CH1810 - Practice Exam #3 - Answers
Name: ____________________________________________ Score: __________________________
Part I (~4 points each)
Multiple Choice - Choose the best answer and place the letter corresponding to the answer in the space provided AND on the Scantron form.
_____ 1. Identify the type of solid for gold.
A) metallic atomic solid B) ionic solid C) nonbonding atomic solid D) molecular solid E) network atomic solid _____ 2. Identify the type of solid for argon.
A) metallic atomic solid B) ionic solid C) nonbonding atomic solid D) molecular solid E) network atomic solid
_____ 3. Give the coordination number for a body-centered cubic cell.
A) 0 B) 6 C) 8 D) 10 E) 12
_____ 4. Name the following: [Pt(H2O)4F2]Br2
A) tetraaquadifluoroplatinum(IV) bromide B) tetraaquadibromodifluoroplatinate C) platinum(II)bromide D) platinum(III)tetraaquadifluorobromide E) platinum (II) dibromodifluorotetrahydride
_____ 5. Choose the chemical formula for diaquadicarbonylzinc tetrabromopalladate (IV).
A) [PdZn(H2O)2(CO)2]Br4 B) [Zn(H2O)2(CO)2]2[PdBr4] C) [Pd(H2O)2][Zn(CO)2]Br4 D) [Pd(H2O)2]2[Zn(CO)2]3Br4 E) [Zn(H2O)2(CO)2][PdBr4]
A
C
C
A
E
_____ 6. For the following balanced equation, determine the rate of reaction with respect to [H2]. N2(g) + 3 H2(g) → 2 NH3(g) A) Rate = + B) Rate = -
C) Rate = + D) Rate = -
_____ 7. Give the characteristic of a first order reaction having only one reactant.
A) The rate of the reaction is not proportional to the concentration of the reactant. B) The rate of the reaction is proportional to the square of the concentration of the reactant. C) The rate of the reaction is proportional to the square root of the concentration of the reactant. D) The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. E) The rate of the reaction is directly proportional to the concentration of the reactant
_____ 8. What is the overall order of the following reaction, given the rate law?
X + 2 Y → 4 Z Rate = k[X][Y] A) 3rd order B) 5th order C) 2nd order D) 1st order E) 6th order
_____ 9. What are the units of k in the following rate law? Rate = k[X][Y]1/2
A) M/s B) M-1s-1 C) M1/2s-1 D) M-1/2s-1
E) M-1s-1/2 _____ 10. Which of the following statements is FALSE?
A) The half life of a zero order reaction is dependent on concentration. B) The half life of a second order reaction is not dependent on concentration. C) The rate of second order reactions is dependent on concentration. D) The rate of a first order reaction is dependent on concentraion. E) None of the statements are FALSE.
E
Δ[H2]Δt
31
Δ[H2]Δt
31
Δ[H2]Δt
13
Δ[H2]Δt
13
C
D
D
B
_____ 11. The half life for the decay of radium is 1620 years. What is the rate constant for this first-order process?
A) 4.28 × 10-4 yr-1 B) 1.12 × 10-4 yr-1 C) 2.33 × 10-4 y-1 D) 8.91 × 10-4 y-1 E) 6.17 × 10-4 yr-1
_____ 12. Identify an heterogeneous catalyst.
A) CFCs with ozone B) solid Pd in H2 gas C) KI dissolved in H2O2 D) H2SO4 with concentrated HCl E) H3PO4 with an alcohol
_____ 13. Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled? Rate = k [X][Y]2
A) The rate of reaction will increase by a factor of 2. B) The rate of reaction will increase by a factor of 4. C) The rate of reaction will increase by a factor of 5. D) The rate of reaction will decrease by a factor of 2. E) The rate of reaction will remain unchanged.
_____ 14. How many half-lives are required for the concentration of reactant to decrease to 12.5% of its original value?
A) 3 B) 2 C) 2.5 D) 2.75 E) 8
_____ 15. The combustion of ethylene proceeds by the reaction
C2H4(g) + 3O2 (g) → 2CO2 (g) + 2H2O(g)
When the rate of disappearance of O2 is 0.28 M s-1, the rate of appearance of CO2 is ________ M s-1.
