Wll be able to use the predictive power eattion, you of the rate law to calculat

Question

Wll be able to use the predictive power eattion, you of the rate law to calculate the half life (ts2) for each process. Procedure: Download the Microsoft Excel file that your instructor has uploaded to Blackboard. Familiarize yourself with the different columns and graphs that are already provided for you. Try plugging some numbers for concentration and time. What happens to the lines on the gra 1) in phs? 2) Let's begin by simulating a simple chemical transformation A B. Start by counting out 15 marshmallows. Each marshmallow represents 1 mole of A. Assume that this reaction occurs in the gas phase and occupies a volume of 0.1 L. 1 mole of A converts into 1 mole of B every 30 seconds. Make a table in the space below of the reaction progress versus time. Track the loss of A and the appearance of B. After you have generated your data table, plot your data (in terms of moles/liter and time) in the Excel spreadsheet provided. What is the order of this reaction? How do you know? What is the value of the rate constant (k)? Write the complete rate law in the space below. A and the appearance of B. After you harve 03 ,-o 0.333 zero order

Explanation / Answer

2. the reaction order is zero because the rate is constant in time.

Rate = - dC/dt = - k            (rate law for 0 order reaction)

Rate = - (1molA/0.1L)/30 s = 0.333 M/s

K= rate = 0.333 M/s

3. rate = 0.333 M/s

for a zero order reaction the rate is constant (it doesn’t depends on the actual concentration).

3.

For a second order reaction

1/C = -kt +1/Co

deltaC

C. mol/L

1/C

t, sec

400

0.0025

0

-80

320

0.003125

30

-50

270

0.003704

60

-40

230

0.004348

90

-25

205

0.004878

120

-15

190

0.005263

150

From the plot 1/C vs t:

1/C = 2x10-5 x t + 0.0025

    k   = 2x10-5 M-1s-1

rate = k[SO2Cl2]2 =

       = 2x10-5 M-1s-1 x (10 M)2 = 2x10-3 M/s

4.

deltaC

C. mol/L

lnC

t, sec

400

5.991465

0

-80

320

5.768321

30

-70

250

5.521461

60

-60

190

5.247024

90

-50

140

4.941642

120

-40

100

4.60517

150

y = - 0.2906x + 6.3792 (from the plot lnC vs t)

For a 1st order reaction

lnC = - kt + lnCo

k = 0.290 s-1

rate = k[A] = 0.290 s-1 x 100 M = 29 M/s

deltaC

C. mol/L

1/C

t, sec

400

0.0025

0

-80

320

0.003125

30

-50

270

0.003704

60

-40

230

0.004348

90

-25

205

0.004878

120

-15

190

0.005263

150

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