chem1001-lab-1-report-chem-1001-lab-1
docx
keyboard_arrow_up
School
York University *
*We aren’t endorsed by this school
Course
1000
Subject
Chemistry
Date
Feb 20, 2024
Type
docx
Pages
4
Uploaded by CommodoreLightning13357
0.0021
M
0.019
M
3
3
3
3
CHEM
1001
Lab
1
Report
(Reaction
Rates),
Winter
2021
Please
write
your
name,
student
number
and
your
signature
on
every
page
of
work
you
submit.
The
lab
must
be
completed
on
this
template
(either
printed/handwritten/scanned,
or
typed).
If
the
report
is
typed,
proper
scientific
syntax/notation
is
required
(ex:
5.76
x
10
6
instead
of
5.75*10^6)
NOTE:
This
lab
report
must
be
an
independently
produced
piece
of
work.
Collaboration
of
any
kind
is
not
permitted
and
violates
the
Senate
Policy
on
Academic
Honesty.
PART
1
1.
Report
the
stock
solution
concentrations
of
iodate
and
bisulfite
(from
your
personalized
data).
[IO
-
]
in
stock
solution
[HSO
-
]
in
stock
solution
2.
Complete
the
following
tables
for
your
experimental
runs
to
determine
the
reaction
order
with
respect
to
IO
-
.
The
time
you
report
is
the
time
taken
for
the
solution
to
turn
blue.
The
concentration
of
iodate
is
its
initial
concentration
after
the
two
starting
solutions
are
mixed.
Run
NaHSO
3
(mL)
KIO
3
(mL)
H
2
O
(mL)
-
-1
Initial
[IO
3
]
(mol
L
)
Time
(s)
1
10.00
5.00
5.00
0.0047
60.1
2
10.00
7.50
2.50
0.0071
45.2
3
10.00
10.00
0
0.0095
30.5
3.
What
is
the
concentration
of
HSO
-
(mol
L
-1
)
consumed
in
all
three
runs?
Show
your
work.
Input
the
value
into
the
first
column
in
the
table
on
the
next
page
(same
for
all
three
runs).
0.0021
x
10
=
M
2
x
20
M
2
=
0.00105
4.
Complete
the
following
table
to
begin
transforming
your
raw
experimental
results.
Remember
the
stoichiometry
between
HSO
3
-
and
IO
3
-
.
0.00105
0.0095
3
3
Run
-
-1
Δ[HSO
3
]
(mol
L
)
-
-1
Δ[IO
3
]
(mol
L
)
Time
(s)
Initial
Reaction
Rate
(mol
L
-1
s
-1
)
1
0.00105
0.0047
0.0071
60.1
1.747
x
10
-5
2
45.2
2.323
x
10
-5
3
30.5
3.443
x
10
-5
0.00105
5.
Using
the
data
from
the
initial
[IO
-
]
in
each
run
along
with
the
initial
reaction
rates
you
just
calculated,
what
is
the
value
of
“m”
if
rate
=
k[IO
-
]
m
?
Complete
the
table
below
and
use
the
lab
manual
as
a
guide
to
help
complete
your
calculations.
Show
your
work
just
for
comparing
runs
1
and
2
.
Runs
to
Compare
Calculated
m
value
Run
1
and
Run
2
0.68
Run
1
and
Run
3
0.96
Run
2
and
Run
3
1.48
Reported
m
value
to
the
nearest
integer
->
1.00
Run
1
and
2:
1.747
x
10
-5
/
2.323
x
10
-5
=
[
0.0047
/
0.0071
]
m
0.752
=
[0.661]
m
--
take
log
on
both
sides
m=0.68
6.
Calculate
the
“modified”
rate
constant
(k)
using
the
reported
m
value
above
along
with
the
initial
rates
for
all
three
runs.
Remember
to
include
proper
units
for
k.
Show
your
work
for
the
value
of
k
from
run
1
.
Run
Calculated
k
value
Run
1
3.717
x
10
-3
s
-1
Run
2
3.271
x
10
-3
s
-1
Run
3
3.625
x
10
-3
s
-1
Average
k
value
->
3.537
x
10
-3
s-
1
k
=
initial
rate
/
[IO
3
-
]
=
1.747
x
10
-5
/
0.0047
=
3.717
x
10
-3
k
=
2.323
x
10
-5
/
0.0071
=
3.271
x
10
-3
Your preview ends here
Eager to read complete document? Join bartleby learn and gain access to the full version
- Access to all documents
- Unlimited textbook solutions
- 24/7 expert homework help
k
=
3.443
x
10
-5
/
0.0095
=
3.625
x
10
-3
PART
2
7.
