PARTICIPATIONUse graphs of concentration and time to determine the order and calculate k of reaction.2N₂O5(g) → 4NO₂(g) + O₂(g)Time (s)060012001800240030003600S.Pasishnyk FSW[N₂O5] (M) In[N₂05]0.03650.02740.02060.01570.01170.008600.00640-3.310-3.597-3.882-4.154-4.448-4.756-5.0511/[N₂O5] (M-1)27.436.548.563.785.5116156=openstax™38

To determine: Order of reaction and k

Use graphs of concentration and time to determine the order and calculate k of reaction. 2N₂O5(g) → 4NO₂(g) + O₂(g) Time (s) 0 600 1200 1800 2400 3000 3600 [N₂O] (M) In[N₂05] 0.0365 0.0274 0.0206 0.0157 0.0117 0.00860 0.00640 -3.310 -3.597 -3.882 -4.154 -4.448 -4.756 -5.051 1/[N₂05] (M-1) 27.4 36.5 48.5 63.7 85.5 116 156

Use graphs of concentration and time to determine the order and calculate k of reaction. 2N₂O5(g) → 4NO₂(g) + O₂(g) Time (s) 0 600 1200 1800 2400 3000 3600 [N₂O] (M) In[N₂05] 0.0365 0.0274 0.0206 0.0157 0.0117 0.00860 0.00640 -3.310 -3.597 -3.882 -4.154 -4.448 -4.756 -5.051 1/[N₂05] (M-1) 27.4 36.5 48.5 63.7 85.5 116 156

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

100%

PARTICIPATION
Use graphs of concentration and time to determine the order and calculate k of reaction.
2N₂O5(g) → 4NO₂(g) + O₂(g)
Time (s)
0
600
1200
1800
2400
3000
3600
S.Pasishnyk FSW
[N₂O5] (M) In[N₂05]
0.0365
0.0274
0.0206
0.0157
0.0117
0.00860
0.00640
-3.310
-3.597
-3.882
-4.154
-4.448
-4.756
-5.051
1/[N₂O5] (M-1)
27.4
36.5
48.5
63.7
85.5
116
156
=
openstax™
38

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Step 1: Given Data

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Step 2: Concentration vs Time graph

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Step 3: ln[N2O5] vs time

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Step 4: 1/[N2O5] vs time

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Step 5: Determination of order and rate constant

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