Determine the rate law for the oxidation of iodine ion to elemental iodine by br

Question

Determine the rate law for the oxidation of iodine ion to elemental iodine by bromate ion in acid aqueous solution using a method of initial rates at room temperature the energy of activation of the reaction will be determined by measuring the rate constant at three temperatures and buying the arrhenius equation
(PLEASE SHOW WORK) EXPERIMENT 4: Chemical Kinetics The lodine Clock Reaction OBJECTIVE The objectives of this experiment are to determine the rate law for the oxidation of iodide ion to elemental iodine by bromate ion in acid aqueous solution using the method of initial rates at room temperature. The energy of activation of the reaction will be determined by measuring the rate constant at three temperatures and applying the Arrhenius equation. This experiment is to be done in two-student teams. INTRODUCTION The Method of Initial Rates In this experiment, you will determine the rate law of a reaction using the method of initial rates. The reaction you will study is the oxidation of iodide ion to elemental iodine by bromate ion in acid aqueous solution: 6 rag) + BrO3Taq) + 6 H30+ (aq) 3 2 (aq) + Br(aq) + 9 H20() The reactants are the iodide ion, the bromate ion, and the hydronium ion. The products are elemental iodine, bromide ion, and water. The rate of the reaction can be expressed in terms of the concentrations of any of the reactants or products. For example: rate - rate of loss of BroBrO1 At (rate of formation of 12)1-141 rate 3 At For most reactions, the rate of reaction depends only on the concentration of reactants, not on the concentration of products. We assume that the rate law takes the form:

Explanation / Answer

Solution:

First of all we have to calculate Rate law for oxidation of iodide ion to elemental iodine using bromate ion by

initial rate method.

So reaction for the above statement is:

6I-(aq) + BrO3-(aq) + H3O+(aq) -------------------->3I2 (aq)+ Br-(aq) + 9H2O(l)

The rate law for this reaction is

Rate=K[I-]m[BrO3-]n[H3O+]p

Initial Rate law is used for reaction having more than one reactant.Different Experiment are performed and

R0 is measured.In next experiment one reactant kept at same concentration while other varie.

The order of reactant concentration in the rate law can be determined by obserbing how the reaction rate

varies with the varies of reactant. This method is repeated for each reactant until all the orders are determined.

At that point, the rate law can be used to find the value of k for each trial.

For Example

Rate1=K[I-]1m[BrO3-]n[H3O+]p

Rate2=K[I-]2m[BrO3-]n[H3O+]p

Keeping all the reactant concentration same we are changing concentration of iodine ion.

To calculate order m,divide both reaction eqution we will get

Rate1/Rate2=[I-]1m/[I-]2m

Taking ln both side we will get

lnRate1/Rate2=ln[I-]1m/[I-]2m

m=ln(Rate1/Rate2/)ln[I-]1/[I-]2

Solution:Arhenius equation

Reaction rate constant = k = A e-Ea/RT

By taking ln both side we will get

lnk=lnA e-Ea/RT

lnk=lnA + lne-Ea/RT=lnA - Ea/RT

By plotting graph between lnk and 1/T we can calculate activation energy.

NOTE=SINCE YOU HAVE NOTE PROVIDED ANY EXPERIMENTAL VALUE SO I HAVE JUST SHOWN

YOU THEORITICAL PART.

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