Factors Affecting Reaction Rates Lab Report Dr. Z Edits (1)
docx
keyboard_arrow_up
School
Southern New Hampshire University *
*We aren’t endorsed by this school
Course
101L
Subject
Chemistry
Date
Feb 20, 2024
Type
docx
Pages
7
Uploaded by DeanMoon13043
Factors Affecting Reaction Rates
Date: 11/19/2023
Data
Activity 1
Data Table 1: Calibration Trial
Na
2
S
2
O
3
(drops)
Reaction time (sec)
1
8 drops
29 seconds 2
6 drops 21 seconds 3
N/A
N/A
Question 1:
How many drops will be used in the remaining experiments? 6 drops of Na
2
S
2
O
3 will be used in the remaining experiments.
Activity 2
Data Table 2a. Effects of KI (I
-
) Concentration Trial
KI
(drops)
HCl
(drops)
Starch
(drops)
H
2
O
(drops)
Na
2
S
2
O
3
(drops)
H
2
O
2
(mL)
Time
1
(sec)
Time
2
(sec)
Average
time
(T
avg
)
(sec)
Average
Rate
(1/T
avg
)
1
8
2
4
0
6
0.4
24
(24 +
22)/2 = 23 1/23=
.043
2
8
2
4
0
6
0.4
22
3
6
2
4
2
6
0.4
33
(33
+36)/2
=34.5
1/34.5=
.029
Trial
KI
(drops)
HCl
(drops)
Starch
(drops)
H
2
O
(drops)
Na
2
S
2
O
3
(drops)
H
2
O
2
(mL)
Time
1
(sec)
Time
2
(sec)
Average
time
(T
avg
)
(sec)
Average
Rate
(1/T
avg
)
4
6
2
4
2
6
0.4
36
5
4
2
4
4
6
0.4
41
(41 +
39)/2 = 40
1/40=
.025
6
4
2
4
4
6
0.4
39
7
2
2
4
6
6
0.4
87
(87+83)/2
= 85
1/85=
.012
8
2
2
4
6
6
0.4
83
Data Table 2b. Effects of H
2
O
2
Concentration Trial
KI
(drops)
HCl
(drops)
Starch
(drops)
H
2
O
(mL)
Na
2
S
2
O
3
(drops)
H
2
O
2
(mL)
Time
1
(sec)
Time
2
(sec)
Average time
(T
avg
) (sec)
Average
Rate
(1/T
avg
)
1
8
2
4
0
6
0.4
24
(24 + 21)/2=
22.5
1/22.5=
.044
2
8
2
4
0
6
0.4
21
3
8
2
4
0.1
6
0.3
32
(32+30)/2=31
1/31=
.032
4
8
2
4
0.1
6
0.3
30
5
8
2
4
0.2
6
0.2
42
(42 + 48)/2 =
45
1/45=
.022
6
8
2
4
0.2
6
0.2
48
7
8
2
4
0.3
6
0.1
30
(30 + 27)/2
=28.5
1/28.5=
.035
8
8
2
4
0.3
6
0.1
27
©2016 2 Carolina Biological Supply Company
Data Table 2c. Effects of HCl (H
+
) Concentration
Trial
KI
(drops)
HCl
(%)
Starch
(drops)
H
2
O
(drops)
Na
2
S
2
O
3
(drops)
H
2
O
2
(mL)
Time
1
(sec)
Time
2
(sec)
Average
time
(T
avg
) (sec)
Average
Rate
(1/T
avg
)
1
8
100%
4
0
6
0.4
20
(20+25)/2=
22.5
1/22.5=
.044
2
8
100%
4
0
6
0.4
25
3
8
75%
4
0
6
0.4
24
(24+22)/2=
23
1/23=
.043
4
8
75%
4
0
6
0.4
22
5
8
50%
4
0
6
0.4
25
(25+28)/2=
26.5
1/26.5=
.038
6
8
50%
4
0
6
0.4
28
7
8
25%
4
0
6
0.4
22
(22 + 26)/2
=24
1/24 =
.042
8
8
25%
4
0
6
0.4
26
Activity 3
Data Table 3. Temperature Effects
Water bath trial
Temperature of the water
bath (°C)
Reaction time (sec)
Cold water
3
25 seconds Room-temperature water
20
18 seconds Hot water
56
6 seconds Question 2:
Explain how each of these treatments affected the reaction rate. Describe the effect at a molecular level.
a. Concentration b. Temperature ©2016 2 Carolina Biological Supply Company
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
Activity 4
Data Table 4. Catalyst Trial
Water (drops)
Diluted CuSO
4
Solution (drops)
Reaction time (sec)
1
4
0
22 seconds 2
3
1
10 seconds 3
2
2
9 seconds 4
1
3
8 seconds 5
0
4
6 seconds Question 3:
How did the addition of copper (II) sulfate affect the reaction rate? Did the amount of catalyst affect the reaction rate?
The addition of copper (II) sulfate increased the reaction rate significantly. The greater the amount of catalyst added (paired with a decrease in the amount of water added each trial), the lower the reaction time (in seconds) was each trial. Activity 5: Data Table 5. Orders of Reactants in the Rate Law
Determine the actual Rate Law: R = k[I
–
]
m
[H
2
O
2
]
n
[H
+
]
p
Calculated Reaction order (X) (e.g. (
concentration
1
concentration
2
)
X
=
rate
1
rate
2
)
You must show your full calculation work for credit. ©2016 2 Carolina Biological Supply Company
Reactant
Concentration
Average
Rate
(1/T
avg
)
Calculated Reaction
order (X)
Show work! Average
Reaction
order
Reaction
Order
(integer)
KI (I
)
8 drops
.043
(1.369
+ .366 +
1.059)/2 =
.931
m = 1
1.369
KI (I
)
6 drops
.029
.366
KI (I
)
4 drops
.025
1.059
KI (I
)
2 drops
.012
You must show your full calculation work for credit. Reactant
Concentration
Average
Rate
(1/T
avg
)
Calculated Reaction
order (X)
Show work! Average
Reaction
order
Reaction
Order
(integer)
H
2
O
2
0.4 mL
.044
(.831
+ .924
-.544)/3
=
.404
n = 0
.831
H
2
O
2
0.3 mL
.032
©2016 2 Carolina Biological Supply Company
Reactant
Concentration
Average
Rate
(1/T
avg
)
Calculated Reaction
order (X)
Show work! Average
Reaction
order
Reaction
Order
(integer)
.924
H
2
O
2
0.2 mL
.022
-.544
H
2
O
2
0.1 mL
.035
You must show your full calculation work for credit. Reactant
Concentration
Average
Rate
(1/T
avg
)
Calculated Reaction
order (X)
Show work! Average
Reaction
order
Reaction
Order
(integer)
HCl (H
+
)
100%
.044
(.08 + .305
- .144)/3 =
.08
p = 0
.08 HCl (H
+
)
75%
.043
.305
HCl (H
+
)
50%
.038
-.144
HCl (H
+
)
25%
.042
©2016 2 Carolina Biological Supply Company
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
Rate Law
R = k
[I–]^1 [H
2
O
2
]^0 [H ]^0
Overall Order of the Reaction
1 + 0 + 0 = 1 Question 4:
Use the rate-law expression you
determined for Data Table 5 to answer the following questions. Answer using doubled, tripled, quadrupled, halved, quartered, no change, etc. A)
If the concentration of I
–
was doubled, how would that affect the reaction rate?
Double.
B)
If the concentration of H
2
O
2
was halved, how would that affect the reaction rate?
No change. C)
If the concentrations of I
–
and H
2
O
2
were both doubled, how would that affect the reaction rate?
It would double due to the concentration of I-, but the reaction rate would not be impacted by the concentration of H2O2.
D)
If the concentration of H
+
(HCl) was doubled, how would that affect the reaction rate?
No change. ©2016 2 Carolina Biological Supply Company
Related Documents
Related Questions
y courses / S22 CHEM 161_01_04 / 27 March - 2 April/ Quiz 9
Time left 0:53:13
Calculate the mass of oxygen that will be prepared through the decomposition
of 50 kg of potassium chlorate ( KCIO3 , Molar mass= 122.55 g/mol)
2 KCIO3 →2 KCI + 3 O2
Select one:
O a. 612 kg
O b. 12.25 kg
O c. 9.8 kg
O d. 19.6 kg
Next page
arrow_forward
#2
arrow_forward
Using the following chemical equation and data:
3A + B + 2C --> D + 2E
Experiment
Initial [A]
Initial [B]
Initial [C]
Initial Rate
1
1.0 x 10-2
4.0 x 10-3
2.0 x 10-2
5 mM/s
2
1.0 x 10-2
8.0 x 10-3
2.0 x 10-2
10 mM/s
3
2.0 x 10-2
8.0 x 10-3
2.0 x 10-2
40 mM/s
4
2.0 x 10-2
8.0 x 10-3
1.0 x 10-2
40 mM/s
Determine the initial rate of reaction if the initial concentrations of A, B, C are 3 x 10-2 M, 5 x 10-3 M, 5 x 10-5 M, respectively, for the reaction.
arrow_forward
Using the following chemical equation and data:
3A + B + 2C --> D + 2E
Experiment
Initial [A]
Initial [B]
Initial [C]
Initial Rate
1
1.0 x 10-2
4.0 x 10-3
2.0 x 10-2
5 mM/s
2
1.0 x 10-2
8.0 x 10-3
2.0 x 10-2
10 mM/s
3
2.0 x 10-2
8.0 x 10-3
2.0 x 10-2
40 mM/s
4
2.0 x 10-2
8.0 x 10-3
1.0 x 10-2
40 mM/s
Determine the rate equation.
arrow_forward
Using the following chemical equation and data:
3A + B + 2C --> D + 2E
Experiment
Initial [A]
Initial [B]
Initial [C]
Initial Rate
1
1.0 x 10-2
4.0 x 10-3
2.0 x 10-2
5 mM/s
2
1.0 x 10-2
8.0 x 10-3
2.0 x 10-2
10 mM/s
3
2.0 x 10-2
8.0 x 10-3
2.0 x 10-2
40 mM/s
4
2.0 x 10-2
8.0 x 10-3
1.0 x 10-2
40 mM/s
Calculate the specific rate constant (k).
arrow_forward
Calculation Tables
Table 4- Logarithms
[l]o (M)
-log[I]o
-log(rate) [H2O2]o (M)
0.0100
-log[H2O2]o
2.00
Experiment #
Rate (M/s)
1
2.63 x10-6
5.58
0.0200
1.70
5.18 x 106
0.0100
0.0400
0.0600
8.01 x 10-6
1.62 x 105
0.0100
4
0.0200
0.0600
3.21 x 105
0.0400
0.0600
Table 5- Rate Constants
Experiment [H2OzJo(M)
[H2O2]om
Initial rate
k
#
(M/s)
2.63 x10-6
1
0.0100
0.0200
2
0.0100
0.0400
5.18 x 10-6
0.0100
0.0600
8.01 x 106
4
0.0200
0.0600
1.62 x 105
5
0.0400
0.0600
3.21 x 105
Value of m (2 significant figures):
Value of n (2 significant figures):
verage value of k (3 significant figures):
arrow_forward
Analyze the following reaction mechanism:
1. H2O2 → H2O + O
2. O + CF2CI2 → CIO + CF2CI
3. CIO + O3 → CI + 202
4. Cl + CF2CI → CF2CI2
From the mechanism provided, write the overall balanced
equation for this chemical reaction. Ignore phases.
4-
2.
2+
3+
4+
1
2
3
4
6
8
04
O6
Do
1
3
8.
(s)
(1)
(g)|(aq)
+
F
CI
H
C
Reset
• x H2O || Delete
3.
arrow_forward
Pre-lab question #10-1: A reaction between substances A and B has been found to
give the following data: 3 A + 2 B → 2 C + D
[A], M
[В], М
Rate of Appearance of
С, М/hr
1.0 x 10-2
1.0
0.300 x 10-6
1.0 x 10-2
3.0
8.10 x 10-6
2.0 x 10-2
3.0
3.24 x 10-5
2.0 x 10-2
1.0
1.20 х 10-6
3.0 x 10-2
3.0
7.30 x 10-5
Using the data above, determine the following:
Pre-lab question #10-1: a) Order of the reaction with respect to A and B
1st order with respect to A, and 2nd order with respect to B
2nd order with respect to A, and 2nd order with respect to B
2nd order with respect to A, and 3rd order with respect to B
3rd order with respect to A, and 2nd order with respect to B
arrow_forward
Pls help ASAP. Pls show all work.
arrow_forward
What is m and n
arrow_forward
#
3
E
D
C
Energy diagrams for two reactions are shown.