A) 0.19 B) 0.093 C) 0.84 D) 0.42 E) 0.56
A
B
B
A
A
_____ 16. Determine the identity of the daughter nuclide from the alpha decay of Rn. A) Po B) Ra C) Th D) Rn E) At
_____ 17. Determine the identity of the daughter nuclide from the electron capture by Fe. A) Co B) Mn C) Co D) Mn
E) Cr
______ 18. The following reaction represents what nuclear process?
Pb → e + Bi
A) beta emission B) positron emission C) gamma emission D) electron capture
______ 19. Which of the following nuclides is most likely to decay via positron emission?
A) Cs-137 B) I-131 C) Al-24 D) K-42 E) N-14
A 222 86
218 84
226 88
224 90
223 86
221 85
B 55 26
55 27
55 25
56 27
54 25
51 24
A137 82
0 -1
137 83
C
Part II (~8 points each) - Show all of your calculations for full credit.
_____ 1. Aluminum crystallizes in a face centered cubic structure with an edge length of 2√2 r. The atomic radius of aluminum is 143 pm. What is the density of aluminum
_____ 2. What is the equilibrium concentration of Co2+ in s solution that is initially 0.090 M Co(NO3)2 and 0.700 M OH- after the following equilibria is established:
Co2+(aq) + 4 (OH)- (aq) ⇄ Co(OH)42- Kf = 5.0 x 109
_____ 3. Determine the rate law and the value of k for the following reaction using the data provided. S2O82⁻(aq) + 3 I⁻(aq) → 2 SO42⁻(g) + I3⁻(aq) [S2O82⁻]i (M) [I⁻]i (M) Initial Rate (M-1s-1) 0.30 0.42 4.54 0.44 0.42 6.65 0.44 0.21 3.33
Answer: 1.3 x 10-9 M
Answer: 2.71 g/cm3
Answer: Rate = 36 M-1s-1 [S2O82-][I-]
_____ 4. The first-order decomposition of N2O at 1000 K has a rate constant of 0.76 s-1. If the initial concentration of N2O is 10.9 M, what is the concentration of N2O after 9.6 s?
_____ 5. The first-order rearrangement of CH3NC is measured to have a rate constant of 3.61 x 10-15 s-1 at 298 K and a rate constant of 8.66 × 10-7 s-1 at 425 K. Determine the activation energy for this reaction.
_____ 6. The age of an ancient tree trunk is estimated using radiocarbon dating. If the trunk has a C-14 decay rate that is 34% of what it is in living plants, how old is the trunk? The half-life of C-14 is 5730 years.
Answer: 7.4 × 10-3 M
Answer: 160. kJ/mol
Answer: 8.92 × 103 years
NC
DP
I R
efer
ence
Tab
les
for
Ch
emis
try
(Oct
ober
200
6 fo
rm A
-v1)
P
age
7
AC
TIV
ITY
SE
RIE
S o
f H
alog
ens:
2F 2
Cl
2B
r
2I
AC
TIV
ITY
SE
RIE
S o
f M
etal
s L
i R
b K
B
a S
r C
a N
a M
g A
l M
n
Zn
C
r F
e C
d C
o N
i S
n
Pb
[2
H]
Sb
Bi
Cu
H
g A
g P
t A
u
Pol
yato
mic
Ion
s + 4
NH
A
mm
oniu
m
3B
rO−
B
rom
ate
CN
−
Cya
nid
e
23
2C
HO
−
3(C
HC
OO
)−
Ace
tate
4C
lO−
P
erch
lora
te
3C
lO−
C
hlo
rate
2C
lO−
C
hlo
rite
ClO
−
Hyp
och
lori
te
3IO
−
Ioda
te
4M
nO
−
Per
man
gan
ate
3N
O−
N
itra
te
2N
O−
N
itri
te
OH
−
Hyd
roxi
de
3H
CO
−
Hyd
roge
n c
arbo
nat
e
4H
SO
−
Hyd
roge
n s
ulf
ate
SC
N−
T
hio
cyan
ate
2 3C
O−
C
arbo
nat
e 2
27
Cr
O−
D
ich
rom
ate
2 4C
rO−
C
hro
mat
e 2 4
SO
−
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lfat
e 2 3
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−
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lfit
e 3 4
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−
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osph
ate
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eact
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h o
xyge
n t
o fo
rm o
xide
s
Rep
lace
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roge
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rom
aci
ds
Rep
lace
hyd
roge
n f
rom
ste
am
Rep
lace
hyd
roge
n
from
col
d w
ater
General
Chem
istryReference
Sheet
This
reference
sheetad
dresses
someof
themorepeculiar
piecesof
inform
ationthat
needto
bemem
orized
inagen-
eral
chem
istrycourse.
