Equations and Conversions
Pressure conversions: 1 atm = 1.01325 x 105 Pa = 760 mm Hg = 760 torr
Ideal Gas Constant: R = 8.314 J K-1 mol-1 = 0.08206 L atm mol-1 K-1
Gas Laws: PV = nRT
†
P+an2
V2
Ê
Ë
Á ˆ
¯
˜ V-nb
( )
=nRT
DE = q + w q = nCDT q = nDHfus/vap
w = Fd = -PextDV
DH = DE + PDVDHo = DHfo(pdt)
-
DHfo(rct)
†
DS=qrev
T
DSo = So(pdt)
-
So(rct) aA + bB Æ cC + dD
DG = DH – TDS
†
DG= DGo+RT lnQ;Q=[C]c[D]d
[A]a[B]b=P
C
cPD
d
PA
aPB
b
DG =
-
RT ln Keq
DG =
-
nFEcell
†
Ecell =Ecell
o-RT
nF lnQ=Ecell
o-0.0592V
nlogQ
F = 96,450 C mol-1
Rate =
†
-1
a
d[A]
dt = - 1
b
d[B]
dt =1
c
d[C]
dt =1
d
d[D]
dt
aA + bB Æ cC + dD
Rate = k[A]m[B]n
Arrhenius equation:
†
k=Aexp -Ea
RT
Ê
Ë
Á ˆ
¯
˜
Integrated Rate Laws:
†
[A]= -kt +[A]ot12
=[A]o
2k
ln[A]= -kt +ln[A]ot12
=ln2
k
1
[A]=kt +1
[A]o
t12
=1
[A]ok
†
pH = -log[H3O+]pK = -logK
pH =pKa+log [A-]
[HA]
Ê
Ë
Á ˆ
¯
˜
Kw=KaKbKw=10-14
†
ax 2+bx +c=0
x=-b±b2-4ac
2a
