For the reaction A →→ products, concentration and time data were collected. Enter these data into the graphing tool and determine the value and units of the rate constant, k, for this reaction. Graphing Tool t k= [A] Add Row 10 total rows In[A] Clear All Data 1/[A] [A] t (min) 0.0 2.0 4.0 6.0 Units of k: [A] vs. t [A] (M) 1.00 0.76 0.52 0.28 In[A] vs. t 1/[A] vs. t

For the reaction A →→ products, concentration and time data were collected. Enter these data into the graphing tool and determine the value and units of the rate constant, k, for this reaction. Graphing Tool t k= [A] Add Row 10 total rows In[A] Clear All Data 1/[A] [A] t (min) 0.0 2.0 4.0 6.0 Units of k: [A] vs. t [A] (M) 1.00 0.76 0.52 0.28 In[A] vs. t 1/[A] vs. t

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter13: Kinetic Methods

Section: Chapter Questions

Problem 9P

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The initial rate for a reaction is equal to the slope of the tangent line at t 0 in a plot of [A] versus time. From calculus, initial rate = d[A]dt . Therefore. the differential rate law for a reaction is Rate = d[A]dt=k[A]n. Assuming you have some calculus in your background, derive the zero-, first-, and second-order integrated rate laws using the differential rate law.
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