Italso
containsasimple
setof
es-
sential
form
ulasin
chem
istrywithcaution
s,explanations,
andgeneral
tips.
Thissheetismeantto
beas
concise
aspossible,an
dman
yinform
ationin
thetextbook
isleft
outin
favo
rof
caution
san
dtips.
This
sheetis,therefore,
bestusedas
asupple-
mentto,not
areplacementof,thetextbook
.
SIFundamen
talUnits
Mass
Kilog
ram
(kg)
Len
gth
Meter
(m)
Tim
eSecon
d(s)
Tem
perature
Kelvin
(K)
Amou
ntof
substan
ceMole(m
ol)
Electriccu
rren
tAmpere(A
)Luminou
sintensity
Can
dela(cd)
Atomic
Experim
ents
andM
odels
J.J.
Thom
son
Discoverede�
;Cathoderay
Plum
puddingmodel
R.A.Millikan
Measuredcharge
ofe�
;Oildrop
H.Becquerel/M
.Curie
Discoveredradioactivity
E.Rutherford
Discovered↵,�,an
d�rays
Discoverednucleu
s;Goldfoilexperim
ent
J.Chad
wick
Discoveredneu
tron
sN.Boh
rBoh
rmodel
(electronorbits)
Quan
tum
mechan
icists
Quan
tum
model
Polyatomic
Ions
NH
4
+
ammon
ium
OH
�hydroxide
CN
�cyan
ide
C2
O4
2�
oxalate
O2
2�
perox
ide
CNO
�cyan
ate
HSO
4
�hydrogen
sul-
fate
C2
H3
O2
�acetate
SCN
�thiocyan
ate
NO
3
�nitrate
SO
3
2�
sulfite
ClO
4
�perchlorate
CO
3
2�
carb
onate
ClO
3
�chlorate
PO
4
3�
phosphate
ClO
�hypochlorite
S2
O3
2�
thiosulfate
HPO
4
2�
hydrogen
phosphate
CrO
4
2�
chromate
H3
O+
hydronium
Cr 2O
7
2�
dichromate
PO
3
3�
phosphite
MnO
4
�perman
ganate
Hg 2
2�
mercu
ry(I)
N3
�azide
C2
2�
carbide
C4
H4
O6
2�
tartrate
S2
2�
disulfide
O2
�superox
ide
AsO
3
3�
arsenite
PO
2
3�
hypop
hosphite
AsO
4
3�
arsenate
SiO
3
2�
silicate
P2
O7
4�
pyrophosphate
Ionic
SolubilityChart
Soluble
Exception
sNO
3
�Non
eCH
3
COO
�Non
eCl�
Ag+
,Hg 2
2+
,Pb2+
Br�
Ag+
,Hg 2
2+
,Pb2+
I�Ag+
,Hg 2
2+
,Pb2+
SO
4
2�
Sr2
+
,Ba2
+
,Hg 2
2+
,Pb2+
Insoluble
Exception
sS2�
NH
4
+
,alkali
metal
cation
s,Ca2
+
,Sr2
+
,Ba2
+
CO
3
2�
NH
4
+
,alkalimetal
cation
sPO
4
3�
NH
4
+
,alkalimetal
cation
sOH
�NH
4
+
,alkali
metal
cation
s,Ca2
+
,Sr2
+
,Ba2
+
StrongAcidsandBases
Stron
gacidsan
dbases
dissociatein
water
completely.
