STO RY OF TH E SA NT
O RY OF E N G L R R VER ritten for the entennial of th e Foundin g of t lair oun t y on ay 8 82 Y EEL N E JEN K RP O N! R ENJ F ] jun E 3 1 92! Ph in t ed b y h e t l a i r R ep u b l i c a n O 4 1922
More informationPhysical Chemistry I CHEM 4641 Final Exam 13 questions, 30 points
Physical Chemistry I CHEM 4641 Final Exam 13 questions, 30 points Name: KEY Gas constant: R = 8.314 J mol -1 K -1 = 0.008314 kj mol -1 K -1. Boltzmann constant k = 1.381 10-23 J/K = 0.6950 cm -1 /K h =
More informationLe Chatelier's Principle. 2. How changes in each factor affect equilibrium (Le Chatelier's Principle)
Chern 12 Notes 11.4 - Le Chatelier's Principle Goals are to learn: 1. The factors that can cause changes in a system at equilibrium 2. How changes in each factor affect equilibrium (Le Chatelier's Principle)
More informationChemistry 31A Autumn 2004 Professors Chidsey & Zare Exam 4 Name: 9:00am 10:00am 2:15pm 3:15pm 7:00pm 8:00pm S02 OC103 Charles
Chemistry 31A Autumn 2004 Professors Chidsey & Zare Exam 4 Name: SUNetID: @stanford.edu Honor Code Observed: (Signature) 9:00am 10:00am 2:15pm 3:15pm 7:00pm 8:00pm S02 OC103 Charles S04 OC103 Charles S06
More informationM14/4/CHEMI/SPM/ENG/TZ1/XX CHEMISTRY. Monday 19 May 2014 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES
M14/4/CEMI/SPM/ENG/TZ1/XX 22146110 CEMISTRY standard level Paper 1 Monday 19 May 2014 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES Do not open this examination paper until instructed to do so. Answer
More informationQuantitative chemistry Atomic structure Periodicity
IB chemistry Units 1-3 review Quantitative chemistry Significant figures The mole- be able to convert to number of particles and mass Finding empirical and molecular formulas from mass percentage States
More informationSolutions CHAPTER OUTLINE
Chapter 8A Solutions 1 CHAPTER OUTLINE Type of Solutions Electrolytes & Nonelectrolytes Equivalents of Electrolytes Solubility & Saturation Soluble & Insoluble Salts Formation of a Solid Precipitation
More informationPERIODIC TABLE OF THE ELEMENTS
Useful Constants and equations: K = o C + 273 Avogadro's number = 6.022 x 10 23 d = density = mass/volume R H = 2.178 x 10-18 J c = E = h = hc/ h = 6.626 x 10-34 J s c = 2.998 x 10 8 m/s E n = -R H Z 2
More informationDURATION: 2 HOUR 45 MINUTES
1 Exam 9 Our country, our future 525/1 S6 CHEMISTRY PAPER 1 DURATION: 2 HOUR 45 MINUTES For Marking guide contact and consultations: Dr. Bbosa Science 0776 802709. Answer all question in part I and six
More informationHANDOUT SET GENERAL CHEMISTRY II
HANDOUT SET GENERAL CHEMISTRY II Periodic Table of the Elements 1 2 3 4 5 6 7 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 IA VIIIA 1 2 H He 1.00794 IIA IIIA IVA VA VIA VIIA 4.00262 3 Li 6.941 11 Na 22.9898
More informationCircle the letters only. NO ANSWERS in the Columns!
Chemistry 1304.001 Name (please print) Exam 5 (100 points) April 18, 2018 On my honor, I have neither given nor received unauthorized aid on this exam. Signed Date Circle the letters only. NO ANSWERS in
More informationOur country, our future 525/1 S6 CHEMISTRY PAPER 1 DURATION: 2 HOUR 45 MINUTES
1 Our country, our future 525/1 S6 CHEMISTRY Exam 10 PAPER 1 DURATION: 2 HOUR 45 MINUTES For Marking guide contact and consultations: Dr. Bbosa Science 0776 802709, Instructions - This paper consists of
More informationM09/4/CHEMI/SPM/ENG/TZ1/XX+ CHEMISTRY. Monday 18 May 2009 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES
M09/4/CHEMI/SPM/ENG/TZ1/XX+ 22096110 CHEMISTRY standard level Paper 1 Monday 18 May 2009 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES Do not open this examination paper until instructed to do so.
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 informationINTRO AND BACKGROUND: Reactions, Moles, Stoichiometry, and Solutions. Chemical Reaction Atoms are REARRANGED to form a different substance
INTRO AND BACKGROUND: Reactions, Moles, Stoichiometry, and Solutions Chemical Reaction Atoms are REARRANGED to form a different substance Changes the way atoms are joined together Atoms CANNOT be created
More informationChemistry 431 Practice Final Exam Fall Hours
Chemistry 431 Practice Final Exam Fall 2018 3 Hours R =8.3144 J mol 1 K 1 R=.0821 L atm mol 1 K 1 R=.08314 L bar mol 1 K 1 k=1.381 10 23 J molecule 1 K 1 h=6.626 10 34 Js N A = 6.022 10 23 molecules mol
More informationChemistry 1 Second Lecture Exam Fall Abbasi Khajo Kruft Levine Mathias Mathias/Ortiz Metlitsky Rahi Sanchez-Delgado Vasserman
Page 1 of 9 Chemistry 1 Second Lecture Exam Fall 2011 Name Circle the name of your recitation/lab instructor(s) Abbasi Khajo Kruft Levine Mathias Mathias/Ortiz Metlitsky Rahi Sanchez-Delgado Vasserman
More informationMarks for each question are as indicated in [] brackets.
