For [A] vs. time: y = -0.0154x + 2.2911, R² = 0.9621 For In[A] vs. time: y = -0.0118x + 0.9163, R² = 1 For 1//A] vs. time: y = 0.0102x+ 0.2883, R² - 0.9621 a.) What order is the reaction? How do you know? [A] b.) Find the value of k, including units. c. Find [A) in M at t = 155 seconds.
For [A] vs. time: y = -0.0154x + 2.2911, R² = 0.9621 For In[A] vs. time: y = -0.0118x + 0.9163, R² = 1 For 1//A] vs. time: y = 0.0102x+ 0.2883, R² - 0.9621 a.) What order is the reaction? How do you know? [A] b.) Find the value of k, including units. c. Find [A) in M at t = 155 seconds.
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.52PAE: Hydrogen peroxide (H20i) decomposes into water and oxygen: H,O2(aq) — H,O(f) + ^O2(g) Ordinarily...
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![1.) For the reaction 2A → B,
was collected over two minutes with an initial concentration of [A] = 2.50 and graphed as [A] vs. time, In[A] vs. time, and 1/[A] vs. time. The graphs are ordered left to
right.
[A] vs. Time
In[A] vs. Time
1/[A] vs. Time
3
1
1.8
1.6
2.5
0.8
1.4
0.6
2
1.2
y= -0.0118x + 0.9163
0.4
R=1
1
15
S 0.2
A 0.8
y= 0.0102x +0.2883
1
R = 0.9621
0.6
20
40
60
80
100
120
140
0.4 .
0.5
y= -0.0154x + 2.2911
-0.2
0.2
R- 0.9621
-0.4
20
40
60
80
100
120
140
20
40
60
80
100
120
140
-0.6
Time (s)
Time (s)
Time (s)
For [A] vs. time: y = -0.0154x + 2.2911, R2 = 0.9621
For In[A] vs. time: y = -0.0118x + 0.9163, R² = 1
For 1/[A] vs. time: y = 0.0102x+ 0.2883, R2 = 0.9621
a.) What order is the reaction? How do you know? [A]
b.) Find the value of k, including units.
c.) Find [A] in M at t = 155 seconds.
d.) Calculate the half-life (t1/2), in seconds.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0391c224-9f55-4f56-98d5-4a4656e6fa93%2F6c3b5b2f-c6b0-4e2e-a308-6882c6905f25%2Fuf3tte8_processed.png&w=3840&q=75)
Transcribed Image Text:1.) For the reaction 2A → B,
was collected over two minutes with an initial concentration of [A] = 2.50 and graphed as [A] vs. time, In[A] vs. time, and 1/[A] vs. time. The graphs are ordered left to
right.
[A] vs. Time
In[A] vs. Time
1/[A] vs. Time
3
1
1.8
1.6
2.5
0.8
1.4
0.6
2
1.2
y= -0.0118x + 0.9163
0.4
R=1
1
15
S 0.2
A 0.8
y= 0.0102x +0.2883
1
R = 0.9621
0.6
20
40
60
80
100
120
140
0.4 .
0.5
y= -0.0154x + 2.2911
-0.2
0.2
R- 0.9621
-0.4
20
40
60
80
100
120
140
20
40
60
80
100
120
140
-0.6
Time (s)
Time (s)
Time (s)
For [A] vs. time: y = -0.0154x + 2.2911, R2 = 0.9621
For In[A] vs. time: y = -0.0118x + 0.9163, R² = 1
For 1/[A] vs. time: y = 0.0102x+ 0.2883, R2 = 0.9621
a.) What order is the reaction? How do you know? [A]
b.) Find the value of k, including units.
c.) Find [A] in M at t = 155 seconds.
d.) Calculate the half-life (t1/2), in seconds.
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