Stron
gAcids
Stron
gBases
HCl
HClO
4
Alkalimetal
hydroxides
HBr
HNO
3
Ca(OH) 2
HI
H2
SO
4
Sr(OH) 2
HClO
3
Ba(OH) 2
ActivitySeries
Metalsbelow
H+
cannot
reactwithacidsto
form
H2
.More
active
metalsarebetterreducingag
ents.
Fro
mmost
activeto
least
active:
Li+,K
+
,Ba2
+
,Ca2
+
,Na+
,Mg2
+
,Al3
+
,Mn2+
,Zn2+
,Cr3
+
,Fe2
+
,Co2
+
,Ni2
+
,Sn2+
,Pb2+
,H
+
,Cu2+
,Ag+
,Hg2
+
,Pt2
+
,Au3+
FlameColors
Calcium
Brick
red
Cop
per
(I)
Blue
Cop
per
(II)
Green
orblue-green
Potassium
Lilac
Lithium
Darkred
Sodium
Brigh
tyellow
Stron
tium
Red
Barium
Lightgreen
Iron
(III)
Gold
Cesium
Blue–Violet
Indium
Blue
Lead
Blue
Rubidium
Red
–Violet
Phase
Changes
From
solid
From
liquid
From
gas
Tosolid
-freezing
dep
osition
Toliquid
melting
-conden
sation
Toga
ssublimation
vaporization
-
SolutionColors
Cop
per
(II)
Blue
Nickel
Green
Perman
ganate
Purple
Chromate
Yellow
Dichromate
Orange
Iron
(II)
Lightblue
Iron
(III)
Rustyyellow
Thermodynamic
Law
sFirst
Law:Energy
cannot
becreatednor
destroyed
.It
canon
lybetran
sferredin
theform
ofeither
heator
work.
Seco
ndLaw:Anysp
ontaneousreaction
increasestheen
-trop
yof
theuniverse.
Third
Law:Anidealsolidcrystal
at0K
has
anen
trop
yof
0.
Thermodynamic
Form
ulas
Standardthermodynam
icconditions
298K;1atm;1M
Kinetic
energy
K=
mv2
/2
Electrostatic
potential
energy
UE=
(kCQ
1
Q2
)/d
Internal
energy
�E
=q+
wEnthalpy
H=
E+
PV
Specificheat
s=
q/(m
·�T)
Entrop
yin
reversible
reaction
�Ssystem
=(�
H)/T
�Ssurrounding
=�(�
H)/T
Microstate-entrop
yrelation
ship
S=
kln
WGibbsfree
energy
G=
H�
TS
Gibbsfree
energy
chan
ge�G
=�H
�T�S
�G
=�G
�+
RTln
QHess’sLaw
�H
total
=⌃�H
i
Constants
Boltzman
n’s
constan
tkB=
1.38
1⇥
10�23
m2
kg·s
�2
K�1
Cou
lomb’s
constan
tkC=
1/(4⇡✏ 0)=
8.98
8⇥10
9
J·m
/C2
Avo
gadro’s
number
NA=
6.02
2⇥
1023
mol
�1
Farad
ay’s
constan
tF
=9.64
9⇥
104
C/m
olPlanck’s
constan
th=
6.62
6⇥
10�34
J·s
Idealga
sconstan
tsR
=0.08
21(L
·atm
)/(m
ol·K
)R
=8.31
4J/
(mol
·K)
Vacuum
permittivity✏ 0
=1/
(µ0
c2)=
8.85
4⇥
10�12
F/m
Vacuum
permeability
µ0
=1.25
7⇥
10�6
N·A
�2
Atomic
mass
1am
u=
1.66
1⇥
10�24
gElectroncharge
e=
1.60
2⇥
10�19
CElectronvo
lt1eV
=1.60
2⇥
10�19
JAtm
ospheric
pressure
1atm
=1.01
3⇥
105
Pa
Absolute
zero
0K
=-273
.15
�C
Speedof
ligh
tin
vacu
um
c=
2.99
8⇥
108
m/s
Quantu
mM
echanicalForm
ulas
Energy
ofaquan
tum
E=
h⌫
Wavelen
gth-frequen
cyrelation
ship
c=⌫·�
Probab
ilitydistribution
PV
=RR
R
V
| (x,y,z)|2
dxdydz
General
Chem
istryReference
Sheet
This
reference
sheetad
dresses
someof
themorepeculiar
piecesof
inform
ationthat
needto
bemem
orized
inagen-
eral
chem
istrycourse.
Italso
containsasimple
setof
es-
sential
form
ulasin
chem
istrywithcaution
s,explanations,
andgeneral
tips.
Thissheetismeantto
beas
concise
aspossible,an
dman
yinform
ationin
thetextbook
isleft
outin
favo
rof
caution
san
dtips.
This
sheetis,therefore,
bestusedas
asupple-
mentto,not
areplacementof,thetextbook
.
SIFundamen
talUnits
Mass
Kilog
ram
(kg)
Len
gth
Meter
(m)
Tim
eSecon
d(s)
Tem
perature
Kelvin
(K)
Amou
ntof
substan
ceMole(m
ol)
Electriccu
rren
tAmpere(A
)Luminou
sintensity
Can
dela(cd)
Atomic
Experim
ents
andM
odels
J.J.
Thom
son
Discoverede�
;Cathoderay
Plum
puddingmodel
R.A.Millikan
Measuredcharge
ofe�
;Oildrop
H.Becquerel/M
.Curie
Discoveredradioactivity
E.Rutherford
Discovered↵,�,an
d�rays
Discoverednucleu
s;Goldfoilexperim
ent
J.Chad
wick
Discoveredneu
tron
sN.Boh
rBoh
rmodel
(electronorbits)
Quan
tum
mechan
icists
Quan
tum
model
Polyatomic
Ions
NH
4
+
ammon
ium
OH
�hydroxide
CN
�cyan
ide
C2
O4
2�
oxalate
O2
2�
perox
ide
CNO
�cyan
ate
HSO
4
�hydrogen
sul-
fate
C2
H3
O2
�acetate
SCN
�thiocyan
ate
NO
3
�nitrate
SO
3
2�
sulfite
ClO
4
�perchlorate
CO
3
2�
carb
onate
ClO
3
�chlorate
PO
4
3�
phosphate
ClO
�hypochlorite
S2
O3
2�
thiosulfate
HPO
4
2�
hydrogen
phosphate
CrO
4
2�
chromate
H3
O+
hydronium
Cr 2O
7
2�
dichromate
PO
3
3�
phosphite
MnO
4
�perman
ganate
Hg 2
2�
mercu
ry(I)
N3
�azide
C2
2�
carbide
C4
H4
O6
2�
tartrate
S2
2�
disulfide
O2
�superox
ide
AsO
3
3�
arsenite
PO
2
3�
hypop
hosphite
AsO
4
3�
arsenate
SiO
3
2�
silicate
P2
O7
4�
pyrophosphate
Ionic
SolubilityChart
Soluble
Exception
sNO
3
�Non
eCH
3
COO
�Non
eCl�
Ag+
,Hg 2
2+
,Pb2+
Br�
Ag+
,Hg 2
2+
,Pb2+
I�Ag+
,Hg 2
2+
,Pb2+
SO
4
2�
Sr2
+
,Ba2
+
,Hg 2
2+
,Pb2+
Insoluble
Exception
sS2�
NH
4
+
,alkali
metal
cation
s,Ca2
+
,Sr2
+
,Ba2
+
CO
3
2�
NH
4
+
,alkalimetal
cation
sPO
4
3�
NH
4
+
,alkalimetal
cation
sOH
�NH
4
+
,alkali
metal
cation
s,Ca2
+
,Sr2
+
,Ba2
+
StrongAcidsandBases
Stron
gacidsan
dbases
dissociatein
water
completely.
Stron
gAcids
Stron
gBases
HCl
HClO
4
Alkalimetal
hydroxides
HBr
HNO
3
Ca(OH) 2
HI
H2
SO
4
Sr(OH) 2
HClO
3
Ba(OH) 2
ActivitySeries
Metalsbelow
H+
cannot
reactwithacidsto
form
H2
.More
active
metalsarebetterreducingag
ents.
