For the reaction A + B `to` products, rate low expression for rate =`k[A][B]^(2)`. If the volume of the vessel is reduced to `1/3` of its original volume then what will be the effect on the rate of reaction?

Explanation

rate = `k[A][B]^(2)`
By reducing the volume to `1/3` of its original volume, the concentration of the reactants will become three times.
`therefore` rate = `k[3A][3B]^(2)=27k[A][B]^(2)` ltbr. Hence, the reaction rate will become 27 times its initial rate.