The rate of a reaction of `Br^-` ions with `BrO_3^-` ions in the acidic medium is `rate= k[Br^-][BrO_3^-][H^+]^2`
The order of reaction

When BrO_3^- iron reacts with Br^- in acid medium, Br_2 is liberated. The equivalent mass of Br_2 in this reaction is :

For the reaction : Ester + H^(+) rarr Acid + Alcohol, rate= k [Ester] [H^+]^0 . Find the order of the reaction .

The rate law for the reaction CHCl_3(g) + Cl_2 (g) rarr C Cl_4 + HCI is rate = k [CHCl_3] [Cl_2]^(1//2) . What is the order of reaction ?

The rate law for a reaction is found to be : Rate = k [NO_2^(-) [I^(-)] [H^+]^2 How would the rate of reaction change when concentration of I^- is halved ?

The rate of reaction is equal to rate constant of the reaction. What is the order of reaction?

Write reactions of K_2Cr_2O_7 , in acidic medium with H_2S .

The rate constant of reaction is 3xx10^-3 atm^-2sec^-1 . The order of reaction is

For a reaction: A+ B rarr P , the rate law is given as: Rate = k[A][B]^2 What is the order of reaction if A is present in large excess.

The decomposition of dimethyl ether leads to the formation of CH_4, H_2 and CO and the reaction rate is given by Rate = k [CH_3OCH_3]^(3/2) . The rate of reaction is followed by increase in pressure in a closed vessel, so the rate can also be expressed in terms of the partial pressure of dimethyl ether, i.e., Rate= k (P_(CH_3OCH_3 )^(3/2) If the pressure is measured in bar and time in minutes, then what are the units of rate and rate constants?

A zero order reaction is one in which the rate of reaction: