[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"detail-sidebar-cat-0-en-105":3,"doc-seo-314914-105":59,"doc-detail-314914-en":131},{"code":4,"msg":5,"data":6},0,"success",[7,13,18,23,28,33,38,43,48,51,55],{"id":8,"doc_module":4,"doc_module_name":9,"category_name":10,"show_sort_weight":11,"slug":12},1,"Document","Story & Novel",90,"story-novel",{"id":14,"doc_module":4,"doc_module_name":9,"category_name":15,"show_sort_weight":16,"slug":17},2,"Literature",80,"literature",{"id":19,"doc_module":4,"doc_module_name":9,"category_name":20,"show_sort_weight":21,"slug":22},4,"Exam",70,"exam",{"id":24,"doc_module":4,"doc_module_name":9,"category_name":25,"show_sort_weight":26,"slug":27},5,"Comic",60,"comic",{"id":29,"doc_module":4,"doc_module_name":9,"category_name":30,"show_sort_weight":31,"slug":32},6,"Technology",50,"technology",{"id":34,"doc_module":4,"doc_module_name":9,"category_name":35,"show_sort_weight":36,"slug":37},7,"Healthcare",40,"healthcare",{"id":39,"doc_module":4,"doc_module_name":9,"category_name":40,"show_sort_weight":41,"slug":42},8,"Research & Report",30,"research-report",{"id":44,"doc_module":4,"doc_module_name":9,"category_name":45,"show_sort_weight":46,"slug":47},9,"Religion & Spirituality",20,"religion-spirituality",{"id":46,"doc_module":4,"doc_module_name":9,"category_name":49,"show_sort_weight":46,"slug":50},"World Cup","world-cup",{"id":52,"doc_module":4,"doc_module_name":9,"category_name":53,"show_sort_weight":52,"slug":54},10,"Lifestyle","lifestyle",{"id":56,"doc_module":4,"doc_module_name":9,"category_name":57,"show_sort_weight":24,"slug":58},19,"General","general",{"code":4,"msg":60,"data":61},"ok",{"site_id":62,"language":63,"slug":64,"title":65,"keywords":66,"description":67,"schema_data":68,"social_meta":124,"head_meta":126,"extra_data":128,"updated_unix":130},105,"en","ap-chemistry-chapter-5-practice-problems","AP Chemistry - Chapter 5 - Practice Problems","","AP Chemistry Chapter 5 multiple-choice practice problems focus on thermochemistry and related calculations. Questions cover heats of combustion and standard enthalpies using thermochemical equations, Hess’s law style combination of reactions, and heats of vaporization. Additional items address standard heat of formation from experimental data, combustion enthalpy for hydrocarbons, and calorimetry for neutralization and specific heat capacity of a metal using temperature changes and q = mcΔT.",{"@graph":69,"@context":123},[70,84,106],{"@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-chapter-5-practice-problems/314914/",{"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-chapter-5-practice-problems/314914.png","ImageObject",300,407,{"name":92,"@type":93},"McGucket","Person",{"url":74,"name":95,"@type":96},"DocShare","Organization","application/pdf","2026-11-06","2026-09-20",true,{"@type":102,"interactionType":103,"userInteractionCount":105},"InteractionCounter",{"@type":104},"ViewAction",38,{"@type":107,"mainEntity":108},"FAQPage",[109,115,119],{"name":110,"@type":111,"acceptedAnswer":112},"How do you determine the heat of combustion for propane from given reaction enthalpies?","Question",{"text":113,"@type":114},"Use the balanced combustion reaction for C3H8 and express its enthalpy in terms of x, y, and z. Match coefficients by rewriting the target reaction using the provided equations, then select the correct algebraic expression.","Answer",{"name":116,"@type":111,"acceptedAnswer":117},"What