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Consider the base­catalyzed​reaction OCl­ (aq) + I­ (aq) → OH­ (aq) + Cl­ (aq) Determine the...

Consider the base­catalyzed​reaction OCl­ (aq) + I­ (aq) → OH­ (aq) + Cl­ (aq) Determine the rate law and the rate constant, using the following initial rate data. (Hint: base­catalyzed​indicates that OH ­ affects the rate despite appearing as a product.)

[OCl-] 1.62e-3 1.62e-3 .00271 .00162
[I-] 1.62e-3 2.88e-3 .00162 .0028
[OH-] .52 .52 .84 .91
initil rate m/s .000306 .00054 .000316 .000311

Solutions

Expert Solution

Solution:

Rate law:

Since given given reaction is base catalyzed and concentration of OH- also affects the overall rate.

so we write rate equation :

Rate = k [OCl-]l [I- ]m [ OH-]n

Here k is rate constant , l , m and n are the orders with respect to OCl- , I- , and OH- respectively.

We use given experimental data to find the orders.

Lets number of the experiment.

Lets compare experiment 1 and 2 and use ratio of rate law.

Lets take ln of both side

Now ration of rate 4 and rate 2

Lets find value of n

n = -1

Lets find value of l

We use rate 3 and rate 1

l = 1

Hence the rate law

Rate = k [OCl-] [I- ] [ OH-]-1

Calculation of rate constant:

Lets use rate 1 to get rate constant

k = 60.631

queen_honey_blossom answered 4 hours ago
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