Macmillan Learning
Energy (kJ/mol)
e
150
100
50-
What is the heat of reaction for Reaction A?
AHrxnA =
4
FER
20
What is the activation energy for Reaction A?
R
F
V
Reaction progress
Reaction A
5
T
G Search or type URL
G
B
tv
6
MacBook Pro
Y
Ⓒ
H
201
7
N
U
S
J
kJ
mol
00
8
M
I
Energy (kJ/mol)
150 T
100-
NIMZAO
✪
50
What is the heat of reaction for Reaction B?
AHxnB =
What is the activation energy for Reaction B?
K
(
- O
9
<
O
I
*
)
-C
O
Reaction progress
Reaction B
L
command
»)
P
. V
=
:
P
W
;
242)
{
option
[
SEC
e
=
?
O
kJ
mol
1
delete
retu
arrow_forward
Lab 6: Chemical Reactions
Post-Lab Questions
Station V: Heating Cu with Atmospheric O₂
Chemical equation:
Complete ionic equation:
Net ionic equation:
General reaction type:
Station VI: Reacting CuSO4 Solution with Steel Wool (Fe)
arrow_forward
3. Using the following data below for the reaction of AB A+ B
Time (sec)
[AB] (M)
0.0
4.77 x 104
1.00
2.00
3.00
5.00
10.00
30.00
-50.00
4.31 x 104
3.91 x 104
3.53 x 104
2.89 x 104
1.76 x 10-4
2.4 x 10-5
3.2 x 10-6
a. Plot the data shown and determine what order the reaction
b. Calculate the k value for this reaction.
C.
What is the half-life for this reaction?
d. What is the concentration of AB after 40 seconds?
arrow_forward
ttps://prod04-cnow-owl.ceng...
✪
>
Google N Home - Netflix Disney+ | Movies a...
Problems
1 pt
1 pt
1 pt
1 pt
1 pt
1 pt
1 pt
1 pt
1 pt
1 pt
1 pt
1 pt
1 pt
1 pt
1 pt
) 1 pt
Concentration
A
Submit Answer
[References]
Sulfuryl chloride, SO2 Cl2, decomposes when heated.
SO₂ Cl2 (9) → SO2 (9) + Cl₂ (g)
In an experiment, the initial concentration of SO₂Cl₂
was 1.31 x 10-2 mol/L. If the rate constant is
2.2 x 105/s, what is the concentration of SO₂Cl2 after
6.0 hr? The reaction is first order.
6 item attempts remaining
mol/L
Ⓒ
Try Another Version
>
M
Other fa
arrow_forward
Review | Constants | Periodic Table
The half-life of a reaction, t1/2. is the time it takes
for the reactant concentration A to decrease by
half. For example, after one half-life the
concentration falls from the initial concentration
[A]o to [A]o/2, after a second half-life to [A]o/4;
after a third half-life to [Ao/8, and so on. on.
For a first-order reaction, the half-life is constant. It depends only on the rate constant k and not on the reactant
concentration. It is expressed as
0.693
t1/2
For a second-order reaction, the half-life depends on the rate constant and the concentration of the reactant and
so is expressed as
t1/2 =
Part A
A certain first-order reaction (A→products) has a rate constant of 3.60x103s at 45 °C. How many
minutes does it take for the concentration of the reactant, A, to drop to 6.25% of the original concentration?
Express your answer with the appropriate units.
> View Available Hint(s)
HA
Value
min
arrow_forward
I need an answer for this question with solutions. Thank you. #4
arrow_forward
I Review | Constants | Periodic Table
The half-life of a reaction, t1/2, is the time it takes
for the reactant concentration A to decrease by
half. For example, after one half-life the
concentration falls from the initial concentration
Ao to [Alo/2, after a second half-life to [A]o/4,
after a third half-life to [Alo/8, and so on. on.
v Correct
Part B
A certain second-order reaction (B→products) has a rate constant of 1.80x10-3 M.s-1 at 27°C and an
initial half-life of 246 s. What is the concentration of the reactant B after one half-life?
Express your answer with the appropriate units.
• View Available Hint(s)
?
HA
2.04
M
arrow_forward
Fill in the table with the information of Average rates of reaction from experimental data
arrow_forward
Pre-lab question #10-2: A reaction between substances A and B has been found to
give the following data: 3 A + 2 B → 2 C + D
[A], M
[В], М
Rate of Appearance of
C, M/hr
1.0 x 10-2
1.0
0.300 x 10-6
1.0 x 10-2
3.0
8.10 x 10-6
2.0 x 10-2
3.0
3.24 x 10-5
2.0 x 10-2
1.0
1.20 x 10-6
3.0 x 10-2
3.0
7.30 x 10-5
Using the data above, determine the following:
Pre-lab question #10-2: b) find the rate expression for the reaction.
Rate = k[A]°[B] 2
Rate = k[A]²[B]3
%3D
Ok = [A]2[B]3
%D
Ok = [A]°[B]?
arrow_forward
1:37
Search
1
4
The activation energy Ea for a
particular reaction is 42.2 kJ/mol.
How much faster is the reaction
at 343 K than at 323 K? (R =
8.314 J/mol K)
●
7
2
+/-
LO
5
Question 1 of 18
8
30
9
0
Tap here or pull up for additional resources
3
6
5G+ 68
Submit
X
с
x 100
arrow_forward
2. For the reaction A + B + C → products, the following data were collected:
Initial concentration (mmol.L-1)
[A]. [B]. [C]
Experiment
2.06
3.05
4.00
0.87
3.05
4.00
0.50
0.50 0.50
1.00
0.50 1.00
1
2
3
4
Initial rate (mmol • L-1.s-1)
3.7
0.66
0.013
0.072
The initial rate given in the table above is for the rate of loss of A.
(a) Write the rate law for the reaction.
(b) Determine the overall order of the reaction.
(c) Determine the value of the rate constant. Convert mmol to mol first.
arrow_forward
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
Please show all work!
arrow_forward
Please don't provide hand writtin solution....
arrow_forward
SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
Related Questions
- y courses / S22 CHEM 161_01_04 / 27 March - 2 April/ Quiz 9 Time left 0:53:13 Calculate the mass of oxygen that will be prepared through the decomposition of 50 kg of potassium chlorate ( KCIO3 , Molar mass= 122.55 g/mol) 2 KCIO3 →2 KCI + 3 O2 Select one: O a. 612 kg O b. 12.25 kg O c. 9.8 kg O d. 19.6 kg Next pagearrow_forward#2arrow_forwardUsing the following chemical equation and data: 3A + B + 2C --> D + 2E Experiment Initial [A] Initial [B] Initial [C] Initial Rate 1 1.0 x 10-2 4.0 x 10-3 2.0 x 10-2 5 mM/s 2 1.0 x 10-2 8.0 x 10-3 2.0 x 10-2 10 mM/s 3 2.0 x 10-2 8.0 x 10-3 2.0 x 10-2 40 mM/s 4 2.0 x 10-2 8.0 x 10-3 1.0 x 10-2 40 mM/s Determine the initial rate of reaction if the initial concentrations of A, B, C are 3 x 10-2 M, 5 x 10-3 M, 5 x 10-5 M, respectively, for the reaction.arrow_forward
- Using the following chemical equation and data: 3A + B + 2C --> D + 2E Experiment Initial [A] Initial [B] Initial [C] Initial Rate 1 1.0 x 10-2 4.0 x 10-3 2.0 x 10-2 5 mM/s 2 1.0 x 10-2 8.0 x 10-3 2.0 x 10-2 10 mM/s 3 2.0 x 10-2 8.0 x 10-3 2.0 x 10-2 40 mM/s 4 2.0 x 10-2 8.0 x 10-3 1.0 x 10-2 40 mM/s Determine the rate equation.arrow_forwardUsing the following chemical equation and data: 3A + B + 2C --> D + 2E Experiment Initial [A] Initial [B] Initial [C] Initial Rate 1 1.0 x 10-2 4.0 x 10-3 2.0 x 10-2 5 mM/s 2 1.0 x 10-2 8.0 x 10-3 2.0 x 10-2 10 mM/s 3 2.0 x 10-2 8.0 x 10-3 2.0 x 10-2 40 mM/s 4 2.0 x 10-2 8.0 x 10-3 1.0 x 10-2 40 mM/s Calculate the specific rate constant (k).arrow_forwardCalculation Tables Table 4- Logarithms [l]o (M) -log[I]o -log(rate) [H2O2]o (M) 0.0100 -log[H2O2]o 2.00 Experiment # Rate (M/s) 1 2.63 x10-6 5.58 0.0200 1.70 5.18 x 106 0.0100 0.0400 0.0600 8.01 x 10-6 1.62 x 105 0.0100 4 0.0200 0.0600 3.21 x 105 0.0400 0.0600 Table 5- Rate Constants Experiment [H2OzJo(M) [H2O2]om Initial rate k # (M/s) 2.63 x10-6 1 0.0100 0.0200 2 0.0100 0.0400 5.18 x 10-6 0.0100 0.0600 8.01 x 106 4 0.0200 0.0600 1.62 x 105 5 0.0400 0.0600 3.21 x 105 Value of m (2 significant figures): Value of n (2 significant figures): verage value of k (3 significant figures):arrow_forward
- Analyze the following reaction mechanism: 1. H2O2 → H2O + O 2. O + CF2CI2 → CIO + CF2CI 3. CIO + O3 → CI + 202 4. Cl + CF2CI → CF2CI2 From the mechanism provided, write the overall balanced equation for this chemical reaction. Ignore phases. 4- 2. 2+ 3+ 4+ 1 2 3 4 6 8 04 O6 Do 1 3 8. (s) (1) (g)|(aq) + F CI H C Reset • x H2O || Delete 3.arrow_forwardPre-lab question #10-1: A reaction between substances A and B has been found to give the following data: 3 A + 2 B → 2 C + D [A], M [В], М Rate of Appearance of С, М/hr 1.0 x 10-2 1.0 0.300 x 10-6 1.0 x 10-2 3.0 8.10 x 10-6 2.0 x 10-2 3.0 3.24 x 10-5 2.0 x 10-2 1.0 1.20 х 10-6 3.0 x 10-2 3.0 7.30 x 10-5 Using the data above, determine the following: Pre-lab question #10-1: a) Order of the reaction with respect to A and B 1st order with respect to A, and 2nd order with respect to B 2nd order with respect to A, and 2nd order with respect to B 2nd order with respect to A, and 3rd order with respect to B 3rd order with respect to A, and 2nd order with respect to Barrow_forwardPls help ASAP. Pls show all work.arrow_forward
- What is m and narrow_forward# 3 E D C Energy diagrams for two reactions are shown. Macmillan Learning Energy (kJ/mol) e 150 100 50- What is the heat of reaction for Reaction A? AHrxnA = 4 FER 20 What is the activation energy for Reaction A? R F V Reaction progress Reaction A 5 T G Search or type URL G B tv 6 MacBook Pro Y Ⓒ H 201 7 N U S J kJ mol 00 8 M I Energy (kJ/mol) 150 T 100- NIMZAO ✪ 50 What is the heat of reaction for Reaction B? AHxnB = What is the activation energy for Reaction B? K ( - O 9 < O I * ) -C O Reaction progress Reaction B L command ») P . V = : P W ; 242) { option [ SEC e = ? O kJ mol 1 delete retuarrow_forwardLab 6: Chemical Reactions Post-Lab Questions Station V: Heating Cu with Atmospheric O₂ Chemical equation: Complete ionic equation: Net ionic equation: General reaction type: Station VI: Reacting CuSO4 Solution with Steel Wool (Fe)arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill EducationPrinciples of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
- Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill EducationChemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningElementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY