Chemistry 2 Flashcards
SA/WB or SB/WA equivalence point
[titrant] = [analyte]
heat capacity
amount of energy (Joules or Calories) a system must absorb to give a unit change in temperature<div><br></br></div><div>C = q /<a><span>ΔT</span></a></div>
specific heat capacity
energy absorption for an individual substance<div><br></br></div><div>q = mc<a><span>ΔT</span></a></div>
specific heat of water
<a><span>= 1 cal/g°C<br></br>= 4.18 J/g°C</span></a>
coffee cup calorimeter
solve using q = mc<a><span>ΔT</span></a><div><a><span><br></br></span></a></div><div><a><span>allows for PV work</span></a></div>
bomb calorimeter
solve using q = C<a><span>ΔT</span></a><div><a><span><br></br></span></a></div><div><a><span>gives change in internal energy</span></a></div>
first law of thermodynamics
energy can neither be created nor destroyed<div><br></br></div><div><a><span>ΔE = q + w</span></a><br></br></div>
second law of thermodynamics
heat cannot be changed completely into work via cyclical process<div><br></br></div><div>entropy in an isolated system can never decrease</div>
third law of thermodynamics
pure crystalline substances at absolute zero have an entropy of zero
zeroth law of thermodynamics
thermal equilibrium
kinetic energy / temperature
KE = 3/2 kB T
enthalpy
energy contained within chemical bonds
gibbs free energy
amount of free/useful energy available to do work
thermodynamic relation
ΔG = ΔH - TΔS
free energy / equilibrim
<a><span>ΔG<a><span>°</span></a><a><span>= -RTlnKeq</span></a><br></br></span></a><div><a><span><br></br></span></a></div><div><a><span>Keq = e^(-</span></a><a><span>ΔG/RT)</span></a></div>
