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Chemistry Practice Test - Ch. 12 - Kinetics","","A.P. Chemistry practice test covering reaction kinetics and chemical rate laws for Chapter 12, Kinetics. Multiple-choice problems address average rates of disappearance/appearance, valid units for reaction rates, concentration-time data tables, and calculation of reaction order with respect to reactants. Additional questions determine half-life and solve first- and second-order integrated rate law problems using given rate constants, including reaction-rate factor changes and graph interpretation for slopes and constants.",{"@graph":69,"@context":122},[70,84,105],{"@type":71,"itemListElement":72},"BreadcrumbList",[73,77,79,82],{"item":74,"name":75,"@type":76,"position":8},"https://docshare.wps.com","Home","ListItem",{"item":78,"name":9,"@type":76,"position":14},"https://docshare.wps.com/document/",{"item":80,"name":20,"@type":76,"position":81},"https://docshare.wps.com/document/exam/",3,{"item":83,"name":65,"@type":76,"position":19},"https://docshare.wps.com/document/ap-chemistry-practice-test-ch-12-kinetics/461473/",{"url":83,"name":65,"@type":85,"image":86,"author":91,"headline":65,"publisher":94,"fileFormat":97,"inLanguage":63,"description":67,"dateModified":98,"datePublished":99,"encodingFormat":97,"isAccessibleForFree":100,"interactionStatistic":101},"DigitalDocument",{"url":87,"@type":88,"width":89,"height":90},"https://docshare.wps.com/thumbnails/ap-chemistry-practice-test-ch-12-kinetics/461473.png","ImageObject",300,407,{"name":92,"@type":93},"Putri","Person",{"url":74,"name":95,"@type":96},"DocShare","Organization","application/pdf","2026-10-08","2026-09-30",true,{"@type":102,"interactionType":103,"userInteractionCount":34},"InteractionCounter",{"@type":104},"ViewAction",{"@type":106,"mainEntity":107},"FAQPage",[108,114,118],{"name":109,"@type":110,"acceptedAnswer":111},"How do you relate the average rate of appearance of B to the rate of disappearance of A?","Question",{"text":112,"@type":113},"Use stoichiometry from the balanced reaction. The relationship comes from comparing D[B]/Dt with the corresponding D[A]/Dt multiplied by the stoichiometric coefficients and sign changes.","Answer",{"name":115,"@type":110,"acceptedAnswer":116},"What determines the order of a reaction with respect to a reactant like B or ClO2?",{"text":117,"@type":113},"The order is inferred from how the reaction rate changes when that reactant concentration is changed while other reactants are held constant, using the rate law proportionality.",{"name":119,"@type":110,"acceptedAnswer":120},"How are first-order and second-order integrated rate laws used in these problems?",{"text":121,"@type":113},"First-order problems use ln[A] versus time (or equivalent integrated form) and half-life relations; second-order problems use 1/[A] versus time (or equivalent integrated form) to solve for time or concentration changes.","https://schema.org",{"og:url":83,"og:type":124,"og:title":65,"og:site_name":95,"og:description":67},"article",{"robots":126,"canonical":83},"index,follow",{"doc_id":128,"site_id":62},461473,1790949288,{"code":4,"msg":5,"data":131},{"doc_id":128,"user_id":132,"nickname":92,"user_avatar":133,"doc_module":4,"category_id":19,"category_name":20,"doc_title":65,"doc_description":67,"doc_content":134,"file_id":135,"file_url":136,"file_type":137,"file_size":138,"view_count":34,"is_deleted":4,"is_public":8,"is_downloadable":8,"audit_status":8,"page_count":139,"language":140,"language_code":63,"site_id":62,"html_lang":63,"table_of_contents":141,"faqs":142,"seo_title":143,"seo_description":67,"update_tm":144,"read_time":145},962085571259,"https://ap-avatar.wpscdn.com/davatar_29158cc5080c5b710cf443261637dec0","A.P. Chemistry Practice Test: Ch. 12, Kinetics  \nMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.  \n1) Consider the following reaction:  \n3A ¬ 2B  \nThe average rate of appearance of B is given by D[B]/Dt. Comparing the rate of appearance of B and the rate of disappearance of A, we get D[B]/Dt =   x (-D[A]/Dt).  \nA) -2/3 B) -3/2 C) +2/3 D) +3/2 E) +1  \n2) A burning splint will burn more vigorously in pure oxygen than in air because  \nA) nitrogen is a reactant in combustion and its low concentration in pure oxygen catalyzes the combustion.  \nB) oxygen is a reactant in combustion and the concentration of oxygen is higher in pure oxygen than it is in air.  \nC) oxygen is a product of combustion.  \nD) nitrogen is a product of combustion and the system reaches equilibrium at a lower temperature.  \nE) oxygen is a catalyst for combustion.  \n3) Of the following, all are valid units for a reaction rate except  .  \nA) mol/L B) M/s C) mol/hr D) mol/L-hr E) g/s  \nA flask is charged with 0.124 mol ofA and allowed to react to form B according to the reaction A(g) ¬B(g). The following data are obtained for [A] as the reaction proceeds:  \n\n| Time (s) | 1 | 10 | 20 | 30 | 40 |\n| --- | --- | --- | --- | --- | --- |\n| Moles of A | 0.124 | 0.110 | 0.088 | 0.073 | 0.054 |\n\n4) The average rate of disappearance of A between 10 s and 20 s is   mol/s.  \nA) 1.1 ˛ 10-3 B) 4.4 ˛ 10-3 C) 454 D) 9.90 ˛ 10-3 E) 2.2 ˛ 10-3 The peroxydisulfate ion (S 2O82- ) reacts with the iodide ion in aqueous solution via the reaction:  \nS2O82- (aq) + 3I- ¬ 2SO4(aq) + I3- (aq)  \nAn aqueous solution containing 0.050 M ofS2O82-ion and 0.072 M ofI-is prepared, and the progress of the reaction followed by measuring [I- ]. The data obtained is given in the table below.  \n\n| Time (s) | 0 | 400 | 800 | 1200 | 1600 |\n| --- | --- | --- | --- | --- | --- |\n| [I- ](M) | 0.072 | 0.057 | 0.046 | 0.037 | 0.029 |\n\n5) The concentration of S2O82-remaining at 800 s is   M.  \nA) 0.015 B) 0.041 C) 0.076 D) 4.00 ˛10-3 E) 0.046  \n6) Of the units below,   are appropriate for a first-order reaction rate constant.  \nA) L mol-1 s-1 B) s-1 C) M-1 s-1 D) mol/L E) M s-1  \n7) If the rate law for the reaction  \n2A + 3B ¬ products  \nis first order in A and second order in B, then the rate law is rate =    \nA) k[A]2[B]3 B) k[A]2[B]2 C) k[A][B] D) k[A]2[B] E) k[A][B]2  \n8) The kinetics of the reaction below were studied and it was determined that the reaction rate increased by a factor of 9 when the concentration of B was tripled. The reaction is   order in B.  \nA + B ¬ P  \nA) zero B) first C) second D) third E) one-half The data in the table below were obtained for the reaction:  \n2 ClO2(aq) + 2 OH- (aq) ¬ ClO3- (aq) + ClO2- (aq) + H2O (1)  \n\n| Experiment\u003Cbr>Number | [ClO 2](M) | [OH- ](M) | Initial Rate\u003Cbr>(M/s) |\n| --- | --- | --- | --- |\n| 1 | 0.060 | 0.030 | 0.0248 |\n| 2 | 0.020 | 0.030 | 0.00276 |\n| 3 | 0.020 | 0.090 | 0.00828 |\n\n9) What is the order of the reaction with respect to ClO2?  \nA) 4 B) 1 C) 0 D) 2  \n10) What is the order of the reaction with respect to OH-?  \nA) 0 B) 1 C) 2 D) 3  \n11) What is the overall order of the reaction?  \nA) 0 B) 1 C) 4 D) 3  \n12) What is the magnitude of the rate constant for the reaction?  \nA) 115 B) 1.15 x 104 C) 713 D) 4.6  \n13) For a first-order reaction, a plot of   versus   is linear.  \nA) ln [A]t, t B) ~~ [~~1A~~]~~t~~ ~~, t C) In [A] t, ~~ ~~1t~~ ~~ D) [A] t, t  \nE) 3  \nE) 4  \nE) 2  \nE) 230  \nE) t, ~~ [~~1A~~]~~t  \n14) The rate law for a reaction is  \nrate = k [A][B]2  \nWhich one of the following statements is false?  \nA) If [B] is doubled, the reaction rate will increase by a factor of 4.  \nB) The reaction is second order in B.  \nC) The reaction is first order in A.  \nD) k is the reaction rate constant  \nE) The reaction is second order overall.  \n15) The half-life of a first-order reaction    \nA) is constant  \nB) is the time necessary for the reactant concentration to drop to half its original value  \nC)","cbCaipopTFtH8QyC","https://ap.wps.com/l/cbCaipopTFtH8QyC","pdf",354119,15,"English","# Multiple Choice Questions\n## Reaction Rates and Units\n## Rate Laws and Reaction Order\n## Integrated Rate Laws and Half-Life\n## Interpreting Data Tables and Graphs","[{\"question\":\"How do you relate the average rate of appearance of B to the rate of disappearance of A?\",\"answer\":\"Use stoichiometry from the balanced reaction. The relationship comes from comparing D[B]/Dt with the corresponding D[A]/Dt multiplied by the stoichiometric coefficients and sign changes.\"},{\"question\":\"What determines the order of a reaction with respect to a reactant like B or ClO2?\",\"answer\":\"The order is inferred from how the reaction rate changes when that reactant concentration is changed while other reactants are held constant, using the rate law proportionality.\"},{\"question\":\"How are first-order and second-order integrated rate laws used in these problems?\",\"answer\":\"First-order problems use ln[A] versus time (or equivalent integrated form) and half-life relations; second-order problems use 1/[A] versus time (or equivalent integrated form) to solve for time or concentration changes.\"}]","A.P. Chemistry Practice Test - Ch. 12 - Kinetics | PDF",1790761689,38]