Map For the following reaction: t (s) H1(M) CH,OH(aq) H+(aq) CI\"(aq) CH3Cl(aq)

Question

Map For the following reaction: t (s) H1(M) CH,OH(aq) H+(aq) CI"(aq) CH3Cl(aq) H2O(l ) -12.10 + + + 27.0 1.88 the value of [H'] was measured over a period of time. Given the data, find the average 65.0 1.76 24.0 1.59 rate of disappearance of H'(aq) for the time interval between each measurement. Interval: 0s to 27.0 s 27.0 s to 65.0s 65.0 s to 124.0s Number Number Number M/s M/ s M/ s What is the average rate of appearance of CH3Cl(aq) for the same time intervals? Interval: Os to 27.0s 27.0 s to 65.0s 65.0 s to 124.0s Number Number Number Reaction rate: M/s

Explanation / Answer

For reactants:

rate of reaction of [A] = -[A]/t

For products = [C]/t

where [A] is reactant concentration and [C] is product conc.

0-27s

-[1.88M - 2.10M]/27s = 0.00813 M/s = 8.13 x 10-3 M/s

27-64s

-[1.76M-1.88M]/[65s-27s] = 0.00316 M/s = 3.16 x 10-3 M/s

65 - 127s

-[1.59M - 1.76M]/[127s-65s] = 0.00274 M/s = 2.74 x 10-3 M/s

Also rate of reaction of other reactants area given in terms of other components of reaction as:

For A reaction:

aA + bB ----->cC + dD

{-[A]/t}/a = {-[B]/t}/b = [C]/t}/c = {[D]/t}/d ------*

here you can see that if you have to find rate of any other reactant say of [B] and you have rate of reaction of [A],

you just have to use equation *

{-[A]/t}/a = {-[B]/t}/b

{-[B]/t} = b x {-[A]/t}/a

similarly as above for our case rate of CH3Cl is same as rate of H+ as :

{[CH3Cl]/t} = 1 x {-[H+]/t}/1

[CH3Cl]/t = -[H+]/t

hence rate will be exactly same as -[H+]/t:

0-27s

=0.00813 M/s = 8.13 x 10-3 M/s

27-64s

= 0.00316 M/s = 3.16 x 10-3 M/s

65 - 127s

= 0.00274 M/s = 2.74 x 10-3 M/s

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