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Question

The rate law for the reaction, 2Cl2O2Cl2+O2, at 200oC is found to be: Rate=k[Cl2O]2.
(a) How would the rate change if [Cl2O] is reduced to one-third of its original value?
(b) How should the [Cl2O] be changed in order to double the rate?
(c) How would the rate change if [Cl2O] is raised to threefold of its original value?

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Solution

(a) Rate equation for the reaction,
r=k[Cl2O]2
Let the new rate be rl; so, rl=k[Cl2O3]2=19r
(b) In order to have the rate =2r, let the concentration of Cl2O be x.
So. 2r=kx2 ...(i)
We know that, r=k[Cl2O]2 ...(ii)
Dividing equation (i) by equation (ii),
2rr=kx2k[Cl2O]2
or 2=x2[Cl2O]2
or x2=2[Cl2O]2
or x=2[Cl2O]
(c) New rate =k[3Cl2O]2=9k[Cl2O]2=9r
i.e., nine times of the original rate.

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