[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"doc-seo-437264-105":3,"detail-sidebar-cat-0-en-105":81,"doc-detail-437264-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-gases-practice-problems-multiple-choice","AP Chemistry - Gases Practice Problems - Multiple Choice","","AP Chemistry gases practice problems covering ideal gas behavior, real-gas deviations, molecular kinetic theory, effusion, and average molecular speed. Multiple-choice questions address relationships among pressure, volume, temperature, and particle number, including density and molecular speed changes under heating and in a rigid container. Practice also includes gas stoichiometry using molar ratios at 0°C and 1 atm, partial pressures from gas mixtures, and interpreting speed-distribution curves across temperatures. Free-response prompts extend these concepts to gas mixtures, gas collection over water, and diffusion of reactants forming ammonium chloride.",{"@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-gases-practice-problems-multiple-choice/437264/",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-gases-practice-problems-multiple-choice/437264.png","ImageObject",300,407,{"name":42,"@type":43},"Jiven","Person",{"url":19,"name":45,"@type":46},"DocShare","Organization","application/pdf","2026-10-21","2026-09-29",true,{"@type":52,"interactionType":53,"userInteractionCount":55},"InteractionCounter",{"@type":54},"ViewAction",13,{"@type":57,"mainEntity":58},"FAQPage",[59,65,69],{"name":60,"@type":61,"acceptedAnswer":62},"How do pressure and density change for a gas in a rigid container when temperature is doubled?","Question",{"text":63,"@type":64},"In a constant-volume container, heating increases pressure proportionally to absolute temperature. Density also doubles because the amount of gas per fixed volume increases with temperature change under the ideal-gas relationship.","Answer",{"name":66,"@type":61,"acceptedAnswer":67},"What volume of O2 is needed to produce 4.0 L of CO2 at 0°C and 1 atm?",{"text":68,"@type":64},"Use the balanced equation CS2 + 3 O2 → CO2 + 2 SO2 so the gas-volume ratio matches the mole ratio. CO2 volume corresponds directly to moles, giving an O2 volume determined by the 3:1 stoichiometric ratio.",{"name":70,"@type":61,"acceptedAnswer":71},"How is partial pressure of a gas determined in a mixture with known total pressure?",{"text":72,"@type":64},"Compute the mole fraction of the gas from its moles divided by total moles, then multiply by the total pressure: P_gas = X_gas × P_total. This gives the partial pressure for each component in the mixture.","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},437264,1790895305,{"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},1099513958607,"https://ap-avatar.wpscdn.com/avatar/100002390cf8733938c?x-image-process=image/resize,m_fixed,w_180,h_180&k=1778829742770036399","Name:    \nAP Chemistry  \nGases Practice Problems  \nMultiple Choice  \nIdentify the letter of the choice that best completes the statement or answers the question. You  \n  1. At standard temperature and pressure, a 0.50 mol sample of H2 gas and a separate 1.0 mol sample of O2 gas have the same  \na. average molecular kinetic energy c. volume  \nb. average molecular speed d. effusion rate  \n  2. A rigid metal tank contains oxygen gas. Which of the following applies to the gas in the tank when additional oxygen is added at constant temperature?  \na. The volume of the gas increases .  \nb. The pressure of the gas decreases .  \nc. The average speed of the gas molecules remains the same .  \nd. The total number of gas molecules remains the same .  \n  3. What volume of O2(g) is required to react with excess CS2(!) to produce 4.0 L of CO2(g)? (Assume all gases are measured at 0°C and 1 atm.)  \nCS2(!) + 3 O2(g) ® CO2(g) + 2 SO2(g)  \na. 12 L c. 1/3 ´ 22.4 L  \nb. 22.4 L d. 2 ´ 22.4 L  \n4. A hydrocarbon gas with an empirical formula CH2 has a density of 1.88 grams per liter at 0oC and 1.00  \n____  \natmosphere. Which of the following is a possible molecular formula for the hydrocarbon?  \na. CH2 c. C3H6  \nb. C2H4 d. C4H8  \n  5. A 2 L container will hold about 4 g of which of the following gases at 0°C and 1 atm?  \na. SO2 c. CO2  \nb. N2 d. C4H8  \n  6. Under which conditions will a real gas behave most like an ideal gas?  \na. high pressure and high temperature c. low volume and high temperature  \nb. low pressure and low temperature d. low pressure and high temperature  \n  7. When a sample of oxygen gas in a closed container of constant volume is heated until its absolute temperature is doubled, which of the following is also doubled?  \na. The density of the gas  \nb. The pressure of the gas  \nc. The average velocity of the gas molecules  \nd. The number of molecules per cm3  \n  8. Consider the graph below, which shows the speed distribution of a sample of gas molecules at four different temperatures.  \nWhich of the following correctly sequences the curves in order of increasing temperature?  \na. A, C, B, D c. A, B, C, D  \nb. D, B, C, A d. D, C, B, A  \n  9. Equal masses of three different ideal gases, X, Y, and Z, are mixed in a sealed rigid container . If the temperature of the system remains constant, which of the following statements about the partial pressure of gas X is correct?  \na. It is equal to 1/3 the total pressure  \nb. It depends on the intermolecular forces of attraction between molecules of X, Y, and Z.  \nc. It depends on the relative molecular masses of X, Y, and Z.  \nd. It depends on the average distance traveled between molecular collisions .  \n  10. A flask contains 0.25 mole of SO2(g) , 0.50 mole of CH4(g) , and 0.50 mole of O2(g) . The total pressure of the gases in the flask is 800 mm Hg. What is the partial pressure of the SO2(g) in the flask?  \na. 800 mm Hg c. 250 mm Hg  \nb. 600 mm Hg d. 160 mm Hg  \n  11. Consider the graph below, which shows the speed distribution of three different pure substances in the gas phase at a temperature of 566 oC. Which of the following statements accurately describes the molar masses of the substances and provides the correct explanation?  \na. Substance A has the highest molar mass, because Substance A has the lowest average speed.  \nb. Substance C has the highest molar mass, because Substance C has the highest average speed.  \nc. Substance A has the lowest molar mass, because Substance A has the lowest average speed.  \nd. Substances A, B and C all have the same molar mass.  \n  12. In a laboratory experiment, H2(g) is collected over water in a gas-collection tube as shown in the diagram below.  \nThe temperature of the water is 21oC and the atmospheric pressure in the laboratory is measured to be 772 torr. Before measuring the volume of gas collected in the tube, what step, if any, must be taken to make it possible to determine the total gas pressure inside the tube?  \na. Tilt the tube to the side ","cbCaiuWWTrB2uF1m","https://ap.wps.com/l/cbCaiuWWTrB2uF1m","pdf",460761,11,"English","# Multiple Choice\n## Gas laws and ideal gas behavior\n## Stoichiometry and gas mixtures\n## Molecular speed distributions and kinetic theory\n# Free Response Questions\n## Gas mixtures in a rigid cylinder\n## Identical balloons with pure gases\n## Diffusion and reaction ring formation\n## Gas collection over water","[{\"question\":\"How do pressure and density change for a gas in a rigid container when temperature is doubled?\",\"answer\":\"In a constant-volume container, heating increases pressure proportionally to absolute temperature. Density also doubles because the amount of gas per fixed volume increases with temperature change under the ideal-gas relationship.\"},{\"question\":\"What volume of O2 is needed to produce 4.0 L of CO2 at 0°C and 1 atm?\",\"answer\":\"Use the balanced equation CS2 + 3 O2 → CO2 + 2 SO2 so the gas-volume ratio matches the mole ratio. CO2 volume corresponds directly to moles, giving an O2 volume determined by the 3:1 stoichiometric ratio.\"},{\"question\":\"How is partial pressure of a gas determined in a mixture with known total pressure?\",\"answer\":\"Compute the mole fraction of the gas from its moles divided by total moles, then multiply by the total pressure: P_gas = X_gas × P_total. This gives the partial pressure for each component in the mixture.\"}]","AP Chemistry - Gases Practice Problems - Multiple Choice | PDF",1790680818,28]