Fro
mmost
activeto
least
active:
Li+,K
+
,Ba2
+
,Ca2
+
,Na+
,Mg2
+
,Al3
+
,Mn2+
,Zn2+
,Cr3
+
,Fe2
+
,Co2
+
,Ni2
+
,Sn2+
,Pb2+
,H
+
,Cu2+
,Ag+
,Hg2
+
,Pt2
+
,Au3+
FlameColors
Calcium
Brick
red
Cop
per
(I)
Blue
Cop
per
(II)
Green
orblue-green
Potassium
Lilac
Lithium
Darkred
Sodium
Brigh
tyellow
Stron
tium
Red
Barium
Lightgreen
Iron
(III)
Gold
Cesium
Blue–Violet
Indium
Blue
Lead
Blue
Rubidium
Red
–Violet
Phase
Changes
From
solid
From
liquid
From
gas
Tosolid
-freezing
dep
osition
Toliquid
melting
-conden
sation
Toga
ssublimation
vaporization
-
SolutionColors
Cop
per
(II)
Blue
Nickel
Green
Perman
ganate
Purple
Chromate
Yellow
Dichromate
Orange
Iron
(II)
Lightblue
Iron
(III)
Rustyyellow
Thermodynamic
Law
sFirst
Law:Energy
cannot
becreatednor
destroyed
.It
canon
lybetran
sferredin
theform
ofeither
heator
work.
Seco
ndLaw:Anysp
ontaneousreaction
increasestheen
-trop
yof
theuniverse.
Third
Law:Anidealsolidcrystal
at0K
has
anen
trop
yof
0.
Thermodynamic
Form
ulas
Standardthermodynam
icconditions
298K;1atm;1M
Kinetic
energy
K=
mv2
/2
Electrostatic
potential
energy
UE=
(kCQ
1
Q2
)/d
Internal
energy
�E
=q+
wEnthalpy
H=
E+
PV
Specificheat
s=
q/(m
·�T)
Entrop
yin
reversible
reaction
�Ssystem
=(�
H)/T
�Ssurrounding
=�(�
H)/T
Microstate-entrop
yrelation
ship
S=
kln
WGibbsfree
energy
G=
H�
TS
Gibbsfree
energy
chan
ge�G
=�H
�T�S
�G
=�G
�+
RTln
QHess’sLaw
�H
total
=⌃�H
i
Constants
Boltzman
n’s
constan
tkB=
1.38
1⇥
10�23
m2
kg·s
�2
K�1
Cou
lomb’s
constan
tkC=
1/(4⇡✏ 0)=
8.98
8⇥10
9
J·m
/C2
Avo
gadro’s
number
NA=
6.02
2⇥
1023
mol
�1
Farad
ay’s
constan
tF
=9.64
9⇥
104
C/m
olPlanck’s
constan
th=
6.62
6⇥
10�34
J·s
Idealga
sconstan
tsR
=0.08
21(L
·atm
)/(m
ol·K
)R
=8.31
4J/
(mol
·K)
Vacuum
permittivity✏ 0
=1/
(µ0
c2)=
8.85
4⇥
10�12
F/m
Vacuum
permeability
µ0
=1.25
7⇥
10�6
N·A
�2
Atomic
mass
1am
u=
1.66
1⇥
10�24
gElectroncharge
e=
1.60
2⇥
10�19
CElectronvo
lt1eV
=1.60
2⇥
10�19
JAtm
ospheric
pressure
1atm
=1.01
3⇥
105
Pa
Absolute
zero
0K
=-273
.15
�C
Speedof
ligh
tin
vacu
um
c=
2.99
8⇥
108
m/s
Quantu
mM
echanicalForm
ulas
Energy
ofaquan
tum
E=
h⌫
Wavelen
gth-frequen
cyrelation
ship
c=⌫·�
Probab
ilitydistribution
PV
=RR
R
V
| (x,y,z)|2
dxdydz
apce
ntra
l.col
lege
boar
d.co
m15
apce
ntra
l.col
lege
boar
d.co
m15
16ap
cent
ral.c
olle
gebo
ard.
