The rate of a gaseous reaction is given by the expression kA2B3. 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:

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

$Rate = 32 k [A]^{2} [B]^{3}$

$32 \times Original rate from . . . . (i)$

The rate of a gaseous reaction is given by the expression $k {[A]}^{2} {[B]}^{3} .$ 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: