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CHM 1311 Study Guide - Final Guide: Molar Attenuation Coefficient, Fictitious Force, Ethylenediaminetetraacetic Acid

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redbuffalo440
25 Feb 2015
School
University of Ottawa
Department
Chemistry
Course
CHM 1311
Professor
Wendy Pell

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Document Summary

This experiment deals with the method of using a spectrophotometer in order to obtain and observe the results of a kinetic reaction involving solutions of different ph values for the same reaction. The reaction takes place between chromium nitrate and sodium edta with ph levels of: 4. 0, 4. 5, and 5. 0. As the reaction takes place the colour of the solution changes over time, and can be measured using the spectrophotometer to show how quickly the reaction is progressing. Chemical kinetics is the study and observations of factors the control and affects the rate of a reaction. Although there are many factors that can influence a reaction, the one that will be exposed in this experiment will be concentration of reactants. Concentration of reactants is very important in the rate of the reaction as it directly correlates with the order of the reaction.

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Related Questions

A student studies the kinetics of reaction 1 below using a clock reaction technique, reaction 2, and the procedures given in this experiment. For reaction mixture 1, he measures a time to color change of 121 seconds and for reaction mixture 2, he measures a time of 58 seconds. The temperatures of the reaction mixtures were the same for both experiments.

6I– (aq)+ BrO3– (aq) + 6H+(aq) --> 3I2 (aq) + Br– (aq) + 3H2O(l) (Reaction1,slow)

I2 (aq) + 2 S2O32– (aq) --> 2 I– (aq) + S4O62– (aq) (Reaction 2, fast)

a. Determine the change in concentration of S2O32– that occurred during the time period measured. This should be the same for both the reaction mixtures. First, use M1V1=M2V2 to determine the initial concentration of the S2O32– after mixing the contents of the two flasks but before the reaction begins. Next, find the final concentration of S2O32– by remembering that all the S2O32– is consumed when the color change occurs. You can then find the change in the concentration of S2O32–.

[S2O32–]0 =

∆[S2O32–] =


b. Use the stoichiometry of Reactions 1 and 2 to determine the change in concentration of BrO3– during

the same time period. ∆[BrO3–] =

c. Calculate the initial rate for each reaction mixture. Recall that Rate = − ∆[BrO− ] / ∆t

Rate for mixture 1:

Rate for mixture 2:

d. Method of Initial Rates

Complete the table below using M1V1=M2V2 to find the initial concentration of each reactant after mixing the contents of flasks I and II for both reaction mixtures. Enter the initial rates computed above.

Rxn Mixture [I–]0(M) [BrO3–]0(M) [H+]0 (M) Rate (M/s)

1

2

Use the method of initial rates and the relevant data above to determine the order of reaction 1 with respect to the concentration of iodide ions.

Order with respect to [I–]:_________________________

e. It is critical for the success of this experiment that the concentrations of the reactants I–, BrO3–, and H+ do not change significantly over the time period measured.

Why is this important?

f. By what percent did the bromate ion concentration change during the time period considered for mixture 1 in this experiment?

PercentChange = (|∆[BrO3− ]| / [BrO3− ]0 ) x 100%

Need help with 5. “Calculate molar concentrations of KIO3 and NA2SO3 for solutions A-G” on page 113 please!! Solution #1 (KIO3) and solution #2 (Na2SO3) were both diluted with distilled water to 50mL and mixed together to form solution.....density of KIO3=4.28g/L and Na2SO4=1.01g/L. Thank you!!