# Chem II Final Exam

 .remove_background_ad { border: 1px solid #555555; padding: .75em; margin: .75em; background-color: #e7e7e7; } .rmbg_image { max-height: 80px; } The energy of motion? A.  Kinetic B.  Potential A.  Kinetic Stored energy? A.  Kinetic B.  Potential B.  Potential Energy cannot be created or destroyed; it can only be converted from one form into another. B.   1st Law of Thermodynamics ΔE=Efinal - Einitial A.  Change in Time B.  Change in Rate C.  Change in Energy C.  Change in Energy Energy leaving the system. A.  Efinal > Einitial B.  Efinal < Einitial B. Efinal < Einitial Energy entering the system. A.  Efinal > Einitial B.  Efinal < Einitial A.  Efinal > Einitial A function or property whose value depends only on the present state, or condition, of the system, not on the path used to arrive at that state. State function F x d Work PV work formula. w= -PΔV Enthalpy equation. ΔH=ΔE+PΔV ΔH equals_____. A.  Products - Reactants B.  Reactants - Products A.  Products - Reactants Internal energy formula. ΔE=q-PΔV Heat is represented by. B.   q Energy is represented by. D.   E The amount of heat required to raise the temperature of a certain object or amount by a certain temperature. Heat capacity Heat capacity is represented by. B.   C Heat capacity formula. C=q/ΔT Specific heat formula. q=C*m or mols*ΔT The overall enthalpy change for a reaction is equal to the sum of the enthalpy changes for the individual steps. Hess's law For bond dissociation ΔH=______. A.  Products - Reactants B.  Reactants - Products B.  Reactants - Products Spontaneous process happens when___ B.   ΔH is - and ΔS is + Nonspontaneous process happens when___ B.   ΔH is + and ΔS is - Free energy change formula. ΔG=ΔH-TΔS When ΔG is < 0 then the process is______. C.   spontaneous When ΔG is = 0 then the process is______. B.   at equilibrium When ΔG is > 0 then the process is______. C.   nonspontaneous When a process proceeds on its own without and external influence. Spontaneous process Entropy change for a reaction is ΔS=_________. A.  products - reactants B.  reactants - products A.  products - reactants Entropy change formula for ideal gas. ΔS°=nRln(Vfinal/Vinitial) or Pinitial/Pfinal In any process, spontaneous or nonspontaneous, the total energy of a system and its surroundings is constant. A.   1st Law of thermodynamics In an spontaneous process, the total entropy of a system and its surroundings always increases. B.   2nd Law of thermodynamics The entropy of a perfectly ordered crystalline substance at 0 K is zero. B.   3rd Law of thermodynamics Formula for entropy change in the surroundings for a reaction. ΔSsurroundings=-ΔH/T Formula for relationship between ΔG and K. ΔG=-RTlnK Formula for free energy change under nonstandard conditions. ΔG=ΔG°+RTlnQ Formula for standard free energy of a reaction. ΔG°ΔG°products-ΔG°reactants Rate Law. Rate=Δ[A]/Δt or k[A]m[B]n Rate equals k A.   zeroth order Rate equals k[A] D.   first order Rate equals k[A][B] B.   second order Rate equals k[A][B]2 A.   third order Formula for half life of a first order reaction. t1/2=0.693/k Equilibrium equation. Kc=([C]c[D]d)/([A]a[B]b Mole of solute divided by liters of solution. Molarity Equilibrium equation is______. B.   products over reactants Gas constant R equals____. C.   0.08206 A substance that can transfer H+. Bronsted-Lowry Acid A substance that can accept H+. Bronsted-Lowry Base H2O conjugate acid is? H3O+ HA conjugate base is? A- NH3 conjugate acid is. NH4+ H2O conjugate base is. OH- Chemical species who formulas differs only by one proton are called. conjugate acid-base pairs .remove_background_ad { border: 1px solid #555555; padding: .75em; margin: .75em; background-color: #e7e7e7; } .rmbg_image { max-height: 80px; } Authorbradolder ID346632 Card SetChem II Final Exam DescriptionGen Chem II final review cards. Updated2019-04-19T01:17:07Z Show Answers