(a) Determine whether this hydrogen peroxide reaction is first-order or second-order by first calculating the necessary concentration variable for each point (below). In [H₂O₂] 1/[H₂O₂] L/mol Time (min) [H₂O₂] mol/L 0.0200 0.0160 0.0131 0.0106 0.0086 0.0069 0.0056 0.0037 0.0024 0 200 400 600 800 1000 1200 1600 2000 (b) Plot In [H₂O2] vs. time. Attach the graph. (c) Plot 1/[H₂O₂] vs. time. Attach the graph. (d) Write the rate law for this reaction. Explain how you know the order (exponent) for [H₂O₂] in this reaction.

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4. Concentration vs. Time. Determining the Order or a Reaction.
(a) Determine whether this hydrogen peroxide reaction is first-order or second-order by
first calculating the necessary concentration variable for each point (below).
In [H₂O₂]
1/[H₂O₂] L/mol
Time (min) [H₂O₂] mol/L
0
0.0200
200
0.0160
400
0.0131
600
0.0106
800
0.0086
1000
0.0069
1200
0.0056
1600
0.0037
2000
0.0024
(b) Plot In [H₂O₂] vs. time.
Attach the graph.
(c) Plot 1/[H₂O2] vs. time.
Attach the graph.
(d) Write the rate law for this reaction. Explain how you know the order (exponent) for
[H₂O₂] in this reaction.
Transcribed Image Text:4. Concentration vs. Time. Determining the Order or a Reaction. (a) Determine whether this hydrogen peroxide reaction is first-order or second-order by first calculating the necessary concentration variable for each point (below). In [H₂O₂] 1/[H₂O₂] L/mol Time (min) [H₂O₂] mol/L 0 0.0200 200 0.0160 400 0.0131 600 0.0106 800 0.0086 1000 0.0069 1200 0.0056 1600 0.0037 2000 0.0024 (b) Plot In [H₂O₂] vs. time. Attach the graph. (c) Plot 1/[H₂O2] vs. time. Attach the graph. (d) Write the rate law for this reaction. Explain how you know the order (exponent) for [H₂O₂] in this reaction.
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