Name Student Number CHEMISTRY 140 FINAL EXAM December 10, 2002 Numerical answers must be given with appropriate units and significant figures. Please place all answers in the space provided for the question.
More information(please print) (1) (18) H IIA IIIA IVA VA VIA VIIA He (2) (13) (14) (15) (16) (17)
CHEM 10113, Quiz 3 September 28, 2011 Name (please print) All equations must be balanced and show phases for full credit. Significant figures count, show charges as appropriate, and please box your answers!
More information2. In each of the following pairs of reactions, which would have the faster reaction rate?
CHEMISTRY 12 REACTION RATES WORKSHEET 1. The following data were collected for the reaction: Zn (s) + 2HCl (aq) H 2(g) + ZnCl 2(aq) in which zinc metal was reacted with 0.200 M HCl (aq) : Time (seconds)
More informationM11/4/CHEMI/SPM/ENG/TZ2/XX CHEMISTRY STANDARD LEVEL PAPER 1. Monday 9 May 2011 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES
M11/4/CHEMI/SPM/ENG/TZ/XX 116116 CHEMISTRY STANDARD LEVEL PAPER 1 Monday 9 May 011 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES Do not open this examination paper until instructed to do so. Answer
More informationINTRODUCTION TO SOLUBILITY UNIT 3A SOLUBILITY THEORY. There are three classes of compounds which can form ionic solutions:
INTRODUCTION TO SOLUBILITY There are three classes of compounds which can form ionic solutions: Acids: HCl, H 2 SO 4, HNO 3 Bases: NaOH, KOH, NH 3 Chemistry 12 UNIT 3A SOLUBILITY THEORY Salts: NaCl, KMnO
More information8. Relax and do well.
CHEM 1225 Exam I John I. Gelder February 4, 1999 Name KEY TA's Name Lab Section Please sign your name below to give permission to post your course scores on homework, laboratories and exams. If you do
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 informationChem 51, Spring 2015 Exam 8 (Chp 8) Use your Scantron to answer Questions There is only one answer for each Question. Questions are 2 pt each.
Chem 51, Spring 2015 Exam 8 (Chp 8) Name 120 pt Use your Scantron to answer Questions 1-32. There is only one answer for each Question. Questions are 2 pt each. CHP 8.1 Solutions are Mixtures 1. A saturated
More information3. Which of the following elements is primarily responsible for the photochemical smog? Chemistry 12, Exam III, Form A, April 4, 2001
Chemistry 12, Exam III, Form A, April 4, 2001 In all questions involving gases, assume that the ideal-gas laws hold, unless the question specifically refers to the non-ideal behavior. 1. It takes 21.3
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 information4. What is the number of unpaired electrons in Ni? Chemistry 12 Final Exam Form A May 4, 2001
Chemistry 12 Final Exam Form A May 4, 2001 In all questions involving gases, assume that the ideal-gas laws hold, unless the question specifically refers to the non-ideal behavior. 1. Which of the following
More informationConservation The Law of Conservation of Matter states that matter cannot be created or destroyed in ordinary chemical reactions. This means that no
Chemical Reactions Conservation The Law of Conservation of Matter states that matter cannot be created or destroyed in ordinary chemical reactions. This means that no atoms can be lost or gained. This
More informationOregon State University, Summer 2009 Chemistry 121 Midterm Exam 2, July 3rd, 10 am
Oregon State University, Summer 2009 Chemistry 121 Midterm Exam 2, July 3rd, 10 am DO NOT OPEN THIS EXAM UNTIL INSTRUCTED. CALCULATORS ARE NOT TO BE SHARED. Instructions : You should have with you several
More informationHomework #3 Chapter 11 Electrochemistry
Homework #3 Chapter 11 Electrochemistry Chapter 4 83. a) Oxidation ½ Reaction Fe + HCl HFeCl 4 Fe + 4HCl HFeCl 4 Fe + 4HCl HFeCl 4 + 3H + Fe + 4HCl HFeCl 4 + 3H + + 3e Reduction ½ Reaction H 2 2H + H 2
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 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 information7. Relax and do well.
CHEM 1215 Exam II John II. Gelder October 7, 1998 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 5 different pages. The last page includes a periodic table and a solubility
More informationCHEMICAL COMPOUNDS MOLECULAR COMPOUNDS
48 CHEMICAL COMPOUNDS - Dalton's theory does not mention this, but there is more than one way for atoms to come together to make chemical compounds! - There are TWO common kinds of chemical compound, classified
More information