A reaction is second order with respect to a reactant. How is the rate of reaction is affected if the concentration of the reactant is i) doubled ii) reduced to half

Explanation

For r reaction `A to` proudcts
Rate `=k [A]^(2)=ka ^(2)`
i) When concentration of A is doubled
i.e., `[A] =2a`
Rate `=k[2a]^(2)=4ka^(2)`
Rate of reaction becomes 4 times,
ii) When concentration of A is reduced to `1/2 i.e., [A]=1/2a`
Rate `=k [(a)/(2)] =1/4 ka^(2)`
Rate of reaction becomes `1/4` timesa i.e reduced to one fourth.