[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"doc-seo-437263-105":3,"detail-sidebar-cat-0-en-105":81,"doc-detail-437263-en":131},{"code":4,"msg":5,"data":6},0,"ok",{"site_id":7,"language":8,"slug":9,"title":10,"keywords":11,"description":12,"schema_data":13,"social_meta":74,"head_meta":76,"extra_data":78,"updated_unix":80},105,"en","ap-chemistry-unit-3-practice-test-block","AP Chemistry Unit 3 Practice Test - Block","","AP Chemistry Unit 3 practice test covering gases and solutions, including ideal gas behavior, gas stoichiometry with water vapor and partial pressures, and Dalton’s law with mole fractions. Questions assess effusion and kinetic molecular theory, molar mass via effusion rates, and comparisons of gas density, molecular speed, and kinetic energy under equal conditions. Additional items analyze vapor pressure, phase diagrams, intermolecular forces, ionic hydration trends, and condensation behavior for methane versus propane.",{"@graph":14,"@context":73},[15,34,56],{"@type":16,"itemListElement":17},"BreadcrumbList",[18,23,27,31],{"item":19,"name":20,"@type":21,"position":22},"https://docshare.wps.com","Home","ListItem",1,{"item":24,"name":25,"@type":21,"position":26},"https://docshare.wps.com/document/","Document",2,{"item":28,"name":29,"@type":21,"position":30},"https://docshare.wps.com/document/exam/","Exam",3,{"item":32,"name":10,"@type":21,"position":33},"https://docshare.wps.com/document/ap-chemistry-unit-3-practice-test-block/437263/",4,{"url":32,"name":10,"@type":35,"image":36,"author":41,"headline":10,"publisher":44,"fileFormat":47,"inLanguage":8,"description":12,"dateModified":48,"datePublished":49,"encodingFormat":47,"isAccessibleForFree":50,"interactionStatistic":51},"DigitalDocument",{"url":37,"@type":38,"width":39,"height":40},"https://docshare.wps.com/thumbnails/ap-chemistry-unit-3-practice-test-block/437263.png","ImageObject",300,407,{"name":42,"@type":43},"Logic","Person",{"url":19,"name":45,"@type":46},"DocShare","Organization","application/pdf","2026-10-23","2026-09-29",true,{"@type":52,"interactionType":53,"userInteractionCount":55},"InteractionCounter",{"@type":54},"ViewAction",18,{"@type":57,"mainEntity":58},"FAQPage",[59,65,69],{"name":60,"@type":61,"acceptedAnswer":62},"What determines the partial pressure of hydrogen in the experiment described?","Question",{"text":63,"@type":64},"The partial pressure is found by subtracting the water vapor pressure from the total barometric pressure, using Dalton’s law.","Answer",{"name":66,"@type":61,"acceptedAnswer":67},"In a sealed vessel with a pinhole leak, which statements about effusion are correct?",{"text":68,"@type":64},"Correct choices depend on Graham’s law and effusion rates: lighter gases effuse faster, while temperature being constant does not make all gases effuse at the same rate.",{"name":70,"@type":61,"acceptedAnswer":71},"How do you identify the weakest intermolecular forces from the vapor pressure table?",{"text":72,"@type":64},"The liquid with the highest equilibrium vapor pressure at 20°C has the weakest intermolecular forces, since it evaporates most easily.","https://schema.org",{"og:url":32,"og:type":75,"og:title":10,"og:site_name":45,"og:description":12},"article",{"robots":77,"canonical":32},"index,follow",{"doc_id":79,"site_id":7},437263,1790905268,{"code":4,"msg":82,"data":83},"success",[84,88,92,95,100,105,110,115,120,123,127],{"id":22,"doc_module":4,"doc_module_name":25,"category_name":85,"show_sort_weight":86,"slug":87},"Story & Novel",90,"story-novel",{"id":26,"doc_module":4,"doc_module_name":25,"category_name":89,"show_sort_weight":90,"slug":91},"Literature",80,"literature",{"id":33,"doc_module":4,"doc_module_name":25,"category_name":29,"show_sort_weight":93,"slug":94},70,"exam",{"id":96,"doc_module":4,"doc_module_name":25,"category_name":97,"show_sort_weight":98,"slug":99},5,"Comic",60,"comic",{"id":101,"doc_module":4,"doc_module_name":25,"category_name":102,"show_sort_weight":103,"slug":104},6,"Technology",50,"technology",{"id":106,"doc_module":4,"doc_module_name":25,"category_name":107,"show_sort_weight":108,"slug":109},7,"Healthcare",40,"healthcare",{"id":111,"doc_module":4,"doc_module_name":25,"category_name":112,"show_sort_weight":113,"slug":114},8,"Research & Report",30,"research-report",{"id":116,"doc_module":4,"doc_module_name":25,"category_name":117,"show_sort_weight":118,"slug":119},9,"Religion & Spirituality",20,"religion-spirituality",{"id":118,"doc_module":4,"doc_module_name":25,"category_name":121,"show_sort_weight":118,"slug":122},"World Cup","world-cup",{"id":124,"doc_module":4,"doc_module_name":25,"category_name":125,"show_sort_weight":124,"slug":126},10,"Lifestyle","lifestyle",{"id":128,"doc_module":4,"doc_module_name":25,"category_name":129,"show_sort_weight":96,"slug":130},19,"General","general",{"code":4,"msg":82,"data":132},{"doc_id":79,"user_id":133,"nickname":42,"user_avatar":134,"doc_module":4,"category_id":33,"category_name":29,"doc_title":10,"doc_description":12,"doc_content":135,"file_id":136,"file_url":137,"file_type":138,"file_size":139,"view_count":55,"is_deleted":4,"is_public":22,"is_downloadable":22,"audit_status":22,"page_count":140,"language":141,"language_code":8,"site_id":7,"html_lang":8,"table_of_contents":142,"faqs":143,"seo_title":144,"seo_description":12,"update_tm":145,"read_time":146},1099513958762,"https://ap-avatar.wpscdn.com/avatar/1000023916a998db790?x-image-process=image/resize,m_fixed,w_180,h_180&k=1784791008015729253","AP Chemistry Unit 3 Practice Test Name    \nSolids, Liquids, Gases and Solutions Date   Block    \n1. A real gas would act most ideal at  \n(A) 1 atm and 273 K (D) 0.5 atm and 546 K  \n(B) 10 atm and 547 K (E) 0.5 atm and 273 K  \n(C) 10 atm and 273 K  \n2. Zinc reacts with aqueous sulfuric acid to form hydrogen gas:  \nZn (s) + H2 SO4 (aq) ¬ ZnSO4 (aq) + H2 (g)  \nIn an experiment, 201 mL ofwet H2 is collected over water at 27°C and a barometric pressure of 733 torr. The vapor pressure of water at 27°C is 26.74 torr. The partial pressure of hydrogen in this experiment is   atm.  \n(A) 0.929 (D) 1.00  \n(B) 760 (E) 0.964  \n(C) 706  \n3. A mixture of gases contains 1.5 moles of oxygen, 3.0 moles of nitrogen, and 0.5 mole of water vapor. If the total pressure is 700 mmHg, what is the partial pressure of the nitrogen gas?  \n(A) 70 mmHg (D) 350 mmHg  \n(B) 210 mmHg (E) 420 mmHg  \n(C) 280 mmHg  \n4. Equal numbers of moles of CO2(g), N2(g), and NH3(g) are placed in a sealed vessel at room temperature. If the vessel has a pinhole-size leak, which of the following will be true after some of the gas mixture has effused?  \nI. The mole fraction of CO2 in the sample will increase.  \nII. The N2 will effuse the fastest since it is the lightest.  \nIII. All gases will effuse at the same rate since the temperature is held constant.  \n(A) I only (C) I and II (E) I, II, and III  \n(B) III only (D) II and III  \n5. A sample of oxygen gas was found to effuse at a rate equal to two times that of an unknown gas. The molecular weight of the unknown gas is   g/mol.  \n(A) 128 (B) 8  \n(C) 16  \n(D) 64  \n6. Two flexible containers for gases are at the same temperature and pressure. One holds 14 gof nitrogen and the other holds 22 g of carbon dioxide. Which of the following statements about these gas samples is true?  \n(A) The volume of the carbon dioxide container is the same as the volume of the nitrogen container.  \n(B) The number of molecules in the carbon dioxide container is greater than the number of molecules in the nitrogen container.  \n(C) The density of the carbon dioxide sample is the same as that of the nitrogen sample.  \n(D) The average kinetic energy of the carbon dioxide molecules is greater than the average kinetic energy of the nitrogen molecules.  \n(E) The average speed of the carbon dioxide molecules is greater than the average speed of the nitrogen molecules.  \n7. A hydrocarbon gas with the empirical formula CH2 has a density of 1.3 g/L at 0ºC and 1.00 atm. A possible formula for the hydrocarbon is:  \n(A) CH2  \n(B) C2H4  \n(C) C3H6  \n(D) C4H8  \n(E) C5H 10  \n8. A 0.33 mole sample of CaCO3(s) is placed in a 1 L evacuated flask, which is then sealed and heated. The CaCO3(s) decomposes completely according to the balanced equation below. The total pressure in the flask, measured at 300 K is closest to which of the following?(The gas constant, R = 0.082 L atm/mol K)  \nCaCO3(s) → CaO(s) + CO2(g)  \n(A) 2.0 atm  \n(B) 4.1 atm  \n(C) 8.1 atm  \n(D) 16 atm  \n(E) 18 atm  \n9. When a sample of carbon dioxide gas in a closed container of constant volume at 0.5 atm and 200 K is heated until its temperature reaches 400 K, its new pressure is closest to  \n(A) 0.25 atm (D) 1.5 atm  \n(B) 0.50 atm (E) 2.0 atm  \n(C) 1.0 atm  \n10. The pressure of 4.0 L of an ideal gas in a flexible container is decreased to one-third of its original pressure and its absolute temperature is decreased by one-half. The volume then is  \n(A) 1.0 L  \n(B) 4.0 L  \n(C) 6.0 L  \n(D) 8.0 L  \n(E) 24 L  \n11. A given mass of a gas occupies 5.00 L at 65 °C and 480 mmHg. What is the volume of the gas at 630 mmHg and 85 °C?  \n12. A gas sample is confined in a 5-liter container. Which of the following will occur if the temperature of the container is increased?  \nI. The kinetic energy of the gas will increase.  \nII. The pressure of the gas will increase  \nIII. The density of the gas will increase.  \n(A) I only (C) I and II only (E) I, II, and III  \n(B) II only (D) I and III only  \n13.The normal boiling point of","cbCaiiOZ8nCdw1Sf","https://ap.wps.com/l/cbCaiiOZ8nCdw1Sf","pdf",413092,11,"English","# Solids, Liquids, Gases and Solutions\n## Ideal gas behavior and partial pressures\n## Effusion, kinetic theory, and molecular speed\n## Molar mass and gas laws\n## Phase diagrams, vapor pressure, and intermolecular forces\n## Ionic attractions and condensation","[{\"question\":\"What determines the partial pressure of hydrogen in the experiment described?\",\"answer\":\"The partial pressure is found by subtracting the water vapor pressure from the total barometric pressure, using Dalton’s law.\"},{\"question\":\"In a sealed vessel with a pinhole leak, which statements about effusion are correct?\",\"answer\":\"Correct choices depend on Graham’s law and effusion rates: lighter gases effuse faster, while temperature being constant does not make all gases effuse at the same rate.\"},{\"question\":\"How do you identify the weakest intermolecular forces from the vapor pressure table?\",\"answer\":\"The liquid with the highest equilibrium vapor pressure at 20°C has the weakest intermolecular forces, since it evaporates most easily.\"}]","AP Chemistry Unit 3 Practice Test - Block | PDF",1790680818,28]