Rate expression for two reaction are : (a) `"rate"_(a) = k_(a)[A]` and (b) `"rate"_(b) = k_(b) [B]^(2)` . When [A] = [B] `= 1 mol l^(-1) , k_(a) = k_(b) mol L^(-1)`. If [A] = [B] = 2 mol `L^(-1)` , write the relation between `"rate"_(a) ` and `"rate"_(b)` .

Explanation

`"Rate"_(a)=k_(a)[2" mol L"^(-1)]`
`"Rate"_(b)=k_(b)["2 mol L"^(-1)]^(2)=k_(1)["2 mol L"^(-1)]^(2)`
The ration of the rates of two reactions (a) and (b) is given as, `("Rate"_(a))/("Rate"_(b))=(k_(a)["2 mol L"^(-1)])/(k_(a)["2 mol L"^(-1)]^(2))=1/2`
The ration of the rates = `1:2`.