Part 4: Let's collect data to try to derive a rate law for a chemical reaction. Put on safety goggles and lab aprons. In this experiment, we will collect data to calculate rate of reaction. If a trial does not go as planned, try again to get good data. You should collect two good runs for each trial (e.g. Trial la and 1b). Trial 1: 1 mL NaHSO3 with 2 mL H2O and 2 mL KIO3 Trial 2: 1 mL NaHSO3 with 3 mL H20 and 1 mL KIO3 Trial 3: 2 mL NaHSO3 with 1 mL H20 and 2 mL KIO3 Trial 4: 2 mL NaHSO3 with 2 mL H20 and 1 mL KIO3 i. ii. iii. In the Data Sheet, write predictions as to which trial your group expects to be the fastest, 2nd place", "3rd place", slowest. Into a small test tube, add the designated mL of 0.015 M NaHSO3 solution. In another test tube, add the designated drops of H20 and 0.010 M KIO3 solution. (Shake tube to mix H20 and KIO3 solution.) You will start timing at the moment that the reactants combine. Stop timing when a distinct color change occurs. We assume that at this point, all of the limiting reactant is used up. When ready, quickly pour the H20/KIO2 into the other test tube and start timing. Calculate the rate of reaction for your trials. Use the change in concentration of NaHSO3. Compare your results to your predictions. Discuss the role of the water in this experiment. iv. V. vi. vii. Names of Group Members: Data Sheet for Part 5 Trial # Predicted Reaction Time Relative Rate (in seconds!) Initial Molarity of KIO3 in reaction test tube Initial Molarity of NaHSO3 in reaction test tube Rate of reaction (M/s) 1 1b 1605 2005 2435 2 26 3lls 3 3b 60s 60s 1346 1125 4 4b viii. Enter your results in class data file. We will use the method of initial rates to calculate the reaction order for your results in lecture