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LB 172L Study Guide - The Exponents, Fast Green Fcf, Taiwanese Units Of Measurement

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School
MSU
Department
Lyman Briggs College
Course
LB 172L
Professor
Maxine Davis

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Document Summary

After doing this lab, you are expected to be able to: Use beers law to determine the concentration of a solute. Determine the rate law of a reaction from time and concentration data. Determine the rate constant to a reaction. Determine concentrations via spectroscopy using beer"s law. Determine the rate law for the reaction between bleach and two dyes. Determine the rate constant for the same reaction. We will be using concentrated bleach which can stain clothes. In this lab, you will be determining how quickly household bleach reacts with a couple of different dyes. In order to be able to understand this, we have to first visit the world of kinetics. Chemical kinetics is the branch of chemistry which is concerned with the study of the rate of chemical reactions. The rate of a reaction is a measure of how quickly reactants are turned into products.

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Related Questions

question d and 2 and part E 1 and 2

Bleach is an aqueous solution of sodium hypochlorite. Above 40°C, the hypochlorite ion will decompose into the chlorate and chloride ions. The results below were measured at 60°C and pH 12.6 to determine the rate law of this decomposition and to identify a possible mechanism.

(a) Write the balanced decomposition reaction of the hypochlorite ion into the chlorate and chloride ions using the smallest integer coefficients. (In this reaction, sodium ions are spectator ions.)

(b) Using the data listed to the left, determine the rate law and the rate constant for this reaction at 60°C with respect to hypochlorite decomposition.

(c) If the initial concentration of hypochlorite is set to 1.100 M, what is the half-life (in min) of the reaction at 60°C.

(d) The activation energy for this reaction is 104 kJ. Estimate the rate constant for this reaction at 50.0°C.

(e) Further experiments suggest that this decomposition follows a two-step mechanism in which the only intermediate is the chlorite ion and the first elementary step is rate-determining. Given your results in part (b), what is this likely two-step mechanism?