[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"doc-detail-183983-en":3,"doc-seo-183983-105":30,"detail-sidebar-cat-0-en-105":90},{"code":4,"msg":5,"data":6},0,"success",{"doc_id":7,"user_id":8,"nickname":9,"user_avatar":10,"doc_module":4,"category_id":11,"category_name":12,"doc_title":13,"doc_description":14,"doc_content":15,"file_id":16,"file_url":17,"file_type":18,"file_size":19,"view_count":20,"is_deleted":4,"is_public":21,"is_downloadable":21,"audit_status":21,"page_count":11,"language":22,"language_code":23,"site_id":24,"html_lang":23,"table_of_contents":25,"faqs":26,"seo_title":27,"seo_description":14,"update_tm":28,"read_time":29},183983,687207024478,"Mia  ","https://ap-avatar.wpscdn.com/davatar_a8503ba1806abce46bf441b54a3ca4cd",4,"Exam","AP Chemistry Equations Sheet - Unit Symbols - Conversions","AP Chemistry equations sheet summarizing key relationships and constants used across multiple chemistry topics. Includes unit definitions and conversions (metric prefixes, gas laws, temperature relations), atomic structure formulas with Planck’s constant and Avogadro’s number, and core kinetic expressions for reaction rates. Also provides equilibrium constants and pH/pOH relations, thermodynamics/electrochemistry parameters, and supporting gas, solution, and stoichiometric variables to support quick problem-solving on exams.","| 57\u003Cbr>La\u003Cbr>138.91 | 58\u003Cbr>Ce\u003Cbr>140.12 | 59\u003Cbr>Pr\u003Cbr>140.91 | 60\u003Cbr>Nd\u003Cbr>144.24 | 61\u003Cbr>Pm | 62\u003Cbr>Sm\u003Cbr>150.36 | 63\u003Cbr>Eu\u003Cbr>151.97 | 64\u003Cbr>Gd\u003Cbr>157.25 | 65\u003Cbr>Tb\u003Cbr>158.93 | 66\u003Cbr>Dy\u003Cbr>162.50 | 67\u003Cbr>Ho\u003Cbr>164.93 | 68\u003Cbr>Er\u003Cbr>167.26 | 69\u003Cbr>Tm\u003Cbr>168.93 | 70\u003Cbr>Yb\u003Cbr>173.05 | 71\u003Cbr>Lu\u003Cbr>174.97 |\n| --- | --- | --- | --- | --- | --- | --- | --- | --- | --- | --- | --- | --- | --- | --- |\n| 89\u003Cbr>Ac | 90\u003Cbr>Th\u003Cbr>232.04 | 91\u003Cbr>Pa\u003Cbr>231.04 | 92\u003Cbr>U\u003Cbr>238.03 | 93\u003Cbr>Np | 94\u003Cbr>Pu | 95\u003Cbr>Am | 96\u003Cbr>Cm | 97\u003Cbr>Bk | 98\u003Cbr>Cf | 99\u003Cbr>Es | 100\u003Cbr>Fm | 101\u003Cbr>Md | 102\u003Cbr>No | 103\u003Cbr>Lr |\n\n\n| UNIT SYMBOLS |\n| --- |\n| gram, g |\n| mole, mol |\n| liter, L |\n| meter, m |\n| second, s |\n| hertz, Hz |\n| atmosphere, atm |\n| millimeter of mercury, mm Hg |\n| degree Celsius, °C |\n| kelvin, K |\n| joule, J |\n| volt, V |\n| coulomb, C |\n| ampere, A |\n\n\n| UNIT CONVERSIONS |\n| --- |\n| 1 hertz = 1 s−1 |\n| 1 atm = 760 mm Hg = 760 torr |\n| K = °C + 273.15 |\n| 1 volt =  1 joule \u003Cbr>1 coulomb |\n| 1 ampere = 11couseoom~~b~~n~~d~~ |\n\n\n| METRIC PREFIXES |  |  |\n| --- | --- | --- |\n| Factor | Prefix | Symbol |\n| 109 | giga | G |\n| 106 | mega | M |\n| 103 | kilo | k |\n| 10−2 | centi | c |\n| 10−3 | milli | m |\n| 10−6 | micro | μ |\n| 10−9 | nano | n |\n| 10−12 | pico | p |\n\n\n| ATOMIC STRUCTURE\u003Cbr>E = hc =  |  | E = energy\u003Cbr> = frequency  = wavelength F = force q = charger = separation\u003Cbr>Planck's constant, h = 6.626 × 10−34 J s Speed of light, c = 2.998 × 108 m s−1\u003Cbr>Avogadro's number = 6.022 × 1023 mol−1 |\n| --- | --- | --- |\n| Fcoulombic |  q1q2 2\u003Cbr>r |  |\n| GASES, LIQUIDS, AND SOLUTIONS\u003Cbr>P1V1   P2 V2\u003Cbr>=\u003Cbr>T1 T2\u003Cbr>PV = nRT\u003Cbr>PA = Ptotal × XA , where XA = tmotoa~~ll~~esmoA~~le~~s Ptotal = PA + PB + PC + ...