Complete
the
following
table
for
your
experimental
runs
to
determine
the
activation
energy.
Remember
the
room
temperature
values
come
from
run
3
in
part
1.
Remember
to
include
proper
units
for
the
rate
constant
k.
Run
Temperature
(K)
Time
(s)
Initial
Reaction
Rate
(mol
L
-1
s
-1
)
Rate
constant
k
Room
temperature
295.95
22.8
4.60
x
10
-5
0.0000460
s
-1
High
temperature
310.05
10.5
1
x
10
-4
0.0001
s
-1
Low
temperature
288.35
64.4
1.63
x
10
-5
0.000163
s-
1
8.
As
explained
in
the
lab
manual,
construct
an
Arrhenius
plot
of
ln
k
vs.
1/T
using
Excel.
Report
the
value
of
the
slope
from
the
linear
trendline
and
use
this
information
to
calculate
the
activation
energy
of
this
reaction.
Include
your
graph
with
your
lab
report
submission.
Slope
Activation
Energy
(kJ
mol
-1
)
Show
your
work
for
calculating
activation
energy
from
the
slope.
Related Documents
Related Questions
Dinitrogen pentoxide rapidly decomposes in the atmosphere with
the rate law noted.
2 N₂O5 (g) → 4 NO2 (g) + O₂(g)
rate= (5.85 × 10-³s-¹) [N₂05]
S
How long does it take for sample to decompose from an initial
concentration of 0.750M to0.211M ?
Answer formatting tip: enter the reaction time using three
significant figures; omit the units of s.
arrow_forward
Be sure to answer all parts.
For the following general reaction, rate -AJAJ and k-1.3 x 102 M.s.
A+B 2C
Use this information to fill in the missing table entries.
Experiment JA] (M) BỊ (M) Initial rate (Mis)
1
0.013
0.250
2.20 x 10
2
0.026
0.250
3
0.500
2.20 x 10
1) Initial reaction rate in experiment 2:
<10
M/s
(Enter your answer in scientific notation.)
2) Initial concentration of A in experiment 3:
arrow_forward
Based on the reaction: 4 A + 5 B = 3 C + 2 D if B is being consumed at a
rate of (6.19x10^-6) M/s, how fast is D being produced (in M/s)?
Enter your answer in scientific notation with 3 sig figs. Do not include any units in
your answer.
Do not round any intermediate calculations.
Note: Your answer is assumed to be reduced to the highest power possible.
Your Answer:
х10
Answer
arrow_forward
The following reaction was analyzed and data was collected.
3 A (g) + 2 B4 (g) + C2 (g) – D (g)
Initial Concentration (mol L)
(Ba]
0.100
Trial
Initial Rate
(mol Ls4)
9.072 x 109
3.629 x 10
2.449 X 107
3.135 х 10%
[A]
[C:]
1
0.100
0.400
2.
0.400
0.100
0.400
0.100
0.300
0.400
4
0.100
0.600
1.60
0.600
0.75
0.100
a) Determine the rate law and rate constant for the reaction. Be sure to show all of your work.
b) Determine the rate for the fifth reaction.
arrow_forward
In a study of the gas phase decomposition of hydrogen iodide at 700 K
HI(g)- → H₂(g) + ½ I₂(g)
the concentration of HI was followed as a function of time.
It was found that a graph of 1/[HI] versus time in seconds gave a
straight line with a slope of 1.64×10-³ M-¹ s-¹ and a y-intercept of
0.418 M-¹.
Based on this plot, the reaction is
order in HI and the rate
constant for the reaction is
M-¹ S-¹.
arrow_forward
In a study of the decomposition of hydrogen iodide on a gold surface at 150 °C
HI(g)% H2(g) + ½ I½(g)
the concentration of HI was followed as a function of time.
It was found that a graph of [HI] versus time in seconds gave a straight line with a
slope of -1.91×10-4 Ms and a y-intercept of 0.235 M.
