Trial [A] (M) Rate (s\') k (specific units) average k (specific units) 1 .0250 .

Question

Trial         [A] (M)           Rate (s')            k (specific units)            average k (specific units)

1              .0250            .0653

2              .0125            .0163

3              .06625          .00408

Equation 5 for question 6:

   Rate' = 1/ time = k' [A] ^m

TRACS : CHEM 1142 Lab Sp |Week 2 Kinetics of Iodine Cl Kinetics of lodine Clock Selected Prelab answers Drc | + tracs.txstate.edu/access/content/group/3ae 14449-2cc6-4797-a 149-1 ddd5c1 ac5a9/Week%204%3A%20%20ki netics%20of%20the%; U N Netflix P Pandora Internet TRACS (2) OneDrive Physical Therapy TX STATE LOGIN BE Grade Calculator Applicant Status Bobcat Mail Chemistry Hw GChegg Data Table 3: Average k (specify units) ria Rate (s) (specify units) 5. Consider the data compiled in Data Table 3. Find the order of the reaction with respect to KI. Briefly justify your answer, either in words or with math 6, write the rate law for the reaction based only on A using the order you found in #5. Leave the rate constant as k. (see Equation 5) 7. Solve for the rate constant for all 3 trials in Data Table 3 using the rate law you wrote in #6. Record your k values with units in Data Table 3. Find the average value of the rate constant, and record in Data Table 3. (Note that since we are using a pseudo-rate law and pseudo-rate constant, the units of your rate constant will not match what they should be from lecture. For instance, for a true rate constant for a fourth order reaction, the units should be Ms. However, with our pseudo-rate law, those are not the units you would get if you decide the reaction is fourth order. Use the units that fall out naturally from our pseudo-rate law; not the units that you "should" get for that order of reaction with a true rate law.) 12:23 PM 2/17/2016

Explanation / Answer

7)

rate=k[A]

So k=rate/[A]

using this formula, completing the table

Trial         [A] (M)           Rate (s')            k (specific units)            average k (specific units)

1              .0250            .0653 2.612

2              .0125            .0163 1.304 1.326

3              .06625          .00408 0.0616

6)

units of rate constant= s-1/mol L-1 = L/( mol s)

rate law:

rate= k[A]

5)

order:

when [A] is decreasing by 2 factor(from data 1 to 2 in table), rate is decreasing four times. Same is the case from 2 ->3.

So order= 2

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