Lab 3. Kinetics of lodine Clock Reaction 1. Consider the following balanced chem

Question

Lab 3. Kinetics of lodine Clock Reaction 1. Consider the following balanced chemical reaction of potassium iodide and potassium persulfate; From this equation, can the rate law for the reaction be written as follows? Explain why or why not (reactants) (products) Rate-kITTsO In the lodine Clock Reaction experiment, the activation energy for the reaction can be determined from the Arrhenius equation In(k)- InA - Ea/RT. Use the following data to 2. the activation energy (Ea), R-8.31 J/mol-K for the reaction. Show all work. (10) Lab 4. Introducing Equilibrium Methyl orange indicator was used in the chromate ion equilibrium illustrated below. Explain what changes would be observed in this reaction upon the addition of sulfuric acid. 1. 2 Cro42(aq, yellow) + 2H30'(aq)Cro-(aq, orange) + 3 HJX1)

Explanation / Answer

Ans 1 :

The rate law expression is determined experimentally , which relates the concentration or the pressures of reactants in a reaction to the rate of reaction.

The concentrations are usually raised to the power of their stoichiometric coeffecients as determined by the balanced chemical reaction.

So here the rate law : rate = k[I-]3[S2O82-]1 , is written appropriately , as the powers of the reactant concentrations are same as their stochiometric coefficients in the reaction.

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