\u003Cbr>n =  m\u003Cbr>M\u003Cbr>D = m\u003Cbr>V\u003Cbr>1 2\u003Cbr>KE = ~~ ~~ mv\u003Cbr>2\u003Cbr>n\u003Cbr>M =  solute \u003Cbr>L\u003Cbr>solution\u003Cbr>A = bc |  | P = pressure\u003Cbr>V = volume\u003Cbr>T = temperature n = number of moles X = mole fraction\u003Cbr>m = mass\u003Cbr>M = molar mass D = density\u003Cbr>KE = kinetic energy v = velocity\u003Cbr>M = molarity\u003Cbr>A = absorbance\u003Cbr> = molar absorptivity b = path length\u003Cbr>c = concentration Gas constant, R = 8.314 J mol−1 K−1\u003Cbr>= 0.08206 L atm mol−1 K−1 STP = 273.15 K and 1.0 atm\u003Cbr>Ideal gas at STP = 22.4 L mol−1 |\n\n\n| KINETICS\u003Cbr>[A]t − [A]0 = −kt ln[A]t − ln[A]0 = −kt\u003Cbr> 1  −  1  = kt [A]t [A]0\u003Cbr>t 1 = 0.693\u003Cbr>2 k\u003Cbr>|  |  | \u003Cbr>k = rate constant t = time\u003Cbr>t 1 = half-life 2 |\n| --- | --- | --- | --- |\n| EQUILIBRIUM\u003Cbr>Kc = [[CA]]ca[[DB]]db~~ ~~ , where a A + b B 􀁔 c C + d DK = (PC )c (PD )d\u003Cbr>p (PA )a (PB )b\u003Cbr>Kw = [H 3O+ ][OH − ] = 1.0 × 10−14 at 25°CpKw = 14 = pH + pOH at 25°C\u003Cbr>pH = − log[H 3O+ ], pOH = − log[OH − ] Ka = [H~~ ~~3A][]A~~ ~~−~~ ~~], Kb = [OH~~ ~~−[B][]HB+~~ ~~] pKa = − log Ka , pKb = − log Kb\u003Cbr>Kw = Ka × Kb , pKw = pKa + pKb\u003Cbr>pH = pKa + log ~~ ~~[[A−HA]] |  |  | Equilibrium Constants\u003Cbr>Kc (molar concentrations) Kp (gas pressures)\u003Cbr>Kw (water)\u003Cbr>Ka (acid)\u003Cbr>Kb (base) |\n| THERMODYNAMICS/ELECTROCHEMISTRY |  |  | q = heat\u003Cbr>m = mass\u003Cbr>c = specific heat capacity\u003Cbr>T = temperature S° = standard entropy H° = standard enthalpy\u003Cbr>G° = standard Gibbs free energy R = gas constant\u003Cbr>K = equilibrium constant\u003Cbr>n = number of moles of electrons E° = standard potential\u003Cbr>I = current (amperes)\u003Cbr>q = charge (coulombs) t = time (seconds)\u003Cbr>Q = reaction quotient Faraday's constant, F = 96, 485 coulombs / 1 mol e − |\n| q\u003Cbr>H 􀁆\u003Cbr>reaction\u003Cbr>S 􀁆\u003Cbr>reaction\u003Cbr>G 􀁆\u003Cbr>reaction\u003Cbr>G  | | mcT\u003Cbr>H 􀁆 ~~ ~~ H 􀁆\u003Cbr>f product f reactant\u003Cbr>S 􀁆 − S 􀁆\u003Cbr>product reactant\u003Cbr>G 􀁆 ~~ ~~ G 􀁆\u003Cbr>f product f reactant\u003Cbr>H ° − TS \u003Cbr>|  |\n| = −RTlnK\u003Cbr>= −nFE °\u003Cbr>I = qt\u003Cbr>Ecell = E􀁆cell − RTnF~~ ~~ ln Q |  |  |  |","cbCaifgV2kxAy3vd","https://ap.wps.com/l/cbCaifgV2kxAy3vd","pdf",954217,2,1,"English","en",105,"# Unit Symbols\n# Unit Conversions\n# Metric Prefixes\n# Atomic Structure\n# Gases, Liquids, and Solutions\n# Kinetics\n# Equilibrium\n# Thermodynamics/Electrochemistry","[{\"question\":\"What unit and conversion formulas are included in the AP Chemistry equations sheet?\",\"answer\":\"The sheet lists common units (g, mol, L, m, s, atm, °C, K, J, V, C, A) and conversion relations such as hertz to seconds and temperature conversion K = °C + 273.15, plus metric prefix factors.\"},{\"question\":\"Which atomic structure and constants equations are provided?\",\"answer\":\"It includes E = hc and the associated relations using Planck’s constant and the speed of light, along with Avogadro’s number for molar calculations.\"},{\"question\":\"What equilibrium and pH/pOH relationships are covered?\",\"answer\":\"The sheet provides equilibrium constant expressions (Kc, Kp, Kw, Ka, Kb) and links pH and pOH through logarithmic forms, including pKa and pKb relationships.\"}]","AP Chemistry Equations Sheet - Unit Symbols - Conversions | 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unit and conversion formulas are included in the AP Chemistry equations sheet?","Question",{"text":74,"@type":75},"The sheet lists common units (g, mol, L, m, s, atm, °C, K, J, V, C, A) and conversion relations such as hertz to seconds and temperature conversion K = °C + 273.15, plus metric prefix factors.","Answer",{"name":77,"@type":72,"acceptedAnswer":78},"Which atomic structure and constants equations are provided?",{"text":79,"@type":75},"It includes E = hc and the associated relations using Planck’s constant and the speed of light, along with Avogadro’s number for molar calculations.",{"name":81,"@type":72,"acceptedAnswer":82},"What equilibrium and pH/pOH relationships are covered?",{"text":83,"@type":75},"The sheet provides equilibrium constant expressions (Kc, Kp, Kw, Ka, Kb) and links pH and pOH through logarithmic forms, including pKa and pKb 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