Practicing Success
In acidic medium the rate of reaction between BrO3- and Br- ions is given by the expression: -\(\frac{d(BrO_3^-)}{dt}\) = k[BrO3-][Br-][H+]2 Which of the following is indicated by the above expression? |
Rate constant of overall reaction is 4 s-1 . The change in pH of solution will not affect the rate. Rate of reaction is independent. Doubling the concentration of H+ ions will increase the reaction rate by 4 times. |
Doubling the concentration of H+ ions will increase the reaction rate by 4 times. |
As rate of reaction is given by = -\(\frac{d(BrO_3^-)}{dt}\) = k[BrO3-][Br-][H+]2 it shows that rate of reaction is of 2nd order with respect to H+. Hence, Doubling the concentration of H+ ions will increase the reaction rate by 4 times. |