com
16ap
cent
ral.c
olle
gebo
ard.
com
• R
ate
= k
[A]0
= k
co
nst
an
t ra
te r
ea
cti
on
s
• [A
] =
-kt
+ [
A] 0
• g
rap
h o
f [A
] v
s. t
ime
is s
trai
gh
t li
ne
wit
h
slo
pe =
-k
an
d y
-in
tercep
t =
[A
] 0
• t ½
= [
A0]/
2k
• w
hen
Ra
te =
M/s
ec, k
= M
/sec
[A] 0
[A]
tim
e
slope =
- k
• R
ate
= k
[A]0
= k
con
stan
t rate
reacti
on
s
• [A
] =
-kt
+ [
A] 0
• gra
ph o
f [A
] vs.
tim
e i
s st
raig
ht
line w
ith
slop
e =
-k a
nd
y-i
nte
rcep
t =
[A
] 0
• t ½ =
[A
0]/
2k
• w
hen
Rate
= M
/sec, k =
M/s
ec
[A] 0
[A]
tim
e
slo
pe =
- k
Fir
st O
rder
Rea
ctio
ns
• R
ate
= k
[A]
• ln
[A]
= -kt
+ l
n[A
] 0
• g
rap
h l
n[A
] v
s. t
ime
giv
es s
trai
gh
t li
ne
wit
h
slo
pe
= -
k a
nd
y-i
nte
rcep
t =
ln
[A] 0
u
sed t
o d
eter
min
e th
e ra
te c
onst
ant
• t ½
= 0
.69
3/k
• th
e h
alf
-lif
e o
f a
fir
st o
rder
rea
ctio
n i
s co
nst
an
t
• th
e w
hen
Ra
te =
M/s
ec, k
= s
ec-1
Fir
st O
rder
Reacti
on
s
• R
ate
= k
[A]
• ln
[A]
= -kt
+ l
n[A
] 0
• gra
ph l
n[A
] vs.
tim
e g
ives
stra
ight
line w
ith
sl
op
e =
-k
and
y-i
nte
rcep
t =
ln
[A] 0
u
sed
to d
ete
rmin
e t
he r
ate
con
stant
• t ½
= 0
.693
/k
• th
e h
alf
-lif
e o
f a
fir
st o
rd
er r
eacti
on
is
con
sta
nt
• th
e w
hen
Rate
= M
/sec, k =
sec
-1
• R
ate
= k
[A]2
• 1/[
A]
= k
t +
1/[
A] 0
• gra
ph 1
/[A
] vs.
tim
e giv
es s
trai
ght
line
wit
h
slop
e =
k a
nd y
-in
tercep
t =
1/[
A] 0
u
sed t
o d
eter
min
e th
e ra
te c
onst
ant
• t ½
= 1
/(k
[A0])
• w
hen
Rate
= M
/sec, k =
M-1·s
ec
-1
• R
ate
= k
[A]2
• 1
/[A
] =
kt
+ 1
/[A
] 0
• g
rap
h 1
/[A
] v
s. t
ime
giv
es s
trai
gh
t li
ne
wit
h
slo
pe =
k a
nd
y-i
nte
rcep
t =
1/[
A] 0
u
sed
to
det
erm
ine
the
rate
co
nst
ant
• t ½
= 1
/(k
[A0])
• w
hen
Ra
te =
M/s
ec, k
= M
-1·s
ec
-1
Ra
te L
aw
s
In
teg
rate
d R
ate
La
ws
Ha
lf-l
ife
form
ula
t ½ =
[A0]
/2k
t ½ =
0.69
3/k
t ½=
1/(k
[A0]
)
ln[N
] t =
-k
t +
ln
[N] 0
ln[N
] t -
ln
[N] 0
= -
kt
[N] t
= [
N] 0
x e
-kt
Eº ce
ll = E
º cath
odee
- E
º ano
de
Eº ce
ll = E
º red
+ Eº o
xid
1.00
A =
1 C
/sec
KIN
ET
ICS