Based on this plot, the reaction is
reaction is
order in HI and the rate constant for the
Ms!
arrow_forward
Use the information given here to answer both questions (4 and 5).
For the fictitious reaction: AB → A + B
Some data was collected measuring the [AB] at certain time intervals. This data was then graphed as described below.
A graph of 1/[AB] versus time (s) gives a straight line with the equation: y = 0.0052x + 0.1135 and a R2 = 0.9995. A graph of ln[AB] versus time (s) gives a straight line with the equation: y = -0.0068x + 1.725 and a R2 = 0.8925. Assume the data doesn't fit a zero order reaction.
What is the rate law for this reaction?
Select one:
a. Rate = k[AB]2
b. Rate = k[A][B]
c. Rate = k[AB]
d. Rate = k
Using the data from the previous question.
What is the value of the rate constant for the given reaction?
Select one:
a. k = 0.0052 M-1s-1
b. k = 0.0157 Ms-1
c. k = 0.0068 s-1
d. There is no way to determine the value of the rate constant from the given information.
arrow_forward
Nitrosyl chloride is produced from the reaction of nitrogen monoxide and chlorine:2NO(g) + Cl2(g) 2NOCl(g)The following initial rates at a given temperature were obtained for the concentrations listed below.Experiment Initial Rate (mol·L–1·h–1) [NO]0 (mol·L–1) [Cl2]0 (mol·L–1)1 2.21 0.25 0.252 19.89 0.75 0.253 6.63 0.25 0.75From the data, what is the experimental rate law?
arrow_forward
please help and make things clear thank you so much (:
arrow_forward
5.
The rate at which a chemical is depleted from a solution is proportional to the concentration
of the chemical in the solution.
(a) Determine the difference equation (not differential equation) that represents the concentration of the chem-
ical C(t) as a function of time.
(b) Derive the differential equation that represents the concentration of the chemical C(t) as a function of time.
(c) Solve the differential equation with C(0) = Co to obtain C(t).
arrow_forward
what is m and n
arrow_forward
answer choices:
a) 0.12 1/M^2s
b) 0.12 1/Ms
c) 0.15 1/M^2s
d) 0.15 1/Ms
e) 42
arrow_forward
The initial rate data for the reaction 2N205(g) → 4NO2(g) + O2(g) is
shown in the following table. Determine the value of the rate
constant (per second) for this reaction.
Experiment
Rate (M/s)
[N;Os](M)
1.28 x 10²
2.56 x 10?
1
22.5
45.0
Note: Answers must be numeric, not alphanumeric-42, not forty-two.
arrow_forward
According to the reaction below, initial reaction rate was measured at different initial
concentrations of HCI. Suggest a reaction rate expression like - HCIO = KCHCI
4HCI+ CaMg(CO3)2
Mg
2+
2+
+ Ca + 4Cl + 2CO2 + 2H2O
CHCI,O, (mol/cm³)
1
4
2
0.1
0.5
-THCI,O, (mol/s) x 107
1.2
2
1.36
0.36
0.74
arrow_forward
Help me fill out the rest please.
arrow_forward
Nitric oxide gas (NO) reacts with chlorine gas according to the chemical
equation given below.
½CI2
The following initial rates of reaction have been measured for the given
NO
+1
->
NOCI
reagent concentrations.
Experiment
Rate (M/hr)
[NO] (M)
[Cl2] (M)
1
1.19
0.50
0.50
4.79
1.00
0.50
3.
9.59
1.00
1.00
What is the rate law for this reaction?
2.
arrow_forward
8.
Consider the reaction:
Trial #
1
2
3
4
5
6
2NH (g) + 302(g) + 2CH(g) → 2 HCN(g) + 6H₂O(g)
[CH₂] (M)
0.37
0.45
0.45
0.26
0.45
0.17
[NH)] (M)
0.035
0.035
0.054
0.054
0.054
0.079
c. Write the rate law.
b. Determine the overall reaction order.
[0₂] (M)
0.12
0.27
0.12
0.27
a. Determine the order with respect to each of the reactants.
0.27
0.32
d. Solve for the value of the rate constant with units.
Rate M/hr
2.3 x 10²
1.6 x 102
5.5 x 10²
3.7 x 102
3.7 x 10²
arrow_forward
Time (min)
0.5
1
15
2
2.5
3
4.7
From time zero, how long (in min) will it take for the drug's concentration to drop down to 0.05 mg/ml?
