Heres the table it is referring to, Dont worry about Part E, If anyone can tell
ID: 813683 • Letter: H
Question
Heres the table it is referring to, Dont worry about Part E, If anyone can tell me how to do the first part I can figure it out.
Three data Plots are required for analyzing the data in this experiment, two plots from the kinetic trials outlined in Table 24.1 and one plot from Part E. From each data plot, a value is determined toward the completion of the analysis ae kinetic study for the reaction of I- with H2O2. Complete the table in order to focus the analysis. In the collection of the rate data for the experiment, when do START TIME and STOP TIME occur for each kinetic 'al in Table 24.1? b. What is the color of the solution at STOP TIME? c. What is the chemical reaction that accounts for the color of the solution at STOP TIME In the kinetic analysis of this experiment for the reaction of iodide ion with hydrogen peroxide, state the outpace for h of the following solutions (see Table 24.1): deionized water buffer solution (acetic acid, sodium acetate mixture) I. From the following data plot, calculate the activation energy. Ea, for the reaction.Explanation / Answer
Solution: The above experiment is called the Iodine Clock experiment, in which we have to determine three things:
a) Rate of the reaction for each set of the reaction
b) Coefficients of the reactants in the rate law
c) Order of the reaction and Rate Constant
The reactions involved in the above experiment are:
H2O2(aq) + 2I– (aq) + 2H+ (aq) I2(aq) + 2H2O(l)
and 2S2O32–(aq) + I2(aq) S4O62–(aq) + 2 I– (aq)
This type of reaction is called the iodometric reaction, where firstly the oxidizing agent (H2O2) is added to excess iodide to produce iodine, and the iodine produced is determined by titration with sodium thiosulfate, the method is called "iodometry".
Now, in this experiment, you have your solutions prepared in specific concentrations and taken in specidic volumes say 10 mL of solution A and B. Now, as you mix the two solution, the rule is to START the timer as soon as the Solution A is completely poured into Solution B, and give it ONE swirl. And then leave the solution.
Now, just about 20 - 30 seconds in the reaction time, you can see that the color of the solution starts to turn blue, DO NOT stop the timer yet. The thumb rule is that the color blue will keep on getting darker and darker, so as it reaches its saturation point, according to your eye, STOP the timer. Notice that this is different everytime, so watch carefully. Now the experimental part of the reaction is completed.
Now, you have completed the reaction for a set of Solutions A and B. And you have also drawn Concentration versus time graph for the above sets. You should get a STRAIGHT line in your graph. It may or may not pass through origin. This straight line will give you a slope. The slope for this graph is actually the rate of the reaction.
Now earlier I enlisted a few things,
We have the rate of reaction , now the next thing is to write the RATE LAW of this reaction:
Rate = k[I-]a[OH-]b
Since we know the Rate of the reaction, and we have the concentrations of KI and H2O2 solution, we have a few variables here, that is , coefficients a,b and k (Rate Constant).
Now, notice the Set 8 in the given table, this is called the blank set, as it will give us another value for rate of the reaction, and, so we have two different equations, equating the two equations, this way we can cancel out the term k, and find out the coefficients a and b.
Thus, after finding the coefficients you can find out the Order of the reaction, as well as plug the values of the Coefficients to find the Rate Constant of the reaction.