Hydrogen Peroxide and Iodide Kinetics Essay

(Be sure to maintain references for some(prenominal) cited look on at the end of this report. Additionally, all report secular must be in INK pencil or white out will render the work ineligible for mark appeal)1.What observations and conclusions give the bounce you stock about for each one of the three answers that occurred in the test tubes where you combined green iodide, KI, and hydrogen peroxide, H2O2 (in part 1) of the experiment? (Give a detailed account statement of any observations that you made, i.e., what made the colour change, what answers happened?) upshot2.Use the randomness below to develop the obligatory calculations for the prize of reaction from the resultant roles in part B of the experiment enter the initial molarity of iodide ion in each of the solutions, once your solutions are mixed. commend The KI stock solution submerging was know , and you determinationd a specific volume of the solution, -. However, at the start of the reaction you mu st bank bill for the fact that the aggregate volume of each solution was 200 mL. practise front the initial molarity of the hydrogen peroxide in each of your solutions, once the solutions have been mixed. Remember The H2O2 stock solution concentration was cognize , and you apply a specific volume of the solution, . However, at the start of the reaction you must account for the fact that the total volume of each solution was 200 mL.ANSWERCalculate the number of moles of sodium thiosulfate, Na2S2O3, that was initially usher in in each solution. Remember The Na2S2O3 stock solution concentration was known and you used a specific volume of the solution, . This information is used to conciliate the number of moles.ANSWERBalance the reaction that occurred in each of the solutions. adduce to Eq. 1, 3, and 4 in the research laboratory instructions for the components that are involved.ANSWERCalculate the number of moles of hydrogen peroxide that has reacted Note You will need to use st oichiometry to ascertain this. ANSWERCalculate the change in concentration of hydrogen peroxide in each case, i.e., moles of H2O2 reacted per litre of solution. Hint Recall the total volume, and you have calculated the number of moles that reacted, previously.ANSWERCalculate the put of the reaction, which is simply the change in concentration of H2O2 (calculated above) divided by the time it took for the reaction to complete. i.e., the numbers of moles per litre of peroxide consumed divided by the number of seconds necessitate to react completely.ANSWERComplete the table below you discharge manually do the calculations to fill all of the cells, or it is possible to use a spreadsheet platform to calculate the jimmys. (RECOMMENDED) The process you have used above can be repeated to provide the honours for each of the entries in the table.ANSWER3.Use the following steps to calculate the values of a and b as described in the lab procedure (under the heading The rate practice o f law and our process for obtaining a, b, and k.) In the solutions A, B and C, the concentration of hydrogen peroxide used was the same. Therefore, these solutions are a suitable series for an examination of the dependence of the rate of reaction on the concentration of the iodide ion. Similarly, solutions C, D, and E have the same concentration of iodide ion.Therefore, those solutions can be used to examine the dependence of the rate of reaction on the concentration of hydrogen peroxide. Recalling Eq. 5 Eq. 7 in the laboratory instructions, by plotting ln(rate) against lnI-, using selective information from solutions A, B, and C, we can determine the value of a for this reaction. Similarly, by preparing a plot of ln(rate) against lnH2O2 using the data from solutions C, D and E, we can evaluate b for this reaction. See the laboratory instructions near Eq. 5-7 for an explanation of how a and b can be determined from the slopes of the straight breeds of best-fit that should be obtai ned using the experimental data-points.Graph 1 Plot ln(rate) against lnI- using the data from the table for solutions A, B, and C. Add the best-fit straight frontier through your experimental points and determine the slope of this draw in. This is best accomplished by using a spreadsheet program to generate the graphs, and adding a regression line or trendline with the equation for the line displayed. The value of the slope from this line will be the value of b (as shown in equation 6 of the lab manual). Remember the lowest value of b should be integer or half-integer.ANSWERGraph 2 Plot ln(rate) against lnH2O2 using the data from the table for solutions C, D, and E. Add the best-fit straight line through your experimental points and determine the slope of this line. This is best accomplished by using a spreadsheet program to generate the graphs, and adding a regression line or trendline with the equation for the line displayed. The value of the slope of this line is the value of a (as shown in Equation 7 of the lab manual). Remember the final value of a should be integer or half-integer.ANSWER4.Using Equation 2 of the lab manual, calculate the values of k (at room temperature) for each reaction trial you performed, using your values of a, b, and the rate and concentration information in the table. You should end up with 5 values of k, for the five trials that you performed at room temperature.ANSWERCalculate the average value of k. Use this value of k, and the values of a and b to write out the general rate law for the reaction, (see Eq. 2).ANSWER5.Using the rate of reaction for solution A at room temperature, and the rate of the reaction at elevated temperature, use Eq. 10 from the lab procedure to calculate the activation energy, Ea. (Note pay attention to the units of the shove along constant, R)