A reactions is of second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is reduced to half?

Explanation

For a hypothetical reaction of second order:
`2A to `Products
Rate ( r) =`k[A]^(2)`
When the concentration of reactant is reduced to half.
` Rate(r^('))= k[A/2]^(2)`
`r^(')/r=([A/2])^(2)/([A]^(2))=1/4` or `r^(')=r/4`
The rate of reaction becomes `1/4` of the initial rate.