# The rate of a gaseous reaction is given by the expression $\mathrm{k}{\left[\mathrm{A}\right]}^{2}{\left[\mathrm{B}\right]}^{3}.$ The volume of the reaction vessel is suddenly reduced to one half of the initial volume. The reaction rate relative to the original rate will be:

1. A

1/24

2. B

1/32

3. C

32

4. D

24

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### Solution:

$\mathrm{Rate}=\mathrm{k}\left[\mathrm{A}{\right]}^{2}\left[\mathrm{B}{\right]}^{3}$
When volume is halved ,the concentration will become double.

$\mathrm{Rate}=32\mathrm{k}\left[\mathrm{A}{\right]}^{2}\left[\mathrm{B}{\right]}^{3}$

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