(Hint: While you can, you do not have to calculate Co to answer this question)
A. 5.1
B. 7.5
C. 9.5
[Z] (mg/mL)
1
0.66
0.5
0.4
0.334
0.286
0.192
D. 19.5
E. 14.8
arrow_forward
In a study of the gas phase decomposition of nitrogen dioxide at 383 °C
NO₂(g) →→→NO(g) + ½ O₂(g)
the concentration of NO₂ was followed as a function of time.
It was found that a graph of 1/[NO₂] versus time in seconds gave a straight line with a slope of 0.815 M-¹ s¹ and a y-intercept of 11.5 M-¹.
Based on this plot, the reaction is [
✓order in NO₂ and the rate constant for the reaction is
M-¹ S-¹.
arrow_forward
Experimental data for determining rates
# of Experiment
Volume 0.623 M
H2O2 (aq), mL
Volume 0.135M
KMnO4 (aq), mL
Elapsed time, s
1
10.00
2.00
199.1
2
10.00
4.00
199.1
3
5.00
2.00
796.6
What is the rate for Experiment 1?
Thanks.
arrow_forward
The following data were collected for the reaction below.
2 NO (g) + O2 (g) --> 2 NO, (g)
Initial Rate
Experiment
INO] (M)
HO:1 (M)
(M/s)
1.
0.0126
0.0125
1.41 X 10 2
2
0,0252
0.0125
5.64 X 102
13.
0.0252
0.0250
1.13 X 101
What is the rate when (NO] = 0.100 M and [0,] = 0.200 M?
O 7.11 X 10 M251
O 2 M/s
0:0.002 M/s
(0 14.2 M/s
arrow_forward
(Can I get the answer in not more than 45 mins please? or asap. Thank you!)
arrow_forward
1-arr
In a study of the decomposition of dinitrogen pentoxide in carbon tetrachloride solution at 30 °C
N2O5-
→2 NO2 + ½ O2
the concentration of N,O5 was followed as a function of time.
It was found that a graph of In[N2O5] versus time in minutes gave a straight line with a slope of -6.31×10* min and a y-
intercept of -1.34 .
Based on this plot, the reaction
O order in N,0g and the rate constant for the reaction is
min-1.
zero
first
second
arrow_forward
What is the order of composition of C4H6?
what is the rate constant k? what is the average rate of disappearance of C4H6 between 0 and 1000 seconds ? Please circle alll answers
arrow_forward
5.0 mL of reactant A (0.10 M) was added to 5.0 mL of reactant B (0.25 M). The reaction was monitored until all of A was consumed, according to the
reaction A + 2B → C. The measured reaction time was 75. seconds. What is the rate of this reaction? Round your answer to 2 significant digits.
M
arrow_forward
I am taking an online chem class and it’s harder than I thought. I have the answers to my whole study guide but I want to understand the WHY of the answers. Thank you!
arrow_forward
Initial rate data was collected for the reaction
3 BHT + 4 MHF → RND + ZWP
Initial rate (M/s)
5.0 x 102
Run
[BHT]
[МHF]
2.00
1
1.00
2.2 x 102
2.62 x 103
2
0.50
2.00
0.25
1.00
4
1.00
0.25
7.6 x 104
.a.
Write the generic rate law
.b. Find the order of reaction with respect to BHT and the order of reaction with
respect to MHF.
.C.
Find k
3.
arrow_forward
The following images depict the evolution of the chemical reaction A → B over time:
B
Part A
A-
t=0 s
Compare the reaction A → B to the reaction Y→ Z. Which reaction has the faster rate?
