Pasel
))-.
CHM l-52l54 Exam 1 FaI1 2004 l-00 pts
1.
Name:
hrral-=
,/
In the reaction
2llo2+2NO+02
a t 3 0 0 o C , I N O Z I d r o p s f r o m 0 . 0 1 0 0 t o 0 . 0 0 6 5 0 M i n l-00 s.
disappearance
of NO2 for this period is
M/s.
a. 0.35
I
1 )
L 0.003s
c) 0.000035
d. 0.0070
e. 0.00L8
2.
- A-L,";
V
'
At
/ D O
*
I-tui<= ^ LCoJ
remains unchanged
triples
i".ieases
by a facror
of 4
is reduced by a factor
of 2.
z
A
n
law of a reaction
is rate = k[a]x.
is second order in A, are _.
ha.*e-
4
f b] I,I-ts-t
c. t/s
d. I/M
e. s/tQ
The units
of
k,
if
a. remain
.
the
=*-&-fnJ-*
//1-=
s
i N sI
A reaction
was found to be third
order in A.
Increasing
the
concentration
of A by a factor
of 3 will
cause the reaction
rate
,/iq
kept
-= I
tal
::"J;iliJ"
The rate
reaction
a. M/s
constant,
C9,/ rncrease by a factor
c. increase by a factor
d. triple
e. decrease by a factor
of
_ q
o € 5 D - 0 . o l o o= ] - f x / o J
J
A reaction
was found to be second order in carbon monoxide
concentrat.ion.
The rate of the reaction
if the
concentration
of carbon monoxide is doubled r6ith everything
else
b.
c.
(E)
Y.
4.
/
The rate
of 27
of 9
of
cube r o o t
the
of 3
r.fr = h. tA:
n \
/
1
n
l3l
l
-
u-Jl
'
\
4
to
)1+
Page2
5.
Using the information
below, the rate
reaction is .u-1s-1.
A + B - ' P
Experiment
Number
tAl (M)
tBl (M)
L
2
3
38.0
0.278
L5.Z
4 2. 0
2.21
0.273
0.273
0 .B L 9
^
H:
f-r
r
l l
( r'rn wS1
following
2.83
l
at
"^&:
(E) z
o . J
e. 4
150oC.
cons anEt for a
l - 5 0 o C , a n df Jl __ ..1_ X l_o - 3 u f o r t h i s reac
reac r i o n a t 2 5
, ll ? x l o - Y
a. L32
ym
LO
I
b. 55
c. 99
tt
e. 22
what is
the
A S
Y1-, '\jA- )
/ r ' \
llr4,)
\ /
N,tu* ALn)'/
A
s
The rate
lg
the
for Bl Pt"'n f,r P
b*0
7.
for
.jll'ifi)", rc{0, hUD'Lq'
0.763
The rate constant
for
l-00oC, and 1.1- x l_0reaction?
a .
constant
=
overall
order
of
the
,-\
rti cular reaction
s l-.3 x 10-4M-1s-1 at
1
f a t
2 0 0 " C . W h a:t i s the energy of act,ivation
I
?
s
\JCL
q
f u = 1 1 0 1 1 J, I x l o -3
9. 3 t'-l
I
I
I
413;,
[ '
I
I
, -
_; -I u
/
4t-
I
The reaction
CH3-N=C t CH3-C=\
is
a first,-order
lCH3-N=Clg is
reaction.
At 230.3"C, k - 6.29 x l_0-4 s-1.
If
0 . 0 0 1 0 0 M , t C H 3 - N T l i n M a f r e r j - . O O Ox L 0 3 s i s
@ s.rg x 1o-4
b.
c.
d.
e.
2.34
1.88
4.27
1.00
x
x
x
x
L0-4
10-3
L0-3
10-6
-4t t 1"Id,
f,r1.:
),'
,...}'&''o
oo'
x/19
=
6,!,,Lilo (: K' )I
-1,53f,7.--a
=
l.-LA),
7,83(1'
l A l ,= e l - 1
L/ "r
'M
X
I
D
= 5,33
aa\ ,) t'-7
V,.*
Page3
9.
The rat.e constant f or a second-ord.ex, reaction
is 0.1-3 U-1s-1.
If the
initial
concentration
of reactant
is .0.2G mol/L,
it takes
" al"t the concentration
to decrease to 0.13 mol/L.
". 0.0i?
b.o.so
rr
(' 'ir
c. 1.0
Oe.t t4.4 x r.o-r
lo. t !
= At+#
Lfi)"
./
\
1-0. The half-life
of a €rref*rOer
concent,ration of reactant
is
d
e
c
r
e
a
s
e
t
o
0
.
0
5
5
;(o
Y. rn1
Yd . 0ll,
.048
1 1
J
'
The reaction
A -> B is first.
order
the rate constant
for this reaction
time (s)
tAl (M)
0.0
5.0
l - 0 .0
1"5.0
20.0
a. 0.013
b. 0.030
If
^
in
is
?.
Using
[A]
initial
m i n f o-r\ i t
r
the
6-d:;i --,I
"'L*fo\fUr,fL
o
/,/
data
below,
s-1.
t
lrl
L.60
0.80
0.40
0.20
0 .t 0
the
=g '0fi3)t*)^b'ost
,^fo,ort
-
n'"=^-T
,l{=- 0,0533A;-r
e . 8 . 4
(
[ol e1
reaction
is 13 min.
0.085 M, it takes
n
r-^-r
-(r,
( a) a.z
) q
J- -
! -af
shPe
cr^,9?tPo{
X
i
- - r
t- )*,LAi o
(A o.u
Y s.o
e. 3.L x 10-3
1,2. The rate constant
is s-1.
a. 0.693
(6) t. o8 x i.o-3
Y. t.zs
d. 12.5
e. 4.44 x l-0-3
of
a first-order
process
that
tr-= &_r
A
0,(f3
"ft.: L 2 s 5
has a h a l f - I i f e
of 225
0 .( (3
= O . 0 o 3 6 ?s - l
)rn?-Page4
13.
beLween first
Qne difference
and second-order
reactions
is that
*"
half-life
of a first-order
r
e
a
c
t
i
o
n
d
o
e
s
n
o
t
d
e
p
e
n
d on tAlO; t.he
.VQ
talf-rife
of a second.-order reaction
does depend on tAl 0
b. the rate of a first-order
reaction
does not depend on reactant
concentrations;
the rate of a second-order
reaction
does depend. on
reactant
concentrations
c. the rate of a first-order
reaction
depends on reactant
concent,rations;
the rate of a second-order
reaction
does not depend
on reactant
concentrations
d. a first-order
reaction
can be catalyzed;
a second-order reaction
cannot be catalyzed
e. the half-life
of a first-order
reaction
depend.s on tAlo; the
half-1ife
of a second.-order reaction
does not depend on tAl 0
1 4 . As t.he temperature
of a reaction
is increased,
the rate of the reaction
increases
because the
a. reactant molecules collide
less frequently
,^.
molecules collide
( b) reactant
with greater
enerqy p e r c o l l i s i o n
-f. activation
energy is lowered
d. reactant molecules collide
less frequently
and with greater
energry
per collision
e. reactant molecules collide
m o r e frequently
with less energry per
collision
l-5.
In
at
d
(
9.)
c.
d.
e.
l-5.
the potential
energry prof i1e of a reactl-on,
the maxi-mum on the curve is called
the
trroduct
activated
complex
activation
energly
enthalpy of reaction
atomic state
The activation
energy of a first.-order
reaction
o f 4 . 4 L x l - 0 - 3 s - 1 a r 351K and rate constant, of
k.l/mol.
a.
b.
;q.
\d\
Y.
2.67
2.90
0.0s89
22.4
0.4s0
4,4ty/o-3
V,r?
n;-
A
the
species
that
that has a rate const,ant
.\
9.79 x 10-2s-1 588K is
_I_\
l_l_
3st )
B],-vr [ssE
Fr., r )2
1)
q Al t 1 , -t - ,
I
o 1 - t . / , . /
'
," 1r'r
1'7. The stoichiometric
equations
and rate laws for several
reactions
given below.
Of these, only-could represent
an elementary
a_.2A+P
rate=klAl"
6pn+B+p
c. A + 28 e P
d . A + B + g + P
e. A + 28 + P
rare=klAllBl
rate = kAIAW
ra te = ktAl tCI /' ' - /
rate
exists
= k[A] lBf----
are
step.
Page5
18.
The stoichiometric
equation
for
a reaction
is:
2 A + 2 8 s C
The mechanism for
(1)
(2)
(3)
A + 3 - r P
D + 3 r g
A + E + C
Of the following
t.his
reacLion
is:
(sIow; (
(fast )
(fast )
rate
1aws,
is the correcL rate law for this
,PEchanism.
(9 xate = kr [A] [B]
b. Rate = k:[A] [E]
c. Rate = kt [A]2 :.Bl2
d. Rate = kZ [D] [B]
e. Rate = k2k3tAl tBl tDl
1-9. Of the following,
will
lower the activation
reaction.
a. increasing
the concentrations
of reactants
the
temperature
of
the
reaction
_\raising
a
(c-ladding
suitable
catalyst
-d-.
all of the above
e. none of the above
energy
for
a
Page6
20.
Which one of
concentration
a. graph a
b. graph b
c. graph c
d. graph d
e. graph e
the following
and time for
graphs shows the correct
relationship
between
a reaction
that is second order in tAl ?
a) h tAl
time
b)
time
1{Al
time
d)
tAI
time
e)
time
21.
The graph shown below
time for the following
The slope o f
a. k
b. -1lk
c. ln [A]g
this
cfl -t<
Y ru*
2A-C
In [A]
time
line
depicts
the relationship
chemical reacti,on.
is
equal
to
between
concentration
and
PageT
22. which energy difference in the reaction profire
activation
energy for the forward react.ion?
b e l o w corresponds
to
A W
q
9*
c. y
d . z
e . w a n d z
Extentof Reaction
The following
table
questions
below.
For the reaction:
E:<periment
of
e>cperimental
data
is
necessary
lox- 1
1
0.060 M
0.030 M
z
3:3333:333 l::H:
2 3 . W h a t i s the order
ct.
a
l-
b. 0
€)2
d . 3
e. 4
2 4 . What is
a. 0
of
the
initial
rate
0.0248M/s
reaction
o. oe,{s
(g- }j9).X
O,ooll(
\o'oT0/
the order of the reaction
d . 3
e. 4
o - Dot )- I
O.t) -J-/C
3
2 5 . W h a t i s the value of the rate
a . 1 . 1 - 5x 1 0 4
A1;3
\*/ rrs
with
(;
^X rr
/
0.,
=^[&^ - /) Ll0l/-)
"J
r,'x'
^
with.respect
to
CIO2?
,n--
i'x =
? = (s)r
€p
c . 2
answer the
2 C l O z ( a q ) + 2 O H -( a q ) + C l O l - ( a S ) + C l O z - ( a S ) + H z O ( l )
IcIo2l
3
to
\
.esp"et-E6-6H-z
(C- 'EP\V
Q.rrett I
conitant
,
for
the reaction
=r I
r*J_ f
frfr
e. 71-3
o,orq8=^&,06D'[0.030
-k=?)?'d
the