[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"detail-sidebar-cat-0-en-105":3,"doc-seo-331700-105":59,"doc-detail-331700-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","general-chemistry-ii-equation-sheet","General Chemistry II - Equation Sheet","","This comprehensive equation sheet for General Chemistry II serves as an essential reference for students studying key chemical principles. It provides a structured collection of formulas covering phase changes, colligative properties, electrochemistry, thermodynamics, concentration calculations, acid-base equilibria, and chemical kinetics. The document acts as a concise study aid for solving complex chemistry problems by organizing fundamental relations such as the Nernst equation, Gibbs free energy, pH/pOH relationships, and reaction rate laws, making it a valuable resource for exam preparation and academic 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Vance","Person",{"url":74,"name":95,"@type":96},"DocShare","Organization","application/pdf","2026-11-08","2026-09-21",true,{"@type":102,"interactionType":103,"userInteractionCount":105},"InteractionCounter",{"@type":104},"ViewAction",13,{"@type":107,"mainEntity":108},"FAQPage",[109,115,119],{"name":110,"@type":111,"acceptedAnswer":112},"What formula is used to calculate the change in boiling point?","Question",{"text":113,"@type":114},"The change in boiling point is calculated using the formula ΔTb = iKbm, where i is the van 't Hoff factor, Kb is the molal boiling-point elevation constant, and m is the molality of the solution.","Answer",{"name":116,"@type":111,"acceptedAnswer":117},"How is Gibbs free energy related to the equilibrium constant?",{"text":118,"@type":114},"The relationship between Gibbs free energy and the equilibrium constant is defined by the equation ΔG° = -RT ln(K), which allows for the determination of spontaneity in chemical reactions at equilibrium.",{"name":120,"@type":111,"acceptedAnswer":121},"Which equation describes the effect of temperature on the rate constant?",{"text":122,"@type":114},"The Arrhenius equation, k = Ae^(-Ea/RT), describes how the rate constant k changes with temperature T, where Ea is the activation energy and A is the frequency factor.","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},331700,1790233897,{"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":14,"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":24,"preview_page_count":4},549768064622,"https://ap-avatar.wpscdn.com/davatar_6f874abed73319feea01a86fa6f0fab8","General Chemistry II Equation Sheet  \nThink about how to set up the problem 􀀌rst, then apply the needed principles and formulas.  \nPhase Changes  \n􀀁Tb = iKbm  \n􀀁Tf = iKfm  \n􀀙 = iMRT c = kP~~c 1~~p~~ ~~1 = ~~c~~p~~2~~2  \nPsolution = solventPolvent  \n􀀁P = Polvent 􀀀 Psolution = solute Polvent  \nCells  \nE = E 􀀎 􀀀 RTnF ln(Q)  \nE = E 􀀎 􀀀 ~~0:05~~n~~92~~ log(Q) (at 25􀀎 C)  \n􀀁G = 􀀀nFE cell  \n􀀁G􀀎 = 􀀀nFEell Eell = RTnF ln(K)  \nEell = ~~0:059~~n~~2~~V log(K) (at 25􀀎 C)  \nUSE ONE:  \nEell = Eathode (red:) 􀀀 Enode (red:)  \nEell = Eathode (red:) + Enode (ox:)  \nThermodynamics  \n􀀁G = 􀀁H 􀀀 T 􀀁S  \n􀀁Ssurr = 􀀀􀀁HTsys  \n􀀁Suniv = 􀀁Ssys + 􀀁Ssurr  \n􀀁Sxn = 􀀆Sroducts + 􀀆Seactants  \n􀀁Gxn = 􀀆􀀁Groducts + 􀀆􀀁Geactants  \nConcentrations  \nmolality = m~~m~~as~~o~~s~~les solu~~solvent~~t~~(~~e~~kg)  \n% by mass = masss~~m~~ol~~ol~~ute~~so~~m~~lu~~a~~te~~sssolvent 􀀂 100% parts per million = masss~~m~~ol~~ol~~ute~~so~~m~~lu~~a~~te~~sssolvent 􀀂 106  \nparts per billion = masss~~m~~ol~~ol~~ute~~so~~m~~lu~~a~~te~~sssolvent 􀀂 109  \nAcids and Bases  \nKw = [H3 O+ ][OH 􀀀 ] = Ka 􀀂 Kb pOH = 􀀀 log[OH 􀀀 ]  \n[OH 􀀀 ] = 10 􀀀pOH  \npH + pOH = pKa + pKb = 14:00 (at 25􀀎 C) pH = pKa + log [[AH]]  \npOH = pKb + log [B[HB]+~~ ~~]% ionization [H[3OHA+]0]eq 􀀂 100% pKa = 􀀀 log(Ka)  \npKb = 􀀀 log(Kb) Ka = 10 􀀀pKa  \nKb = 10 􀀀pKb  \nEquilibria  \nQc = [[CA]]ca[[DB]]db Kc = [[CA]]ca[[DB]]db Qp = PPdDaA􀀁􀀁PPcCbB Kp = PPdDaA􀀁􀀁PPcCbB  \nKp = Kc[R 􀀂 T ]􀀁n  \n􀀁G = 􀀁G􀀎 + RT ln(Q)  \n􀀁G􀀎 = 􀀀RT ln(K) rate = k[A]x [B]y k = Ae 􀀀 ER~~a~~T  \nln( ~~k 1~~k~~ ~~2 ) = ER~~a~~ ( ~~1~~T2 􀀀 ~~1~~T1 )  \nhalf life = lnk(2) (1st order reactions only)  \n[A]t = 􀀀kt + [A]o ln([A]t) = 􀀀kt + ln([A]o)[~~1~~A]t = kt + [~~1~~A]o  \nBurdge, J., & Overby, J. (2018) . Chemistry: Atoms First. McGraw-Hill Education.","cbCaikBl92fRNXIg","https://ap.wps.com/l/cbCaikBl92fRNXIg","pdf",199395,"English","# Phase Changes\n# Cells\n# Thermodynamics\n# Concentrations\n# Acids and Bases\n# Equilibria","[{\"question\":\"What formula is used to calculate the change in boiling point?\",\"answer\":\"The change in boiling point is calculated using the formula ΔTb = iKbm, where i is the van 't Hoff factor, Kb is the molal boiling-point elevation constant, and m is the molality of the solution.\"},{\"question\":\"How is Gibbs free energy related to the equilibrium constant?\",\"answer\":\"The relationship between Gibbs free energy and the equilibrium constant is defined by the equation ΔG° = -RT ln(K), which allows for the determination of spontaneity in chemical reactions at equilibrium.\"},{\"question\":\"Which equation describes the effect of temperature on the rate constant?\",\"answer\":\"The Arrhenius equation, k = Ae^(-Ea/RT), describes how the rate constant k changes with temperature T, where Ea is the activation energy and A is the frequency factor.\"}]","General Chemistry II - Equation Sheet | PDF",1789994767]