Y→Z
t = 20 s
t=0 s
t = 20 s
t = 40 s
t = 40 s
t = 60 s
t = 60 s
A
B
Y
Z
●
arrow_forward
SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Related Questions
- Dinitrogen pentoxide rapidly decomposes in the atmosphere with the rate law noted. 2 N₂O5 (g) → 4 NO2 (g) + O₂(g) rate= (5.85 × 10-³s-¹) [N₂05] S How long does it take for sample to decompose from an initial concentration of 0.750M to0.211M ? Answer formatting tip: enter the reaction time using three significant figures; omit the units of s.arrow_forwardBe sure to answer all parts. For the following general reaction, rate -AJAJ and k-1.3 x 102 M.s. A+B 2C Use this information to fill in the missing table entries. Experiment JA] (M) BỊ (M) Initial rate (Mis) 1 0.013 0.250 2.20 x 10 2 0.026 0.250 3 0.500 2.20 x 10 1) Initial reaction rate in experiment 2: <10 M/s (Enter your answer in scientific notation.) 2) Initial concentration of A in experiment 3:arrow_forwardBased on the reaction: 4 A + 5 B = 3 C + 2 D if B is being consumed at a rate of (6.19x10^-6) M/s, how fast is D being produced (in M/s)? Enter your answer in scientific notation with 3 sig figs. Do not include any units in your answer. Do not round any intermediate calculations. Note: Your answer is assumed to be reduced to the highest power possible. Your Answer: х10 Answerarrow_forward
- The following reaction was analyzed and data was collected. 3 A (g) + 2 B4 (g) + C2 (g) – D (g) Initial Concentration (mol L) (Ba] 0.100 Trial Initial Rate (mol Ls4) 9.072 x 109 3.629 x 10 2.449 X 107 3.135 х 10% [A] [C:] 1 0.100 0.400 2. 0.400 0.100 0.400 0.100 0.300 0.400 4 0.100 0.600 1.60 0.600 0.75 0.100 a) Determine the rate law and rate constant for the reaction. Be sure to show all of your work. b) Determine the rate for the fifth reaction.arrow_forwardIn a study of the gas phase decomposition of hydrogen iodide at 700 K HI(g)- → H₂(g) + ½ I₂(g) the concentration of HI was followed as a function of time. It was found that a graph of 1/[HI] versus time in seconds gave a straight line with a slope of 1.64×10-³ M-¹ s-¹ and a y-intercept of 0.418 M-¹. Based on this plot, the reaction is order in HI and the rate constant for the reaction is M-¹ S-¹.arrow_forwardIn a study of the decomposition of hydrogen iodide on a gold surface at 150 °C HI(g)% H2(g) + ½ I½(g) the concentration of HI was followed as a function of time. It was found that a graph of [HI] versus time in seconds gave a straight line with a slope of -1.91×10-4 Ms and a y-intercept of 0.235 M. Based on this plot, the reaction is reaction is order in HI and the rate constant for the Ms!arrow_forward
- Use the information given here to answer both questions (4 and 5). For the fictitious reaction: AB → A + B Some data was collected measuring the [AB] at certain time intervals. This data was then graphed as described below. A graph of 1/[AB] versus time (s) gives a straight line with the equation: y = 0.0052x + 0.1135 and a R2 = 0.9995. A graph of ln[AB] versus time (s) gives a straight line with the equation: y = -0.0068x + 1.725 and a R2 = 0.8925. Assume the data doesn't fit a zero order reaction. What is the rate law for this reaction? Select one: a. Rate = k[AB]2 b. Rate = k[A][B] c. Rate = k[AB] d. Rate = k Using the data from the previous question. What is the value of the rate constant for the given reaction? Select one: a. k = 0.0052 M-1s-1 b. k = 0.0157 Ms-1 c. k = 0.0068 s-1 d. There is no way to determine the value of the rate constant from the given information.arrow_forwardNitrosyl chloride is produced from the reaction of nitrogen monoxide and chlorine:2NO(g) + Cl2(g) 2NOCl(g)The following initial rates at a given temperature were obtained for the concentrations listed below.Experiment Initial Rate (mol·L–1·h–1) [NO]0 (mol·L–1) [Cl2]0 (mol·L–1)1 2.21 0.25 0.252 19.89 0.75 0.253 6.63 0.25 0.75From the data, what is the experimental rate law?arrow_forwardplease help and make things clear thank you so much (:arrow_forward
- 5. The rate at which a chemical is depleted from a solution is proportional to the concentration of the chemical in the solution. (a) Determine the difference equation (not differential equation) that represents the concentration of the chem- ical C(t) as a function of time. (b) Derive the differential equation that represents the concentration of the chemical C(t) as a function of time. (c) Solve the differential equation with C(0) = Co to obtain C(t).arrow_forwardwhat is m and narrow_forwardanswer choices: a) 0.12 1/M^2s b) 0.12 1/Ms c) 0.15 1/M^2s d) 0.15 1/Ms e) 42arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning