The rate constant for an isomerisation reaction, `ArarrB " is " 4.5xx10^(-3)"min"^(-1).` If the initial concentration of A is 1(M), calculate the rate of the reaction after 1 h.

Explanation

The unit of rate constant is `"min"^(-1)` , implying that the reaction is first order.
For a first order reaction `k=(2.303)/(t)log.(a)/(a-x)`
or, `k=(2.303)/(t)log.([A]_(0))/([A]) " or, " 4.5xx10^(-3)=(2.303)/(60)log.(1)/([A])`
Hence , the concentration of A after 1 h , [A] = 0.7634 (M)
`therefore` The reaction -rate after 1 h `=k[A]=4.5xx10^(-3)xx0.7634`
=`3.435xx10^(-3)"mol.L"^(-1)."min"^(-1)`