is the approach for finding a reaction’s standard enthalpy change from thermochemical equations?",{"text":118,"@type":114},"Combine the provided thermochemical equations to reach the target reaction, adjusting for stoichiometric coefficients. Add the enthalpy changes accordingly to obtain ΔH for the desired reaction.",{"name":120,"@type":111,"acceptedAnswer":121},"In calorimetry problems using q = mcΔT, what measurements are required to calculate q?",{"text":122,"@type":114},"You need the mass (or equivalent for the combined solution), the specific heat capacity, and the temperature change ΔT between initial and final temperatures. With these, compute q directly from q = mcΔT.","https://schema.org",{"og:url":83,"og:type":125,"og:title":65,"og:site_name":95,"og:description":67},"article",{"robots":127,"canonical":83},"index,follow",{"doc_id":129,"site_id":62},314914,1789902141,{"code":4,"msg":5,"data":132},{"doc_id":129,"user_id":133,"nickname":92,"user_avatar":134,"doc_module":4,"category_id":19,"category_name":20,"doc_title":65,"doc_description":67,"doc_content":135,"file_id":136,"file_url":137,"file_type":138,"file_size":139,"view_count":105,"is_deleted":4,"is_public":8,"is_downloadable":8,"audit_status":8,"page_count":39,"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":130,"read_time":46,"preview_page_count":4},1236954412713,"https://us-avatar.wpscdn.com/davatar_29158cc5080c5b710cf443261637dec0","Name:    \nAP Chemistry  \nChapter 5 Practice Problems  \nMultiple Choice  \nIdentify the letter of the choice that best completes the statement or answers the question. Since these are “legacy” AP Chem questions, you may use your calculator for these MC!  \n  1. Consider the following information.  \n\n| Reaction | Enthalpy of reaction |\n| --- | --- |\n| 3C(s) + 4 H2(g) ® C3H8(g) | x |\n| C(s) + O2(g) ® CO2(g) | y |\n| H2(g) + 􀀡 O2(g) ® H2O(!) | z |\n\nBased on the information above, which expression gives the heat of combustion, ∆􀀢$\\#$%& , for propane, C3H8? C3H8 (g) + 5 O2(g) ® 3 CO2(g) + 4 H2O(!)  \na. x- (y + z) d. x- (3y + 4z)  \nb. (y + z) + x e. (3y + 4z) -x  \nc. x + (3y + 4z)  \n  2. Determine ∆􀀢$'() for the following reaction,  \nN2(g) + 3 H2(g) ® 2 NH3(g)  \ngiven the thermochemical equations below.  \nN2(g) + O2(g) ® 2 NO(g) DH= +180.8 kJ  \n4 NH3(g) + 5 O2(g) ® 4 NO(g) + 6 H2O(g) DH= -906.2 kJ  \n2 H2(g) + O2(g) ® 2 H2O(g) DH= -483.6 kJ  \na. -1209.0 kJ c. -756.5 kJ  \nb. -1189.0 kJ d. -91.5 kJ  \n3.  \n____  \n3 C2H2(g) ® C6H6(g)  \nWhat is the standard enthalpy change, ∆􀀢$'() , for the reaction represented above?  \n∆􀀢$*of C2H2(g) is 230 kJ mol-1 ; ∆􀀢$* of C6H6(g) is 83 kJ mol-1 .)  \na. -607 kJ c. -19 kJ  \nb. -147 kJ d. + 19 kJ  \nCH4(g) + 2 O2(g) ® CO2(g) + 2 H2O(!) ∆􀀢$'() = –889.1 kJ  \nDHf H2O(l) = –285.8 kJ/mol  \nDHf CO2(g) = –393.3 kJ/mol  \n 4.What is the standard heat of formation of methane, CH4(g) , as calculated from the data above?  \na. –210.0 kJ/mole c. –75.8 kJ/mole  \nb. –107.5 kJ/mole d. 75.8 kJ/mole   5. Calculate ∆􀀢$'() for the combustion of gaseous ethanol,  \nC2H5OH(g) + 3 O2(g) ® 2 CO2(g) + 3 H2O(g)  \nusing standard molar enthalpies of formation.  \nmolecule ∆􀀢$* (kJ/mol)  \nC2H5OH(g) -235.3  \nCO2(g) -393.5  \nH2O(g) -241.8  \na. -1747.7 kJ c. -793.5 kJ  \nb. -1277.1 kJ d. -400.0 kJ  \n  6. When 27.0 g of an unknown metal at 88.4 °C is placed in 115 g H2O at 21.0 °C, the final temperature of the water is 23.7 °C. What is the specific heat capacity of the metal? The specific heat capacity of water is 4.184 J/g·K.  \na. 0.34 J/g·K c. 0.74 J/g·K  \nb. 0.51 J/g·K d. 0.94 J/g·K  \n7. The thermochemical equation for the combustion of hexane is shown below.  \n____  \nC6H 14(g) + +-, O2(g) ® 6 CO2(g) + 7 H2O(g) ∆􀀢$'() = -4163 kJ  \nWhat is the enthalpy change for the combustion of 2.50 g C6H 14?  \na. -121 kJ c. -1.04 ´ 104 kJ  \nb. -1.66 ´ 103 kJ d. -1.43 ´ 105 kJ  \n  8. Which of the following chemical equations corresponds to the standard molar enthalpy of formation of N2O?  \na. NO(g) + 1/2 N2(g) ® N2O(g)  \nb. N2(g) + 1/2 O2(g) ® N2O(g)  \nc. 2N(g) + O(g) ® N2O(g)  \nd. N2(g) + O(g) ® N2O(g)  \n  9. The heat of vaporization of benzene, C6H6, is 30.8 kJ/mol at its boiling point of 80.1 °C. How much heat is required to vaporize 128 g benzene at its boiling point?  \na. 4.04 kJ c. 19.3 kJ  \nb. 18.8 kJ d. 50.5 kJ  \nProblem  \n10. 2002 D  \nH+(aq) + OH- (aq) ® H2O(! l)  \nA student is asked to determine the molar enthalpy of neutralization, DHneut , for the reaction represented above. The student combines equal volumes of 1.0 M HCl and 1.0 M NaOH in an open polystyrene cup calorimeter. The heat released by the reaction is determined by using the equation q = mcDT.  \nAssume the following.  \n• Both solutions are at the same temperature before they are combined.  \n• The densities of all the solutions are the same as that of water .  \n• Any heat lost to the calorimeter or to the air is negligible .  \n• The specific heat capacity of the combined solutions is the same as that of water .  \n(a) Give appropriate units for each of the terms in the equation q = mcDT. (2 pts)  \n(b) List the measurements that must be made in order to obtain the value of q. (2 pts)  \n(c) Explain how to calculate each of the following.  \n(i) The number of moles of water formed during the experiment (1 pt)  \n(ii) The value of the molar enthalpy of neutralization, DHneut , for the reaction between HCl(aq) and NaOH(aq) (2 pts)  \n(d) The student repeats the experiment with the same equal v","cbCaii7ffPA0DMkr","https://ap.wps.com/l/cbCaii7ffPA0DMkr","pdf",194878,"English","# Multiple Choice\n## Combustion and heat of formation\n## Thermochemical equations and Hess’s law\n## Vaporization and enthalpy changes\n## Calorimetry and q = mcΔT","[{\"question\":\"How do you determine the heat of combustion for propane from given reaction enthalpies?\",\"answer\":\"Use the balanced combustion reaction for C3H8 and express its enthalpy in terms of x, y, and z. Match coefficients by rewriting the target reaction using the provided equations, then select the correct algebraic expression.\"},{\"question\":\"What is the approach for finding a reaction’s standard enthalpy change from thermochemical equations?\",\"answer\":\"Combine the provided thermochemical equations to reach the target reaction, adjusting for stoichiometric coefficients. Add the enthalpy changes accordingly to obtain ΔH for the desired reaction.\"},{\"question\":\"In calorimetry problems using q = mcΔT, what measurements are required to calculate q?\",\"answer\":\"You need the mass (or equivalent for the combined solution), the specific heat capacity, and the temperature change ΔT between initial and final temperatures. With these, compute q directly from q = mcΔT.\"}]","AP Chemistry - Chapter 5 - Practice Problems | PDF"]