In acidic medium the rate of reaction between {BrO3}– and Br– ions is given by the expression
\(-\frac{\mathrm{d}\left(\mathrm{BrO}_3{ }^{-}\right)}{\mathrm{dt}}=\mathrm{k}\left[\mathrm{BrO}_3^{-}\right]\left[\mathrm{Br}^{-}\right]\left[\mathrm{H}^{+}\right]^2\)
It means
1
Rate constnat of overall reaction is 4 sec-1
2
Rate of reaction is independent of the conc. of acid
3
The cange in pH of the solution will not affect the rate
4
Doubling the conc. of H+ ions will increase the reaction rate by 4 times
5
Question Not Attempted